I have two Blood parrots in a 20 gallon tank, The 20 gallon tank has a ph of 6.2.
4 weeks ago i bought a new 38 gallon tank for the blood parrots.
I havent yet moved the blood parrots to the new tank because i wanted to wait until it went through its nitrogen cycle first.
I just tested the water in the new tank in which showed ammonia at 0, nitrite at 0 and nitrates at 5, Therefore i assume the tank is now cycled.
The only thing that concerns me about moving the blood parrots is that the new tank has a ph of 7.2.
How dangerous will it be for the fish to go from a sudden ph change of 6.2 to 7.2?
Any advice?Ph difference in new tank.?
That is large pH difference and can kill you fish from pH shock if not properly acclimated.
With such a large pH difference, I would suggest using the drip method to acclimate your fish. Put him a bucket of water from the old tank. The using a air hose, suck in the water. Then using the valve, adjust till such that it water is now dripping on drop every 10 or 20 second. When the bucket in full throw half of it away and repeat the process. After about 30 minutes you can put the fish in the new tank.
Tuesday, May 31, 2011
How do salts affect pH of a solution?
I am a planted aquarium enthusiast and am curious about how certain salts, when used as fertilizers, will affect pH. (Beware, the extent of my chemistry knowledge is what I half remember from high school, combined with a little reading I have done to research this.)
Take, for example, the salt Ca(NO3)2. According to what I have read, the pH of a salt depends on the relative acidity and “baseness” (whatever the term is) of the acid and base that combined to form the salt. So in this case would it be nitric acid and calcium peroxide? Or are there different ones that would work? What are the pH values for these?
Also I have read that the reason that the end result salt affects pH (in those cases where it does) is because part of the salt in solution reacts with water, splitting it, which is the mechanism behind the pH change. The site that I was reading provided tables of ions that react with water and ones that do not. Ca +2 and (NO3) –1 were ions that they said tended to not react with water; so is this to say that calcium nitrate will not affect pH?
And some final questions – What happens when one ion is depleted from water faster than the other. Plants use much more NO3 than Ca, plus I would expect a small continuous loss of NO3 from the aquarium through the activity of denitrifying bacteria forming N2 gas. This is preventable since I can add other sources of N, I am just curious about what happens when calcium ions accumulate. Would that affect pH? I have read that adding solid calcium and/or quick lime to water will form a caustic solution of Ca(OH)2; will the Ca ions from Ca(NO3)2 do something similar at a certain point?
For reference, the link to the site I used is http://www.science.uwaterloo.ca/~cchieh/cact/c123/salts.html
Please help, chemistry experts!How do salts affect pH of a solution?
That site is accurate, as far as I can see. Salts are composed of two parts (two ions). If you have a salt that's composed of two ';neutral'; ions, it will not have an impact on the pH of your aquarium. Also note that salts containing one ';acid'; ion and one ';base'; ion will -approximately- cancel each other out and leave the water at the same pH, though if you need a very particular pH, I would advise against doing this (since one ion might be stronger and predominate).
Your understanding of how this works is also correct. When added to water, salts dissociate, which means they fall apart into their two constituent ions (a cation, the positively charged one, and an anion, the negatively charged one). Depending on the acid-base chemistry of these ions, they may or may not react with the water itself to produce acids and bases. In your example, the nitrate ion (NO3 1-) that's formed would need to form nitric acid (HNO3) if it were to react with water. However, nitric acid really doesn't like existing in water, and tends not to spontaneously form, which means the NO3 ion is inert. Calcium is the same: it really tends not to mess with water molecules, which means this salt will indeed not affect pH of the water it's added to.
However, if you take, for example, sodium acetate (NaCH3COO, the salt that's formed when you react vinegar and baking soda), it will dissociate into a sodium cation (Na 1+) and an acetate anion (CH3COO 1-). The sodium ion does nothing to water, but the acetate ion will tend to rip hydrogen off water molecules, forming acetic acid (vinegar) and hydroxide, in the following reaction:
CH3COO 1- + H2O ---%26gt; CH3COOH + OH 1-
This only occurs with about 5% of the acetate ions, but it's enough to change the pH. The free hydroxide (OH 1-) will make the solution slightly basic (yes: the formation of an acid makes the solution basic. It's counter-intuitive, but it's due to the nature of acid-base chemistry, and it does make sense).
By the way, the word for ';baseness'; is ';alkalinity';.
Unfortunately, I'm more of an organic chemistry person than an inorganic chemistry person, so I can't really help you with your second question. Perhaps someone else can shed light on that. I can, however, tell you that water with high calcium ion concentrations is refered to as ';hard water'; (as opposed to ';soft water';). I know nothing about aquariums, but perhaps you can look around online for problems involving hard water and see if any other aquarium-savvy people know if that causes a problem and how to fix it.
Cheers!
PyeHow do salts affect pH of a solution?
You must be kidding. Salt is a building block to acid. Of course it will alter it towards acidity. You can counter it by putting cloride or baking soda in it. That should neutralize it or bring it back to it's previous state. (Use same amount as salt exactly or it will become too base.)
Take, for example, the salt Ca(NO3)2. According to what I have read, the pH of a salt depends on the relative acidity and “baseness” (whatever the term is) of the acid and base that combined to form the salt. So in this case would it be nitric acid and calcium peroxide? Or are there different ones that would work? What are the pH values for these?
Also I have read that the reason that the end result salt affects pH (in those cases where it does) is because part of the salt in solution reacts with water, splitting it, which is the mechanism behind the pH change. The site that I was reading provided tables of ions that react with water and ones that do not. Ca +2 and (NO3) –1 were ions that they said tended to not react with water; so is this to say that calcium nitrate will not affect pH?
And some final questions – What happens when one ion is depleted from water faster than the other. Plants use much more NO3 than Ca, plus I would expect a small continuous loss of NO3 from the aquarium through the activity of denitrifying bacteria forming N2 gas. This is preventable since I can add other sources of N, I am just curious about what happens when calcium ions accumulate. Would that affect pH? I have read that adding solid calcium and/or quick lime to water will form a caustic solution of Ca(OH)2; will the Ca ions from Ca(NO3)2 do something similar at a certain point?
For reference, the link to the site I used is http://www.science.uwaterloo.ca/~cchieh/cact/c123/salts.html
Please help, chemistry experts!How do salts affect pH of a solution?
That site is accurate, as far as I can see. Salts are composed of two parts (two ions). If you have a salt that's composed of two ';neutral'; ions, it will not have an impact on the pH of your aquarium. Also note that salts containing one ';acid'; ion and one ';base'; ion will -approximately- cancel each other out and leave the water at the same pH, though if you need a very particular pH, I would advise against doing this (since one ion might be stronger and predominate).
Your understanding of how this works is also correct. When added to water, salts dissociate, which means they fall apart into their two constituent ions (a cation, the positively charged one, and an anion, the negatively charged one). Depending on the acid-base chemistry of these ions, they may or may not react with the water itself to produce acids and bases. In your example, the nitrate ion (NO3 1-) that's formed would need to form nitric acid (HNO3) if it were to react with water. However, nitric acid really doesn't like existing in water, and tends not to spontaneously form, which means the NO3 ion is inert. Calcium is the same: it really tends not to mess with water molecules, which means this salt will indeed not affect pH of the water it's added to.
However, if you take, for example, sodium acetate (NaCH3COO, the salt that's formed when you react vinegar and baking soda), it will dissociate into a sodium cation (Na 1+) and an acetate anion (CH3COO 1-). The sodium ion does nothing to water, but the acetate ion will tend to rip hydrogen off water molecules, forming acetic acid (vinegar) and hydroxide, in the following reaction:
CH3COO 1- + H2O ---%26gt; CH3COOH + OH 1-
This only occurs with about 5% of the acetate ions, but it's enough to change the pH. The free hydroxide (OH 1-) will make the solution slightly basic (yes: the formation of an acid makes the solution basic. It's counter-intuitive, but it's due to the nature of acid-base chemistry, and it does make sense).
By the way, the word for ';baseness'; is ';alkalinity';.
Unfortunately, I'm more of an organic chemistry person than an inorganic chemistry person, so I can't really help you with your second question. Perhaps someone else can shed light on that. I can, however, tell you that water with high calcium ion concentrations is refered to as ';hard water'; (as opposed to ';soft water';). I know nothing about aquariums, but perhaps you can look around online for problems involving hard water and see if any other aquarium-savvy people know if that causes a problem and how to fix it.
Cheers!
PyeHow do salts affect pH of a solution?
You must be kidding. Salt is a building block to acid. Of course it will alter it towards acidity. You can counter it by putting cloride or baking soda in it. That should neutralize it or bring it back to it's previous state. (Use same amount as salt exactly or it will become too base.)
Can anyone explain? ';For maximum buffer capacity, pH=pKa';?
I understand that this is because the concentration of the salt and acid are equal, but how does this make buffer capacity maximum? Wouldn't a solution with a higher salt concentration be able to better resist pH changes if H+ is added? (Or a solution with more acid resisting pH changes better if OH- is added)Can anyone explain? ';For maximum buffer capacity, pH=pKa';?
Max buffer capacity means that it resists change in pH the most. Look up the buffer titration curve. When you have equal H-salt and salt-, you are at a flattest part of the curve, meaning if you add OH- or H+, your solution will resist pH changes the most.
Max buffer capacity means that it resists change in pH the most. Look up the buffer titration curve. When you have equal H-salt and salt-, you are at a flattest part of the curve, meaning if you add OH- or H+, your solution will resist pH changes the most.
If my tank's pH seems to stay at a low lvl (6.2-6.4), how do I acclimate new fish from a fish store?
I have a 3month old 10gallon freshwater tank. It's my first tank and I've just been doing what the guys at the local ';boutique'; fish store have told me to do. I do weekly 25% water change, use Neutral regulator, add some salt (but not too much), Amquel water conditioner. At first I also used distilled water but then after a month used tap water (which has a pH of 7-7.2). Maybe my problems with my low pH are due to general hardness or alkalinity, but in any case I can't seem to keep my pH higher than 6.4. I'm not neglecting anything... Last Saturday the tropical fish store even gave me some kind of saltwater powder stuff that they said was SURE to get my pH up. Nope. They also gave me a rock that i believe is some kind of carbonate rock. They say all my other stats are fine (ie Ammonia, nitrates, nitrites)
Through all my trolling in fish forums it looks like I could just let the pH remain low and just let fish adapt to it. So the question is... can I put the new fish in a little bowl (i could add a bubbler) and slowly add my tank's water to it? They say sudden pH changes is the worst for fish... how am I ever gonna add new fish if the store's pH is closer to 7.0-7.2?
btw, I had a swordtail, red wag platy, 5 tetras, and a tiny bottom feeder(forget name)... I am now down to just one neon tetra. Heh, I bought the tank so I could watch fish.... not water with a rocks! lolIf my tank's pH seems to stay at a low lvl (6.2-6.4), how do I acclimate new fish from a fish store?
Your natural water may in fact have a low Ph most water companies buffer the water for the pallet, this buffer generally breaks down after 24hrs, you can find this out by storing some tap water for 24hrs and testing the Ph then do it again after another 24hrs to see the difference.
Trying to adjust the Ph in an aquarium is not something I do on a regular basis, when I had a fish house and required different Ph's I would use the likes of Peat moss to lower or carbonate substances in the filtration system, Of course I had various filtration units that I could use and generally used a external canister system.
The Ph you have is fairly suitable for all south american fish which given your tank size would be your best bet.
When you buy your fish, I'd float the bag to match the temp then every 10 Min's let some of the water from the tank into the bag, just a small amount do this until the bag is on the verge of sinking then net the fish out and allow them into the tank, this should be sufficient to acclimatize the fish to the Ph.
The fish shops water sounds as if is being replaced quicker than the breakdown of the buffer if that's the source. I would stop using artificial additives to the tank as this will only solve the problem in the short term and will have a detrimental effect on the likes of Neon Tetras as they would be more comfortable at the 6.2/6.5 range anyway.If my tank's pH seems to stay at a low lvl (6.2-6.4), how do I acclimate new fish from a fish store?
Here's what I would do, change your water about half way, fill with clean water, add a air/bubble stone (bigger the better) then change out or rinse out your filters good. then leave the pump on and let the water settle. You should be fine.
I would put some plants in the tank it helps control ph I have a 55 gallon and i had the same issue the more plants the better off your tank will be. Also when you check you water check your tap water to see what the ph is and there are some fish that can tolerate a low ph. Ask your local pet store about what fish but i would try the plants and give it about a week to see if that helps. Good look
Through all my trolling in fish forums it looks like I could just let the pH remain low and just let fish adapt to it. So the question is... can I put the new fish in a little bowl (i could add a bubbler) and slowly add my tank's water to it? They say sudden pH changes is the worst for fish... how am I ever gonna add new fish if the store's pH is closer to 7.0-7.2?
btw, I had a swordtail, red wag platy, 5 tetras, and a tiny bottom feeder(forget name)... I am now down to just one neon tetra. Heh, I bought the tank so I could watch fish.... not water with a rocks! lolIf my tank's pH seems to stay at a low lvl (6.2-6.4), how do I acclimate new fish from a fish store?
Your natural water may in fact have a low Ph most water companies buffer the water for the pallet, this buffer generally breaks down after 24hrs, you can find this out by storing some tap water for 24hrs and testing the Ph then do it again after another 24hrs to see the difference.
Trying to adjust the Ph in an aquarium is not something I do on a regular basis, when I had a fish house and required different Ph's I would use the likes of Peat moss to lower or carbonate substances in the filtration system, Of course I had various filtration units that I could use and generally used a external canister system.
The Ph you have is fairly suitable for all south american fish which given your tank size would be your best bet.
When you buy your fish, I'd float the bag to match the temp then every 10 Min's let some of the water from the tank into the bag, just a small amount do this until the bag is on the verge of sinking then net the fish out and allow them into the tank, this should be sufficient to acclimatize the fish to the Ph.
The fish shops water sounds as if is being replaced quicker than the breakdown of the buffer if that's the source. I would stop using artificial additives to the tank as this will only solve the problem in the short term and will have a detrimental effect on the likes of Neon Tetras as they would be more comfortable at the 6.2/6.5 range anyway.If my tank's pH seems to stay at a low lvl (6.2-6.4), how do I acclimate new fish from a fish store?
Here's what I would do, change your water about half way, fill with clean water, add a air/bubble stone (bigger the better) then change out or rinse out your filters good. then leave the pump on and let the water settle. You should be fine.
I would put some plants in the tank it helps control ph I have a 55 gallon and i had the same issue the more plants the better off your tank will be. Also when you check you water check your tap water to see what the ph is and there are some fish that can tolerate a low ph. Ask your local pet store about what fish but i would try the plants and give it about a week to see if that helps. Good look
PH Questions for biology?
1. If the pH of a sample was 3 how many times more acidic is it than a solution with a pH of 6?
2. How might one correct the pH of a lake with a reading of 3?
3. What is the pH of human skin?
4. How does non-tearing shampoo work?
5. What is the pH of rain water?
6. What local industries pump materials into the atmosphere to create a drastic pH change in rain water?
Please answer correctly with detail thank you so much if u do !! =]PH Questions for biology?
1. 1000 times
2 This is very, very acidic, so a lot of damage would have been done. Add limestone.
3 Maybe 5.5
4 Probably has a pH of about 7.
5 Varies between maybe 5.5 and 7.5 if it is not polluted.
6 Coal burning facilities, if there is sulphur in the coal.web design company flatron lcd monitor
2. How might one correct the pH of a lake with a reading of 3?
3. What is the pH of human skin?
4. How does non-tearing shampoo work?
5. What is the pH of rain water?
6. What local industries pump materials into the atmosphere to create a drastic pH change in rain water?
Please answer correctly with detail thank you so much if u do !! =]PH Questions for biology?
1. 1000 times
2 This is very, very acidic, so a lot of damage would have been done. Add limestone.
3 Maybe 5.5
4 Probably has a pH of about 7.
5 Varies between maybe 5.5 and 7.5 if it is not polluted.
6 Coal burning facilities, if there is sulphur in the coal.
How is the pH level affected of a substance when it is mixed with a acid, base, or neutral?
I tried to mix diffrent acids and bases as well as neutral water with vinegar an acid to see how it would affect the vinegars pH level. The pH level did change when i mixed the other substance but i don't understand the pattern. Why did the pH level change, and why only a specific amount?How is the pH level affected of a substance when it is mixed with a acid, base, or neutral?
Not sure how in depth of an answer you are looking for?
Assuming water is 7, adding acid will lower the pH. Adding a base will increase the pH.
The amount that changes is based on the concentration (and reactivity) of acids and bases.
Molar/Molal concentrations will affect this as well, since a more concentrated, stronger acid/base will affect total PH more than a weaker reagent.
Also, the total volume of liquid affects the concentration as well.
Free hydrogen is acidic
Free hydroxide is basic
Since water is H20, things that react in water to make excess free hydrogen or peroxide react as above too.
Not sure how in depth of an answer you are looking for?
Assuming water is 7, adding acid will lower the pH. Adding a base will increase the pH.
The amount that changes is based on the concentration (and reactivity) of acids and bases.
Molar/Molal concentrations will affect this as well, since a more concentrated, stronger acid/base will affect total PH more than a weaker reagent.
Also, the total volume of liquid affects the concentration as well.
Free hydrogen is acidic
Free hydroxide is basic
Since water is H20, things that react in water to make excess free hydrogen or peroxide react as above too.
Lab calculations please help immediately!?
I WILL RATE YOU 10 POINTS IF YOU SHOW ME HOW TO DO THIS:
For Part A: Undiluted BUffers there are three Buffers: A, B, and C
ADD HCl:
Buffer A: pH of original buffer solutions is 10.09
Volume of .100 M HCl to change pH by 1.0: .15 mL
Final pH: 9.06
Buffer B:
pH of original buffer solutions: 9.01
Volume of .100M HCl to change pH by 1.0: .15mL
Final pH: 8.07
Buffer C:
pH of original buffer: 9.09
Volume of .100 M HCl to change pH by 1.0: .63mL
final pH: 8.18
ADD NaOH:
Buffer A:
pH of original buffer solutions: 11.08
volume of .100M NaOH to change pH by 1.0 :.42mL
final pH: 12.16
Buffer B:
pH of original: 10.67
volume of .100 M NaOH change pH by 1.0: .34mL
final pH: 11.73
Buffer C:
pH original: 8.47
Volume of .100M NaOH: .26 mL
final pH:9.54
PART B: DILUTED BUFFERS
ADD HCl, same # moles as Part A:
BUFFER A:
pH of original: 10.04
Volume of .100 M HCl to change pH by 1.0: .075mL
final pH: 8.85
BUFFER B:
pH original: 8.84
volume HCl: .16mL
final pH: 1.99
ADD NaOH, same # of molLab calculations please help immediately!?
yeah right
For Part A: Undiluted BUffers there are three Buffers: A, B, and C
ADD HCl:
Buffer A: pH of original buffer solutions is 10.09
Volume of .100 M HCl to change pH by 1.0: .15 mL
Final pH: 9.06
Buffer B:
pH of original buffer solutions: 9.01
Volume of .100M HCl to change pH by 1.0: .15mL
Final pH: 8.07
Buffer C:
pH of original buffer: 9.09
Volume of .100 M HCl to change pH by 1.0: .63mL
final pH: 8.18
ADD NaOH:
Buffer A:
pH of original buffer solutions: 11.08
volume of .100M NaOH to change pH by 1.0 :.42mL
final pH: 12.16
Buffer B:
pH of original: 10.67
volume of .100 M NaOH change pH by 1.0: .34mL
final pH: 11.73
Buffer C:
pH original: 8.47
Volume of .100M NaOH: .26 mL
final pH:9.54
PART B: DILUTED BUFFERS
ADD HCl, same # moles as Part A:
BUFFER A:
pH of original: 10.04
Volume of .100 M HCl to change pH by 1.0: .075mL
final pH: 8.85
BUFFER B:
pH original: 8.84
volume HCl: .16mL
final pH: 1.99
ADD NaOH, same # of molLab calculations please help immediately!?
yeah right
PH please help?
A beaker with 195ml of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.1M . A student adds 8.90ml of a 0.410 M solution to the beaker. How much will the pH change? The PKa of acetic acid is 4.76.PH please help?
You need to give more information, as in 8.90 ml of a 0.410 M solution of what type of solution to the beaker.PH please help?
ew chemistry and math problems dont you just hate those haha
You need to give more information, as in 8.90 ml of a 0.410 M solution of what type of solution to the beaker.PH please help?
ew chemistry and math problems dont you just hate those haha
A beaker with 200 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop...?
The total molarity of acid and conjugate base in this buffer is 0.1 M. A student adds 8.00 mL of a 0.280 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.76.
Please show your work. Thank you!A beaker with 200 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop...?
The ionisation of a weak acid given by
HA ==%26gt; H+ + A- with Ka = [H+] [A-] / [HA]. Rearranging Ka and taking logs it is easy to show pH = pKa + log ([A-] / [HA]) Eqn 1.
The corresponding charge balance is
[Na+] + [H+] ===%26gt; [OH-] + [A-]
Given that [Na+] %26gt;%26gt;%26gt; [H+] and [A-] %26gt;%26gt;%26gt; [OH-] the charge balance approximates to [Na+] = [A-]
Substituting pH=5.0, pKa = 4.76 into Eqn 1 leads to log ([A-] / [HA]) = 0.24 or [A-] = 1.738 [HA]. Eqn 2
Given is [A-] + [HA] = 0.1 Eqn 3
Solving Eqn 2 %26amp; 3 simultaneously leads to [A-] = 0.0635 M. Hence [Na+] = 0.0635 M and [HA] = 0.0365 M
Now add HCl
The dilution factor becomes 200 / (200 + 8) = 0.962
Thus
1. [Na+] = 0.0635 x 0.962 = 0.0611 M
2. [A-] + [HA] = 0.1 x 0.962 = 0.0962 M
3. [Cl-] = 8 x 0.28 /(200 + 8) = 0.0108 M
The new charge balance becomes
[Na+] + [H+] ===%26gt; [OH-] + [A-] + [Cl-] which simplifies (for the same reasons as before) to
[Na+] ===%26gt; [A-] + [Cl-] . Thus [A-] = [Na+] - [Cl-] = 0.0611 -0.0108 = 0.0503 M
Hence [HA] = 0.0962 - 0.0503 = 0.0459M
From Eqn 1 and substituting values
pH = 4.76 + log (0.0503/0.0459) = 4.80A beaker with 200 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop...?
The ';a'; and ';b'; start at 0.02 moles each.
Now work out how many moles of HCl are added: 8 x 0.28/1000.
';a'; goes up by this amount, and ';b'; goes down by this amount.
Now work out the new number of moles of ';a'; and ';b';.
Now apply [H+] = Ka x a/b.
The new volume, 208, cancels out.
Please show your work. Thank you!A beaker with 200 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop...?
The ionisation of a weak acid given by
HA ==%26gt; H+ + A- with Ka = [H+] [A-] / [HA]. Rearranging Ka and taking logs it is easy to show pH = pKa + log ([A-] / [HA]) Eqn 1.
The corresponding charge balance is
[Na+] + [H+] ===%26gt; [OH-] + [A-]
Given that [Na+] %26gt;%26gt;%26gt; [H+] and [A-] %26gt;%26gt;%26gt; [OH-] the charge balance approximates to [Na+] = [A-]
Substituting pH=5.0, pKa = 4.76 into Eqn 1 leads to log ([A-] / [HA]) = 0.24 or [A-] = 1.738 [HA]. Eqn 2
Given is [A-] + [HA] = 0.1 Eqn 3
Solving Eqn 2 %26amp; 3 simultaneously leads to [A-] = 0.0635 M. Hence [Na+] = 0.0635 M and [HA] = 0.0365 M
Now add HCl
The dilution factor becomes 200 / (200 + 8) = 0.962
Thus
1. [Na+] = 0.0635 x 0.962 = 0.0611 M
2. [A-] + [HA] = 0.1 x 0.962 = 0.0962 M
3. [Cl-] = 8 x 0.28 /(200 + 8) = 0.0108 M
The new charge balance becomes
[Na+] + [H+] ===%26gt; [OH-] + [A-] + [Cl-] which simplifies (for the same reasons as before) to
[Na+] ===%26gt; [A-] + [Cl-] . Thus [A-] = [Na+] - [Cl-] = 0.0611 -0.0108 = 0.0503 M
Hence [HA] = 0.0962 - 0.0503 = 0.0459M
From Eqn 1 and substituting values
pH = 4.76 + log (0.0503/0.0459) = 4.80A beaker with 200 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop...?
The ';a'; and ';b'; start at 0.02 moles each.
Now work out how many moles of HCl are added: 8 x 0.28/1000.
';a'; goes up by this amount, and ';b'; goes down by this amount.
Now work out the new number of moles of ';a'; and ';b';.
Now apply [H+] = Ka x a/b.
The new volume, 208, cancels out.
Help please!!! pH nightmare!!?
Calculate the change in pH to 0.01 pH units caused by adding 10. mL of 2.78-M NaOH is added to 630. mL of each of the following solutions.
a) water
pH before mixing = 7
pH after mixing= 12.64
pH change = 5.64
b) 0.148 M NH41+
pH before mixing = ?
pH after mixing= ?
pH change = ?
c) 0.148 M NH3
pH before mixing = ?
pH after mixing= ?
pH change = ?
d) a buffer solution that is 0.148 M in each NH41+ and NH3
pH before mixing = ?
pH after mixing= ?
pH change = ?
I found a but am having a lot of trouble figuring out how to do b c and d. I have no clue.Help please!!! pH nightmare!!?
just keep in mind that when doing dilutions that C1*V1 = C2*V2 so if you are adding 10 ml of 2.78 mol/L NaOH to 630 mL of water and you want to find the new concentration so you can determine the pH, you can just plug in.
(2.78M)(10mL)=(C2)(630mL)
C2 = .004M
with that new conc you can find the pH
you must find the pOH since you know the conc of how much acid you are adding, not base
pOH = -log[OH-]
where [OH-] is the concentration you just solved for
kind in mind that pH + pOH = 14
note, this only works for assumed near 100% ionizationHelp please!!! pH nightmare!!?
uh, yea im not gunna do your homework for you.grey hair ireland
a) water
pH before mixing = 7
pH after mixing= 12.64
pH change = 5.64
b) 0.148 M NH41+
pH before mixing = ?
pH after mixing= ?
pH change = ?
c) 0.148 M NH3
pH before mixing = ?
pH after mixing= ?
pH change = ?
d) a buffer solution that is 0.148 M in each NH41+ and NH3
pH before mixing = ?
pH after mixing= ?
pH change = ?
I found a but am having a lot of trouble figuring out how to do b c and d. I have no clue.Help please!!! pH nightmare!!?
just keep in mind that when doing dilutions that C1*V1 = C2*V2 so if you are adding 10 ml of 2.78 mol/L NaOH to 630 mL of water and you want to find the new concentration so you can determine the pH, you can just plug in.
(2.78M)(10mL)=(C2)(630mL)
C2 = .004M
with that new conc you can find the pH
you must find the pOH since you know the conc of how much acid you are adding, not base
pOH = -log[OH-]
where [OH-] is the concentration you just solved for
kind in mind that pH + pOH = 14
note, this only works for assumed near 100% ionizationHelp please!!! pH nightmare!!?
uh, yea im not gunna do your homework for you.
Adding a strong acid to a buffer please help i cant figure this one out?
A beaker with 110 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M . 4.30mL of a 0.330 M solution is added to the beaker. How much will the pH change? The pKa of acetic acid is 4.760.Adding a strong acid to a buffer please help i cant figure this one out?
you did not give the identity of the added acid
HCl, H2SO4,..., ???
you did not give the identity of the added acid
HCl, H2SO4,..., ???
Chemistry pH Calculation Help?
I've worked on this, and the answer I reached was:
';change in pH = 5';
Calculate the pH change when 1.0 mL of 1.0 M NaOH is added to 0.100 L of a solution of
a) 0.10 M acetic acid and 0.10 M sodium acetate.
There are others asked, but I was hoping to understand based on seeing how to do this problem, especially since I am way off!
(The real answer: ';change in pH = 0.1';) Chemistry pH Calculation Help?
pKa of acetic acid = 4.7
pH = pKa + log [CH3COO-] / [CH3COOH]
initial pH = 4.7 + log 0.10 / 0.10 = 4.7
Moles acetic acid = moles acetate = 0.10 M x 0.100 L = 0.010
Moles NaOH = 0.0010 L x 1.0 M = 0.0010
CH3COOH + OH- %26gt;%26gt; CH3COO- + H2O
moles acetic acid = 0.010 - 0.0010 =0.0090
moles acetate = 0.010 + 0.0010 =0.011
total volume = 0.101 L
concentration acetic acid = 0.0090 / 0.101 =0.089 M
concentration acetate = 0.011 / 0.101 =0.11 M
pH = 4.74 + log 0.11 / 0.089 = 4.8
dekta pH = 4.8 - 4.7 = 0.1
';change in pH = 5';
Calculate the pH change when 1.0 mL of 1.0 M NaOH is added to 0.100 L of a solution of
a) 0.10 M acetic acid and 0.10 M sodium acetate.
There are others asked, but I was hoping to understand based on seeing how to do this problem, especially since I am way off!
(The real answer: ';change in pH = 0.1';) Chemistry pH Calculation Help?
pKa of acetic acid = 4.7
pH = pKa + log [CH3COO-] / [CH3COOH]
initial pH = 4.7 + log 0.10 / 0.10 = 4.7
Moles acetic acid = moles acetate = 0.10 M x 0.100 L = 0.010
Moles NaOH = 0.0010 L x 1.0 M = 0.0010
CH3COOH + OH- %26gt;%26gt; CH3COO- + H2O
moles acetic acid = 0.010 - 0.0010 =0.0090
moles acetate = 0.010 + 0.0010 =0.011
total volume = 0.101 L
concentration acetic acid = 0.0090 / 0.101 =0.089 M
concentration acetate = 0.011 / 0.101 =0.11 M
pH = 4.74 + log 0.11 / 0.089 = 4.8
dekta pH = 4.8 - 4.7 = 0.1
How can a substance with pH of 5 changed to pH of 7 by using 45% KOH?
a solution with pH =5 has
[H+] = 1E-5
1 liter has 1E-5 mol H+
to reach pH=7 you need 1E-5 mol KOH
1E-5 mol = 1E-5*(39+1+16) = 5.60E-04 KOH
so you need for each liter of original solution
5.6E-4/0.45 = 1.24E-03 g of KOH 45%How can a substance with pH of 5 changed to pH of 7 by using 45% KOH?
To me the question is rather why do you need so much KOH to change the pH by only 2 units... the answer to that is that the substance in question is a buffer that resist change in pH. Buffer solutions consist of a weak acid and its conjugate base. The resistive action is the result of the equilibrium between the weak acid and its conjugate base.
[H+] = 1E-5
1 liter has 1E-5 mol H+
to reach pH=7 you need 1E-5 mol KOH
1E-5 mol = 1E-5*(39+1+16) = 5.60E-04 KOH
so you need for each liter of original solution
5.6E-4/0.45 = 1.24E-03 g of KOH 45%How can a substance with pH of 5 changed to pH of 7 by using 45% KOH?
To me the question is rather why do you need so much KOH to change the pH by only 2 units... the answer to that is that the substance in question is a buffer that resist change in pH. Buffer solutions consist of a weak acid and its conjugate base. The resistive action is the result of the equilibrium between the weak acid and its conjugate base.
Chemistry calculate pH?
You dilute a diluted Hydrochloric acid-solution with water to twice volume. How did pH change ?Chemistry calculate pH?
If you reduce the concentration of H+ to half (you double the volume) the pH will increase by 0.3pH.
Example: 0.1M HCl pH = -log 0.1 = 1.0
0.05M HCl , pH = -log 0.05 = 1.3
0.0008M HCl pH = -log 0.0008 = 3.1
0.0004M HCl pH = -log 0.0004 = 3.4
It does not matter what pH or [H+] you start with, if you halve the [ H+] the pH will increase by 0.3
take any random [H+]
0.000004684 M HCl pH = 5.33
halve this
0.000002342M HCl pH = 5.63
Chech the log of 2.0 and you will see whyChemistry calculate pH?
Initial concentration of HCl is needed
If you reduce the concentration of H+ to half (you double the volume) the pH will increase by 0.3pH.
Example: 0.1M HCl pH = -log 0.1 = 1.0
0.05M HCl , pH = -log 0.05 = 1.3
0.0008M HCl pH = -log 0.0008 = 3.1
0.0004M HCl pH = -log 0.0004 = 3.4
It does not matter what pH or [H+] you start with, if you halve the [ H+] the pH will increase by 0.3
take any random [H+]
0.000004684 M HCl pH = 5.33
halve this
0.000002342M HCl pH = 5.63
Chech the log of 2.0 and you will see whyChemistry calculate pH?
Initial concentration of HCl is needed
How does aerobic respiration in cells leads to a change in the ph of blood plasma?
As you probably already know, aerobic respiration is the process by which organisms take up O2 and convert it to CO2 and H20 with extraction of energy. So what happens to the CO2 byproduct? It goes straight back to the lungs and gets breathed out, right? Wrong!
CO2 in the blood interacts with water and gets converted to H2CO3. H2CO3 then looses a proton and becomes HCO3- (bicarbonate). HCO3- is how CO2 travels through the blood untill it gets to the lungs where it is converted back to CO2 and leaves as a gas. Now if ventilation decreases and CO2 starts to build up, bicarbonate builds up as well. All of those H+ ions coming off H2CO3 to form HCO3- cause an decrease in pH and the result is acidosis. On the other hand if too much CO2 is being removed, pH increases, acid character decreases, and the result is alkalosis. Its a delicate balance.How does aerobic respiration in cells leads to a change in the ph of blood plasma?
In aerobic tissues the utillization of glucose or fatty acids for energy results in production of CO2 by in the case of glucose the linker reaction (PDH , 2pyruvate to 2 acetyl CoA + 2CO2 ) ,and two CO2s per acetyl CoA from the isocitrate dehydrogenase reaction ( ICDH, isocitrate to alphaketoglutarate + CO2 ) and from the alphaketogltarate dehydrogenase reaction ( aKGDH, alphaketogutarate to succinyl CoA + CO2 ).For fatty acids you get only the two dehydrogenase reactions. In any case the CO2 leaves the tissues and enters the RBC is converted to carbonic acid by carbonic anhydrase then the acid ionizes to yield protons that bind to R hemoglobin and cause it to give up the oxygen , the Bohr effect ( used in aerobic oxidation by the ETS ) and bicarbonate.The bicarbonate leaves the RBC in exchange for Cl^-1..meaning the venous blood has a higher pH than arterial blood , as bicarbonate is a reasonably strong baseproblem with my pc lagging How do you make a quilt
CO2 in the blood interacts with water and gets converted to H2CO3. H2CO3 then looses a proton and becomes HCO3- (bicarbonate). HCO3- is how CO2 travels through the blood untill it gets to the lungs where it is converted back to CO2 and leaves as a gas. Now if ventilation decreases and CO2 starts to build up, bicarbonate builds up as well. All of those H+ ions coming off H2CO3 to form HCO3- cause an decrease in pH and the result is acidosis. On the other hand if too much CO2 is being removed, pH increases, acid character decreases, and the result is alkalosis. Its a delicate balance.How does aerobic respiration in cells leads to a change in the ph of blood plasma?
In aerobic tissues the utillization of glucose or fatty acids for energy results in production of CO2 by in the case of glucose the linker reaction (PDH , 2pyruvate to 2 acetyl CoA + 2CO2 ) ,and two CO2s per acetyl CoA from the isocitrate dehydrogenase reaction ( ICDH, isocitrate to alphaketoglutarate + CO2 ) and from the alphaketogltarate dehydrogenase reaction ( aKGDH, alphaketogutarate to succinyl CoA + CO2 ).For fatty acids you get only the two dehydrogenase reactions. In any case the CO2 leaves the tissues and enters the RBC is converted to carbonic acid by carbonic anhydrase then the acid ionizes to yield protons that bind to R hemoglobin and cause it to give up the oxygen , the Bohr effect ( used in aerobic oxidation by the ETS ) and bicarbonate.The bicarbonate leaves the RBC in exchange for Cl^-1..meaning the venous blood has a higher pH than arterial blood , as bicarbonate is a reasonably strong base
PH of milk and water?
1. With acid addition, does pH drop faster or slower in the milk, as compared to the water? Why?
2. How does the presence of suspended protein in the milk affect the pH change brought about by adding a given amount of acid?
3. What is the relative strength of vinegar and acetic solutions? What is the chemical nature of vinegar?PH of milk and water?
1. With acid addition, does pH drop faster or slower in the milk, as compared to the water? Why?
Slower, because milk has buffer capacity. The two most important buffer components of milk are caseins (buffer maximum near pH 4.6) and calcium phosphate (buffer maxima near pH 7.0).
2. How does the presence of suspended protein in the milk affect the pH change brought about by adding a given amount of acid?
Suspended protein, much of which is casein, is an effective buffer in milk, reducing the amount of pH change caused by the addition of acid.
3. What is the relative strength of vinegar and acetic solutions? What is the chemical nature of vinegar?
They are both composed of water and acetic acid, also known as ethanoic acid, which is the organic chemical that gives vinegar its sour taste and pungent smell.
Acetic acid is a weak, effectively monoprotic acid in aqueous solution, and a 1 molar solution has a pH of 2.4. Vinegar generally has an acetic acid concentration lower than 1 M., and contains other ingredients, so its pH is slightly higher, usually ranging from 2.4 to 3.4.
Vinegar is an acidic liquid processed from the fermentation of ethanol in a process that yields its key ingredient, acetic acid (also called ethanoic acid). It also may come in a diluted form. The acetic acid concentration typically ranges from 4 to 8 percent by volume for table vinegar (typically 5%) and higher concentrations for pickling (up to 18%). Natural vinegars also contain small amounts of tartaric acid, citric acid, and other acids. Vinegar has a density of approximately 0.96 g/mL. The density level depends on the acidity of the vinegar. Household vinegar used for cooking is 1.05 g/mL.
2. How does the presence of suspended protein in the milk affect the pH change brought about by adding a given amount of acid?
3. What is the relative strength of vinegar and acetic solutions? What is the chemical nature of vinegar?PH of milk and water?
1. With acid addition, does pH drop faster or slower in the milk, as compared to the water? Why?
Slower, because milk has buffer capacity. The two most important buffer components of milk are caseins (buffer maximum near pH 4.6) and calcium phosphate (buffer maxima near pH 7.0).
2. How does the presence of suspended protein in the milk affect the pH change brought about by adding a given amount of acid?
Suspended protein, much of which is casein, is an effective buffer in milk, reducing the amount of pH change caused by the addition of acid.
3. What is the relative strength of vinegar and acetic solutions? What is the chemical nature of vinegar?
They are both composed of water and acetic acid, also known as ethanoic acid, which is the organic chemical that gives vinegar its sour taste and pungent smell.
Acetic acid is a weak, effectively monoprotic acid in aqueous solution, and a 1 molar solution has a pH of 2.4. Vinegar generally has an acetic acid concentration lower than 1 M., and contains other ingredients, so its pH is slightly higher, usually ranging from 2.4 to 3.4.
Vinegar is an acidic liquid processed from the fermentation of ethanol in a process that yields its key ingredient, acetic acid (also called ethanoic acid). It also may come in a diluted form. The acetic acid concentration typically ranges from 4 to 8 percent by volume for table vinegar (typically 5%) and higher concentrations for pickling (up to 18%). Natural vinegars also contain small amounts of tartaric acid, citric acid, and other acids. Vinegar has a density of approximately 0.96 g/mL. The density level depends on the acidity of the vinegar. Household vinegar used for cooking is 1.05 g/mL.
How do biological materials respond to changes in pH?
They certainly do. Amino acids can be charged or uncharged as a result of the pH of the solution they are in, and the charge of amino acids is what effects the tertiary structure of a protein.
Help with a gr.12 chem question? (re: dilution and pH)?
A 1 mL sample of 0.1 M HCl is diluted with water to a volume of 100 mL. By how many pH units does the pH change because of the dilution?
thanks!Help with a gr.12 chem question? (re: dilution and pH)?
0.1=10=pH1
.0001=10000=pH4
thanks!Help with a gr.12 chem question? (re: dilution and pH)?
0.1=10=pH1
.0001=10000=pH4
How to follow the rate of reaction?
I'm doing AS chemistry and was wondering if anyone knew how I would be able to follow what happens during a chemical reaction (no particular one in mind). This would be a way of measuring what happens during a reaction as time goes by...like a pH change or a change in gas given off. Also if you have any examples of reactions and the way they are monitored it would be a HUGE help...thanx!How to follow the rate of reaction?
Lots of different ways. If hydrogen ions are produced or lost in the reaction, you can use a pH electrode, but this is not very sensitive as it responds to the log of the changing concentration. If a gas is given off or absorbed, you can measure changes in volume and/or pressure.
One very common method is spectroscopic. At its simplest, you choose a wavelength where only one of the reagents absorbs light, and measure how optical density at that wavelength changes over time.
An exciting variation of this, which won Norrish and Porter (UK scientists) the Nobel prize, is flash photolysis. Here you use a very short pulse of bright light to generate unstable reagents photochemically, and then use spectroscopy to see how quickly they disappear.How to follow the rate of reaction?
For my A-level chemistry course work I followed the chemical reaction of different amounts of hydrogen peroxide and yeast and measured the amount of oxygen produced.
don't u mean ';optical intensity';. Or more specifically, transmittance or absorbance (absorbance has a logarithmic relationship i think).
Lots of different ways. If hydrogen ions are produced or lost in the reaction, you can use a pH electrode, but this is not very sensitive as it responds to the log of the changing concentration. If a gas is given off or absorbed, you can measure changes in volume and/or pressure.
One very common method is spectroscopic. At its simplest, you choose a wavelength where only one of the reagents absorbs light, and measure how optical density at that wavelength changes over time.
An exciting variation of this, which won Norrish and Porter (UK scientists) the Nobel prize, is flash photolysis. Here you use a very short pulse of bright light to generate unstable reagents photochemically, and then use spectroscopy to see how quickly they disappear.How to follow the rate of reaction?
For my A-level chemistry course work I followed the chemical reaction of different amounts of hydrogen peroxide and yeast and measured the amount of oxygen produced.
don't u mean ';optical intensity';. Or more specifically, transmittance or absorbance (absorbance has a logarithmic relationship i think).
How do biological materials respond to changes in pH?
Not very well. The function of biochemicals relies heavily on pH, because peptides are made up out of amino acids, molecules whose net charges are different in diferrent pH's. As such, a part of protein which might need to cluster closely together for it to function might suddenly have a ton of negative charges when the pH increases, which will repulse each other and cause that part to open up. Moreover, the stability of alpha-helices and b猫ta-sheets will decrease rapidly.
Each protein has an optimal pH. A good example are the digestive enzymes in the stomach, which are active in the low, acidic pH of the stomach lumen, but are quickly inactivated by the basic pH of the duodenum.
Other molecules that will respond to pH are acids and bases, of course - Fatty acids, for example, will likely look slightly different at different pHs, but these changes aren't as large as the ones in proteins.gives out fashion advice mobile
Each protein has an optimal pH. A good example are the digestive enzymes in the stomach, which are active in the low, acidic pH of the stomach lumen, but are quickly inactivated by the basic pH of the duodenum.
Other molecules that will respond to pH are acids and bases, of course - Fatty acids, for example, will likely look slightly different at different pHs, but these changes aren't as large as the ones in proteins.
How can large changes in pH levels affect reaction?
1.What happens when an acid or a base is added to a buffer solution?
thank you in advanceHow can large changes in pH levels affect reaction?
Buffers are designed to maintain a relatively constant pH when acids or bases are added to a mixture.
However, buffers do have a capacity limit. This means that if too much acid or base is added the buffer will be ineffective and the pH can change drastically.
Some of the factors affecting the capacity of a buffer are:
Vo.ume of the buffer solution. The larger the volume the
more acid or base it can accommodate.
Concentration of the buffering materials. The more
concentrated, the more acid or base it can accommodate.How can large changes in pH levels affect reaction?
if little amounts of these are added nothing happens to pH.thts how we define buffer solution
thank you in advanceHow can large changes in pH levels affect reaction?
Buffers are designed to maintain a relatively constant pH when acids or bases are added to a mixture.
However, buffers do have a capacity limit. This means that if too much acid or base is added the buffer will be ineffective and the pH can change drastically.
Some of the factors affecting the capacity of a buffer are:
Vo.ume of the buffer solution. The larger the volume the
more acid or base it can accommodate.
Concentration of the buffering materials. The more
concentrated, the more acid or base it can accommodate.How can large changes in pH levels affect reaction?
if little amounts of these are added nothing happens to pH.thts how we define buffer solution
I'm ttc and would like to know how to test CM pH level?
My husband and I are ttc a girl. We've heard a lot about the gender diet and supplements and changing the pH level of cervical mucous. But . . . HOW do I measure this? I don't think I can just test my urine with the pH strips. --Not trying to gross anyone out, but do I (literally) just stick the pH strip in my *v* to test the CM?
Any help is greatly appreciated!I'm ttc and would like to know how to test CM pH level?
Dont know how to test but u could always try preseed its got a ph that is fab for sperm so def cant do any harm, give it a go, i did and i'm pregnant.
Goodluck xxxxxxxxxxx
Any help is greatly appreciated!I'm ttc and would like to know how to test CM pH level?
Dont know how to test but u could always try preseed its got a ph that is fab for sperm so def cant do any harm, give it a go, i did and i'm pregnant.
Goodluck xxxxxxxxxxx
How can lake trout adjust to changes in pH?
Supposing the lake is salt water, the trout in the lake would be considered to be an ';osmoregulator.'; An osmoregulator is an organism that controls its internal osmolarity independent of that of its environment. What this means is, they can either expel a lot or a little of the salts (which can change the pH levels in the trout) it takes in from the mouth as urine. Trout live in water more concentrated than body fluids, therefore they tend to lose water and gain salts. Typically, they urinate smaller amounts, and their urine is slightly less concentrated than body fluids. So to answer your question directly: they can adjust to changes in pH by either increasing or decreasing the amount of salt contents they contain and excrete as urine (since they are osmoregulators).
Hope this helps.
-ChrisSmith83
Hope this helps.
-ChrisSmith83
I want to test the effect of ph level on enzyme activity?
how can i go about doing this (changing the ph level) but still have just one control variable.I want to test the effect of ph level on enzyme activity?
Use three test tubes, put equal amout of enzymes in all and put the substance they digest in both (equal amounts of course).
take a test tube(A) and put 2cm3 of Hydrochloric acid.
Take test tube (B) and put 2cm3 of Pure water(pH7).
Take test tube (C) and put 2cm3 of Sodium Hydroxide.
shake them all a little just as you start the test.
Leave them for half an hour at their optimum temperature and other factors.Make sure all factors among them are equal.
After that, Test for the substance you put in (e.g test for starch using iodine if you put starch in).
The one with the most negative result is the optimum pH.
Use three test tubes, put equal amout of enzymes in all and put the substance they digest in both (equal amounts of course).
take a test tube(A) and put 2cm3 of Hydrochloric acid.
Take test tube (B) and put 2cm3 of Pure water(pH7).
Take test tube (C) and put 2cm3 of Sodium Hydroxide.
shake them all a little just as you start the test.
Leave them for half an hour at their optimum temperature and other factors.Make sure all factors among them are equal.
After that, Test for the substance you put in (e.g test for starch using iodine if you put starch in).
The one with the most negative result is the optimum pH.
Does temperature change the acidity (pH levels) of california orange juice? and by how much?
what is the change from normal room temperature to say, a warmer temp, or from the fridge?Does temperature change the acidity (pH levels) of california orange juice? and by how much?
This answer was actually asked before. It does change, but by a very small amount.
http://answers.yahoo.com/question/index;Does temperature change the acidity (pH levels) of california orange juice? and by how much?
temprature has no effect of any substance..
pH is changed only when the amount H+ ions increases or decreases..How do I bind a quilt web design and hosting
This answer was actually asked before. It does change, but by a very small amount.
http://answers.yahoo.com/question/index;Does temperature change the acidity (pH levels) of california orange juice? and by how much?
temprature has no effect of any substance..
pH is changed only when the amount H+ ions increases or decreases..
PH and acid disassociation constant?
if the 0.50M acetic acid solution is diluted to 0.010M, how would its pH change? Does its Ka value change?
For 0.50M acetic acid i got a pH of 2.44 during experiment.PH and acid disassociation constant?
acetic acid
CH3COOH %26lt;-----%26gt; CH3COO- + H+
So, CH3COOH is not completely dissociated to produce hydrogen ions
So, although you change to concentration of acetic acid, your pH of acetic acid will not change appreciably, it can be a little changed.
Ka value never changes (because it is dissociation constant of acid but there is some evidence that Ka value change with temperature)
For 0.50M acetic acid i got a pH of 2.44 during experiment.PH and acid disassociation constant?
acetic acid
CH3COOH %26lt;-----%26gt; CH3COO- + H+
So, CH3COOH is not completely dissociated to produce hydrogen ions
So, although you change to concentration of acetic acid, your pH of acetic acid will not change appreciably, it can be a little changed.
Ka value never changes (because it is dissociation constant of acid but there is some evidence that Ka value change with temperature)
Discuss how disgestion of food can be affected by changes in pH levels in the small intestine?
5+ Stars and Awesome Feedback to the Clear Best Answer.
Help with this would be much appreciated.
Cheers, Good Luck!!.Discuss how disgestion of food can be affected by changes in pH levels in the small intestine?
As the acid chyme enters the duodenum (first 25 cm of the small intestine) a hormone called secretin is released from the intestinal walls to siginal the pancreas to release a bicarbonate solution which neutralizes the acid.
The hormone CHOLECYSTOKININ (CCK), is released from the intestinal cells causing the gall bladder to release bile. It also causes the pancreas to release its digestive enzymes. The hormone ENTEROGESTRONE is also secreted to slow down peristalsis. Protein Digestion: Trypsin and Chymotrypsin are enzymes that break bonds next to specific amino acids. Carboxypeptidase splits off one amino acid at a time.
This enzyme works on the end with the free carboxyl group. Aminopeptidase works in the opposite direction. All the above enzymes are secreted in an inactive form. They are activated by the hormone ENTEROKINASE. Fat Digestion: Bile emulsifies fat. This creates a larger surface area for the enzyme lipase to digest it. Carbohydrate Digestion: Disaccharide digestion is under the control of the enzymes maltase, lactase, sucrase.
If the pH is changed all the reactions above would not work effectively. The small intestine's pH is between 8.1 - 9.3. These enzymes would become denatured and lose their function in an acidic environment.
Help with this would be much appreciated.
Cheers, Good Luck!!.Discuss how disgestion of food can be affected by changes in pH levels in the small intestine?
As the acid chyme enters the duodenum (first 25 cm of the small intestine) a hormone called secretin is released from the intestinal walls to siginal the pancreas to release a bicarbonate solution which neutralizes the acid.
The hormone CHOLECYSTOKININ (CCK), is released from the intestinal cells causing the gall bladder to release bile. It also causes the pancreas to release its digestive enzymes. The hormone ENTEROGESTRONE is also secreted to slow down peristalsis. Protein Digestion: Trypsin and Chymotrypsin are enzymes that break bonds next to specific amino acids. Carboxypeptidase splits off one amino acid at a time.
This enzyme works on the end with the free carboxyl group. Aminopeptidase works in the opposite direction. All the above enzymes are secreted in an inactive form. They are activated by the hormone ENTEROKINASE. Fat Digestion: Bile emulsifies fat. This creates a larger surface area for the enzyme lipase to digest it. Carbohydrate Digestion: Disaccharide digestion is under the control of the enzymes maltase, lactase, sucrase.
If the pH is changed all the reactions above would not work effectively. The small intestine's pH is between 8.1 - 9.3. These enzymes would become denatured and lose their function in an acidic environment.
Need help for a Science Laboratory Introduction, please its easy points!!! ?
What do i need to include in my introduction besides the problem, hypothesis, and prediction.... please i could use some help, we are doing the lab on buffers, acids, and bases. The problem is: How do organisms maintain their pH of their tissues within a normal range despite activities that tend to change pH.Need help for a Science Laboratory Introduction, please its easy points!!! ?
For humans a big part of acid base balance is in your respiratory system
For humans a big part of acid base balance is in your respiratory system
How do you make a buffer solution with a PH of 7?
need to prepare 250 mL of the solution.
50 mL of the buffer solution will need yo be able to absorb 0.1 moles of additional H+ or OH- ions without changing th pH by more than 0.01 units.
Must design a procedure for preparing and testing the buffer.
available chemicals
12M HCl
15M NH3
15M Hc2H3O2
NaOH(s)
NaC2H3O2(s)
NH4Cl
Distilled WaterHow do you make a buffer solution with a PH of 7?
Buffers have their highest capacity (and thus should be used) for the range pH= pKa +/- 1.
Acetic acid has pKa=4.75
NH3 has pKb=4.75, so the conjugate acid (NH4+) has pKa=14-4.75 =9.25
Thus you cannot use a weak and a strong electrolyte, you have to use two weak ones. If you combine acetic acid (HC2H3O2) and NH3 in an equimolar fashion, you will get the salt CH3COONH4. This hydrolyzes and gives approximately
[H+]= squareroot (Kw*Ka(HC2H3O2)/Kb (NH3))
But for pKa (HC2H3O2)= pKb (NH3) =%26gt; Ka (HC2H3O2)= Kb(NH3) and [H+]=squareroot (Kw) =squareroot (10^-14) =10^-7 =%26gt;pH =7
You want to add 0.1/0.05= 2 mole/L H+ or OH- and have a change of less than 0.01 in pH.
Thus the buffering capacity should be
å°¾=dC/dpH= 2/0.01= 200
I think that according to
http://www.chembuddy.com/?left=pH-calcul
å°¾=2.303* (Kw/[H+] + [H+] + CaKa[H+] / ((Ka+[H+])^2) + CbKb[OH-] / ((Kb+[OH-])^2))
and since Ka=Kb, [H+]=10^-7=[OH-] and we need Ca=Cb so that we have only the salt remaining in the solution, we have
å°¾=2.303* (Kw/[H+] + [H+] + 2CaKa[H+] / ((Ka+[H+])^2)) =%26gt;
200 =2.303* (10^-7+10^-7+ 2C*10^-4.75*10^-7/((10^-4.75+10^-7)^2)) =%26gt;
100/2.303 -10^-7= C*10^-11.75 / ((10^-4.75+10^-7)^2) =%26gt;
C=((10^-4.75+10^-7)^2)*10^11.75*(100/2?=%26gt;
C=7808
This is an unrealistic value which means that maybe I didn't use the formula correctly or simply you are asking for extraordinary buffering capacity.
If we had a simple acetate buffer and we wanted the same buffering capacity at pH=pKa=4.75, we would need
200= 2.303*(10^-14/10^-4.75 + 10^-4.75 + C*10^-4.75*10^-4.75/ (10^-4.75+10^-4.75)^2) =%26gt;
200/2.303 = 10^-9.25+10^-4.75+ C/4 =%26gt;
C= 347 M. So you see that the buffering capacity you want is not feasible.How do you make a buffer solution with a PH of 7?
the site could answer your question with the examples on the following chemicals you give
http://www.csudh.edu/oliver/chemdata/buf
This intrigues me:
First of all pHs are almost impossible to read or adjust at .01 ???
Wow, to adjust a buffer to trim out at a range7.01 to 6.99 would be quite a stretch! I would guess that .01 Normal solutions of both acids and bases would have to be used to stabilize a solution at this level of accuracy.
Even a little ambient air CO2 migrating into the solution would drop the pH a smidgen. If you made the buffer with a lot more salt(from the acid-base reaction) and brought it accurately to 7.00 pH; I believe you would still not be able to hold it that stable.
We call his spurious accuracy.
Oh, I almost forgot, the two that you would use to make the attempt would be HCl and NaOH.
Add an Acidic compound
A salt formed due to neutralisation of weak acid with weak base behaves as simple buffer at pH = 7.
50 mL of the buffer solution will need yo be able to absorb 0.1 moles of additional H+ or OH- ions without changing th pH by more than 0.01 units.
Must design a procedure for preparing and testing the buffer.
available chemicals
12M HCl
15M NH3
15M Hc2H3O2
NaOH(s)
NaC2H3O2(s)
NH4Cl
Distilled WaterHow do you make a buffer solution with a PH of 7?
Buffers have their highest capacity (and thus should be used) for the range pH= pKa +/- 1.
Acetic acid has pKa=4.75
NH3 has pKb=4.75, so the conjugate acid (NH4+) has pKa=14-4.75 =9.25
Thus you cannot use a weak and a strong electrolyte, you have to use two weak ones. If you combine acetic acid (HC2H3O2) and NH3 in an equimolar fashion, you will get the salt CH3COONH4. This hydrolyzes and gives approximately
[H+]= squareroot (Kw*Ka(HC2H3O2)/Kb (NH3))
But for pKa (HC2H3O2)= pKb (NH3) =%26gt; Ka (HC2H3O2)= Kb(NH3) and [H+]=squareroot (Kw) =squareroot (10^-14) =10^-7 =%26gt;pH =7
You want to add 0.1/0.05= 2 mole/L H+ or OH- and have a change of less than 0.01 in pH.
Thus the buffering capacity should be
å°¾=dC/dpH= 2/0.01= 200
I think that according to
http://www.chembuddy.com/?left=pH-calcul
å°¾=2.303* (Kw/[H+] + [H+] + CaKa[H+] / ((Ka+[H+])^2) + CbKb[OH-] / ((Kb+[OH-])^2))
and since Ka=Kb, [H+]=10^-7=[OH-] and we need Ca=Cb so that we have only the salt remaining in the solution, we have
å°¾=2.303* (Kw/[H+] + [H+] + 2CaKa[H+] / ((Ka+[H+])^2)) =%26gt;
200 =2.303* (10^-7+10^-7+ 2C*10^-4.75*10^-7/((10^-4.75+10^-7)^2)) =%26gt;
100/2.303 -10^-7= C*10^-11.75 / ((10^-4.75+10^-7)^2) =%26gt;
C=((10^-4.75+10^-7)^2)*10^11.75*(100/2?=%26gt;
C=7808
This is an unrealistic value which means that maybe I didn't use the formula correctly or simply you are asking for extraordinary buffering capacity.
If we had a simple acetate buffer and we wanted the same buffering capacity at pH=pKa=4.75, we would need
200= 2.303*(10^-14/10^-4.75 + 10^-4.75 + C*10^-4.75*10^-4.75/ (10^-4.75+10^-4.75)^2) =%26gt;
200/2.303 = 10^-9.25+10^-4.75+ C/4 =%26gt;
C= 347 M. So you see that the buffering capacity you want is not feasible.How do you make a buffer solution with a PH of 7?
the site could answer your question with the examples on the following chemicals you give
http://www.csudh.edu/oliver/chemdata/buf
This intrigues me:
First of all pHs are almost impossible to read or adjust at .01 ???
Wow, to adjust a buffer to trim out at a range7.01 to 6.99 would be quite a stretch! I would guess that .01 Normal solutions of both acids and bases would have to be used to stabilize a solution at this level of accuracy.
Even a little ambient air CO2 migrating into the solution would drop the pH a smidgen. If you made the buffer with a lot more salt(from the acid-base reaction) and brought it accurately to 7.00 pH; I believe you would still not be able to hold it that stable.
We call his spurious accuracy.
Oh, I almost forgot, the two that you would use to make the attempt would be HCl and NaOH.
Add an Acidic compound
A salt formed due to neutralisation of weak acid with weak base behaves as simple buffer at pH = 7.
Help with ph and percent ionization?
0.035 mol of solid C3H7COONa is added to 450 mL of 0.10 M C3H7COOH. Assume no change in the volume of the solution. Ka for C3H7COOH is 1.52*10-5
a. How much will the percent ionization of the butanoic acid change? Give the absolute value.
b. How much will the pH change?Help with ph and percent ionization?
In the solution of butanoic acid;
C3H7COOH(a) %26lt;------%26gt; C3H7COO-(aq) + H+(aq)
0.10 M - x ................................ x M ............... x M
Ka = [C3H7COO-][H+] / [C3H7COOH] = 1.52x10^-5
(x)(x) / (0.10 - x) = 1.52x10^-5
Since x is very small compared to 0.10, x can be neglected.
x^2 = 1.52 x10^-6
x = 1.23x10^-3 M = [H+]
pH = -log[H+] = -log(1.23x10^-3) = 2.91
% ionization = (1.23x10^-3 / 0.1)x100 = 1.23 %
When sodium butanoate (C3H7COONa) is added to the acid solution, it dissociates completely;
C3H7COONa(aq) -----%26gt; C3H7COO-(aq) + Na+(aq)
0.035 mol .......................... 0.035 mol
Molarity of C3H7COO- ion = n / V = 0.035 mol / 0.450 L
= 0.078 M
The concentration of C3H7COO- ion (0.078 M) produced by the dissociation of the salt is much more larger than that of produced by the dissociation of the acid (1.23x10^-3). Therefore we can neglect 1.23x10^-3 M (The common ion effect).
Ka = [C3H7COO-][H+] / [C3H7COOH] = 1.52x10^-5
(0.078)[H+] / (0.10) = 1.52x10^-5
[H+] = 1.95x10^-5 M
pH = 4.71
pH increases from 2.91 to 4.71
% ionization = (1.95x10^-5 / 0.1)x100 = 0.02 %
Percent ionization decreases from 1.23% to 0.02%Help with ph and percent ionization?
i love youhair straightener set up a cuckold session tonight
a. How much will the percent ionization of the butanoic acid change? Give the absolute value.
b. How much will the pH change?Help with ph and percent ionization?
In the solution of butanoic acid;
C3H7COOH(a) %26lt;------%26gt; C3H7COO-(aq) + H+(aq)
0.10 M - x ................................ x M ............... x M
Ka = [C3H7COO-][H+] / [C3H7COOH] = 1.52x10^-5
(x)(x) / (0.10 - x) = 1.52x10^-5
Since x is very small compared to 0.10, x can be neglected.
x^2 = 1.52 x10^-6
x = 1.23x10^-3 M = [H+]
pH = -log[H+] = -log(1.23x10^-3) = 2.91
% ionization = (1.23x10^-3 / 0.1)x100 = 1.23 %
When sodium butanoate (C3H7COONa) is added to the acid solution, it dissociates completely;
C3H7COONa(aq) -----%26gt; C3H7COO-(aq) + Na+(aq)
0.035 mol .......................... 0.035 mol
Molarity of C3H7COO- ion = n / V = 0.035 mol / 0.450 L
= 0.078 M
The concentration of C3H7COO- ion (0.078 M) produced by the dissociation of the salt is much more larger than that of produced by the dissociation of the acid (1.23x10^-3). Therefore we can neglect 1.23x10^-3 M (The common ion effect).
Ka = [C3H7COO-][H+] / [C3H7COOH] = 1.52x10^-5
(0.078)[H+] / (0.10) = 1.52x10^-5
[H+] = 1.95x10^-5 M
pH = 4.71
pH increases from 2.91 to 4.71
% ionization = (1.95x10^-5 / 0.1)x100 = 0.02 %
Percent ionization decreases from 1.23% to 0.02%Help with ph and percent ionization?
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How do small changes in pH affect an enzyme's rate of reaction?
I understand that extreme pH levels can denature an enzyme's active site, but why do increases/decreases in rate of reaciton occur with smaller changes....what happens structurally or molecularly to the enzyme?How do small changes in pH affect an enzyme's rate of reaction?
pH is a measure of the concentration of hydrogen ions in a solution. Proteins are made of amino acids. Because all amino acids have an NH2 (or NH-) at one end and a COOH (or COO-) at the other, they can readily accept an extra Hydrogen ion (or lose one). In a protein, the amino acids are linked together by peptide bonds, but then the long chain of amino acids are folded into sheets or helixes by hydrogen bonds. It is the 3-dimensional structure of a protein (part of which comes from these sheets or helixes) that gives it its activity. If additional hydrogen atoms are gained or lost, it can disrupt the folding so that the 3-D structure changes slightly. For example, it may make it a little more difficult for the substrate to fit into the active area of the protein, so the procedure catalyzed by that protein would be slowed down.
pH is a measure of the concentration of hydrogen ions in a solution. Proteins are made of amino acids. Because all amino acids have an NH2 (or NH-) at one end and a COOH (or COO-) at the other, they can readily accept an extra Hydrogen ion (or lose one). In a protein, the amino acids are linked together by peptide bonds, but then the long chain of amino acids are folded into sheets or helixes by hydrogen bonds. It is the 3-dimensional structure of a protein (part of which comes from these sheets or helixes) that gives it its activity. If additional hydrogen atoms are gained or lost, it can disrupt the folding so that the 3-D structure changes slightly. For example, it may make it a little more difficult for the substrate to fit into the active area of the protein, so the procedure catalyzed by that protein would be slowed down.
How are changes in pH, temperature, enzyme concentration related to body functions and how are they affected?
Your body function optimally at around 98 degrees. this is the best temp for your enzymes to operate. any lower and they start to get sluggish and not as productive, any higher and the enzymes will denature and won't work at all. The pH is a similar effect. any higher pH and the enzyme will die.
How to find pH of a buffer solution?
A buffer is prepared by mixing 50.4 mL of 0.050 M sodium bicarbonate and 10.8 mL of 0.10 M NaOH.
(a) What is the pH?
(b) How many grams of HCl must be added to 25.0 mL of the buffer to change the pH by 0.07 units?
Answers in gramsHow to find pH of a buffer solution?
I'll do a, you do b.
Ka (H2CO3) = 4.3E-7 and Ka (HCO3-) = 5.6E-11
a)
NaHCO3 + NaOH ---%26gt; Na2CO3 + H2O
50.4 mL * 0.050 M = 2.5 mmol NaHCO3
10.8 mL * 0.100 M = 1.08 mmol NaOH
2.5 mmol NaHCO3 will react completely with 1.08 mmol NaOH to produce 1.08 mmol Na2CO3 (2.5-1.08=1.42 mmol NaHCO3 leftover). So you would have a buffer solution with:
1.42 mmol NaHCO3
1.08 mmol Na2CO3
Use the Henderson-Hasselbalch equation:
pH = pKa + log[A-/HA]
pH = -log[5.6E-11] + log[1.08/1.42]
pH = 10.25 - 0.12 = 10.13
(a) What is the pH?
(b) How many grams of HCl must be added to 25.0 mL of the buffer to change the pH by 0.07 units?
Answers in gramsHow to find pH of a buffer solution?
I'll do a, you do b.
Ka (H2CO3) = 4.3E-7 and Ka (HCO3-) = 5.6E-11
a)
NaHCO3 + NaOH ---%26gt; Na2CO3 + H2O
50.4 mL * 0.050 M = 2.5 mmol NaHCO3
10.8 mL * 0.100 M = 1.08 mmol NaOH
2.5 mmol NaHCO3 will react completely with 1.08 mmol NaOH to produce 1.08 mmol Na2CO3 (2.5-1.08=1.42 mmol NaHCO3 leftover). So you would have a buffer solution with:
1.42 mmol NaHCO3
1.08 mmol Na2CO3
Use the Henderson-Hasselbalch equation:
pH = pKa + log[A-/HA]
pH = -log[5.6E-11] + log[1.08/1.42]
pH = 10.25 - 0.12 = 10.13
Driftwood and pH levels?
In one of my 10 gallon tank, I have a piece of driftwood that about 12 inches long, and 2 inches wide.
So driftwood will change the pH, but how long does it take to do so, and how significant is the change?
If I keep doing water changes, the pH change that I have accumulated will go back to regular tap water pH right?Driftwood and pH levels?
';Make sure the wood came from fresh waters containing no salt or pollution. Quite often the wood will cause the water to turn yellow and drop the pH. If this occurs, transfer the wood to a bucket and make frequent water changes until the wood has nothing left to give. Make sure there are no other factors in the quarantine tank that may lead to such changes in water chemistry. If all looks good, try adding a fish to the aquarium. If the driftwood was found dried out you may need to anchor it down in the tank with large rocks. Remember to scrub even store bought wood clean with a strong brush before introducing it to any aquarium.'; Happy Fish keeping';Driftwood and pH levels?
Driftwood in your tank, leeches, as the term is called, tannins into your water. This directly effects your PH, and your hardness buffer. Typically, as your hardness drops, so will your PH. This is what driftwood does to your PH.
How long it will take is going to vary on several factors, among them being, the volume, the relative PH and hardness in the tank, and the overall size of driftwood in the water. Each tank is going to see a drop in PH at different rates. You also have fish population and your water changes to factor in as well.
You'll never get all the waste cleared out of your substrate, no matter how hard you try. There will always be small amounts leftover. As this material continues to breakdown and decay, it will begin to form small amounts of carbonic and trace amounts of nitric acid in the water. This too goes after your PH and hardness. This is why you typically see mature tanks end up at a lower PH then they started.
Is this a desired result you are trying to achieve, or is this more about how to combat the corresponding drop that will occur? If you are trying to control it, I'd reccomend adding a crushed coral substrate or adding a hardness conditioner to the water you are changing out if that is a concern of yours.
So driftwood will change the pH, but how long does it take to do so, and how significant is the change?
If I keep doing water changes, the pH change that I have accumulated will go back to regular tap water pH right?Driftwood and pH levels?
';Make sure the wood came from fresh waters containing no salt or pollution. Quite often the wood will cause the water to turn yellow and drop the pH. If this occurs, transfer the wood to a bucket and make frequent water changes until the wood has nothing left to give. Make sure there are no other factors in the quarantine tank that may lead to such changes in water chemistry. If all looks good, try adding a fish to the aquarium. If the driftwood was found dried out you may need to anchor it down in the tank with large rocks. Remember to scrub even store bought wood clean with a strong brush before introducing it to any aquarium.'; Happy Fish keeping';Driftwood and pH levels?
Driftwood in your tank, leeches, as the term is called, tannins into your water. This directly effects your PH, and your hardness buffer. Typically, as your hardness drops, so will your PH. This is what driftwood does to your PH.
How long it will take is going to vary on several factors, among them being, the volume, the relative PH and hardness in the tank, and the overall size of driftwood in the water. Each tank is going to see a drop in PH at different rates. You also have fish population and your water changes to factor in as well.
You'll never get all the waste cleared out of your substrate, no matter how hard you try. There will always be small amounts leftover. As this material continues to breakdown and decay, it will begin to form small amounts of carbonic and trace amounts of nitric acid in the water. This too goes after your PH and hardness. This is why you typically see mature tanks end up at a lower PH then they started.
Is this a desired result you are trying to achieve, or is this more about how to combat the corresponding drop that will occur? If you are trying to control it, I'd reccomend adding a crushed coral substrate or adding a hardness conditioner to the water you are changing out if that is a concern of yours.
How do buffers reduce changes in pH when hydrogen ions or hydroxide ions are added to a solution?
The buffer solution is mainly a weak acid and it's salt
CH3COOH %26amp; CH3COONa
when OH ions are added it reacts with the dissociated NA+ ions to form NaOH ,or H ions to form water
when h ions are added , it reacts with The CH3COO- to form CH3COOH
so there is less change in phHow do buffers reduce changes in pH when hydrogen ions or hydroxide ions are added to a solution?
The buffer solutions shift the chemical equilibrium and there is a little change in pH due to common ion effect. If we will add hydrogen ion it will change to lower pH and vice versa. But very little effectdog which university is bigger
CH3COOH %26amp; CH3COONa
when OH ions are added it reacts with the dissociated NA+ ions to form NaOH ,or H ions to form water
when h ions are added , it reacts with The CH3COO- to form CH3COOH
so there is less change in phHow do buffers reduce changes in pH when hydrogen ions or hydroxide ions are added to a solution?
The buffer solutions shift the chemical equilibrium and there is a little change in pH due to common ion effect. If we will add hydrogen ion it will change to lower pH and vice versa. But very little effect
How would hydrochloric acid would change the pH of creek water?
I am doing a lab in Environmental science. It involves having 3 coke bottles filled with creek water, 2 of them also consisting creek sediment. I drop about 4 drops of hydrochloric acid everyday. The purpose of the lab is to see if the acid will evaporate from the bottle or if the sediment 'sucks' the acid from the water. I believe my results are wrong. Does anyone know what should happen?How would hydrochloric acid would change the pH of creek water?
the ph of creek water (a salty substance) is high on the alkaline scale, hydrochloric acid with a ph of about 1-2 would basically neutralize the new mixture made possibly leaving it slightly acidic dependent on the concentraction of the creek waterHow would hydrochloric acid would change the pH of creek water?
i believe the sediment is slightly basic and the hcl is acidic so the sample with sediment should have a more neutral ph
the ph of creek water (a salty substance) is high on the alkaline scale, hydrochloric acid with a ph of about 1-2 would basically neutralize the new mixture made possibly leaving it slightly acidic dependent on the concentraction of the creek waterHow would hydrochloric acid would change the pH of creek water?
i believe the sediment is slightly basic and the hcl is acidic so the sample with sediment should have a more neutral ph
What happens to the pH of water when CO2 is added?
And how does bromthymol blue help detect changes in pH?What happens to the pH of water when CO2 is added?
Obviously a homework question. You should be able to derive your own answer from the link below.
Obviously a homework question. You should be able to derive your own answer from the link below.
How would changes in pH afffect the ability of the blood to carry oxygen?
pH changes would alter the structure of hemoglobin, inhibiting the binding of oxygen to it.How would changes in pH afffect the ability of the blood to carry oxygen?
The main component of blood that carries oxygen are the red blood cells, and the red blood cells contain the protein hemoglobin. Hemoglobin is what attaches to the oxygen.
Since it is a protein, it is made of of amino acids, which are connected by bonds. In this case, hydrogen bonds are what we're looking at specifically.
Since pH is determined by how much hydrogen concentrations in the solution, then a change in pH can change the shape of a protein. There are difference in the concentration of hydrogen that might mess with the hydrogen bonds keeping the protein together.
Since shape = function in proteins, changing the shape of the protein may not allow it to bind with oxygen properly.
HTH.
The main component of blood that carries oxygen are the red blood cells, and the red blood cells contain the protein hemoglobin. Hemoglobin is what attaches to the oxygen.
Since it is a protein, it is made of of amino acids, which are connected by bonds. In this case, hydrogen bonds are what we're looking at specifically.
Since pH is determined by how much hydrogen concentrations in the solution, then a change in pH can change the shape of a protein. There are difference in the concentration of hydrogen that might mess with the hydrogen bonds keeping the protein together.
Since shape = function in proteins, changing the shape of the protein may not allow it to bind with oxygen properly.
HTH.
How do buffer solutions resist changes in pH?
This is for a chemistry take-home test that I have to complete over the summer. I learned in chemistry class last year that buffers resisted changes in pH, but I never really understood how. The choices for the test are:
a. by releasing H+ in acid solutions
b. by releasing H+ in basic solutions
c. by releasing OH- in basic solutions
d. by combining with OH- in acidic solutions
e. by combining with H+ in basic solutionsHow do buffer solutions resist changes in pH?
It's a very icely posed question. Made me think as well.
What's a buffer? It's a mix of a weak acid-weak base conjugate.
It's like CH3COOH + CH3COONa mixture. Suppose we add acid to the solution, the acid will react with the salt and give acetic acid, thus protons being eliminated from acidic solution through combining.
Is it any one of the options? No!
Suppose we add base to the solution. It will react with the acetic acid and extract H+ from it. This is the release of H+ in basic solution. Is it there in the options? Yes. Then THAT is the answer!
a. by releasing H+ in acid solutions
b. by releasing H+ in basic solutions
c. by releasing OH- in basic solutions
d. by combining with OH- in acidic solutions
e. by combining with H+ in basic solutionsHow do buffer solutions resist changes in pH?
It's a very icely posed question. Made me think as well.
What's a buffer? It's a mix of a weak acid-weak base conjugate.
It's like CH3COOH + CH3COONa mixture. Suppose we add acid to the solution, the acid will react with the salt and give acetic acid, thus protons being eliminated from acidic solution through combining.
Is it any one of the options? No!
Suppose we add base to the solution. It will react with the acetic acid and extract H+ from it. This is the release of H+ in basic solution. Is it there in the options? Yes. Then THAT is the answer!
How can changes in pH affect the way an enzyme works?
i have another part to that question im studying for a test and i cant find any notes on it..second part to the question How might this affect the cell as a whole? please help!How can changes in pH affect the way an enzyme works?
Oooh, good question.
As you know, many amino acids are very sensitive to small changes in pH around neutral. So a small drop in pH may cause an carboxylic acid residue like Asp or Glu, to lose its charge and become protonated. This could happen in the active site of an enzyme, causing the enzyme to not perform its catalytic role.
Alternatively, this could happen at another site in the protein. Let's say a pH increase causes a critical lysine residue to deprotonate, and the hard positive charge on the amine moiety is lost. This could cause the neutral lysine to bury itself within the protein and unfold the enzyme; alternatively, it could disrupt a salt bridge that the lysine was engaged in, causing the enzyme to fall apart and unfold.
In the cell, there is a delicate pH balance being maintained. Changing the pH even slightly causes all sorts of problems to the cell. Aqueous chemistry, like biochemistry, is highly dependent on pH. One small kink in the cog can cause the whole factory comes to a grinding halt.Name for a black cat curly hair styles
Oooh, good question.
As you know, many amino acids are very sensitive to small changes in pH around neutral. So a small drop in pH may cause an carboxylic acid residue like Asp or Glu, to lose its charge and become protonated. This could happen in the active site of an enzyme, causing the enzyme to not perform its catalytic role.
Alternatively, this could happen at another site in the protein. Let's say a pH increase causes a critical lysine residue to deprotonate, and the hard positive charge on the amine moiety is lost. This could cause the neutral lysine to bury itself within the protein and unfold the enzyme; alternatively, it could disrupt a salt bridge that the lysine was engaged in, causing the enzyme to fall apart and unfold.
In the cell, there is a delicate pH balance being maintained. Changing the pH even slightly causes all sorts of problems to the cell. Aqueous chemistry, like biochemistry, is highly dependent on pH. One small kink in the cog can cause the whole factory comes to a grinding halt.
How do you raise the ph of soil?
To change the color of my azaleas I need to change the ph of the soil. How do I do this?How do you raise the ph of soil?
your garden center has amendments for this very purpose. A good salesperson will tell you precisely what you need. it'll be something to sprinkle on the ground. Nothing complicatedHow do you raise the ph of soil?
Lime will raise the soil pH. Be very careful in applying it though.
http://www.allotment.org.uk/articles2/So
Here is a web page you could browse, I hope it helps., but do have your soil tested
to raise the ph , lime is added, but for azaleas lime is a no no, get a reading ,if 3.5 - 5.5 lea
your garden center has amendments for this very purpose. A good salesperson will tell you precisely what you need. it'll be something to sprinkle on the ground. Nothing complicatedHow do you raise the ph of soil?
Lime will raise the soil pH. Be very careful in applying it though.
http://www.allotment.org.uk/articles2/So
Here is a web page you could browse, I hope it helps., but do have your soil tested
to raise the ph , lime is added, but for azaleas lime is a no no, get a reading ,if 3.5 - 5.5 lea
Anybody got info on manipulating pH and water activity in foods?
I'm doing a lab project on meat and need to change the pH and water activity to desired levels.
1. I can use ascorbic acid to decrease the pH but how do I know how much to add to decrease to a specific value eg. pH 4.5?
2. In terms of water activity, I was told to use either starch or whey. But again, to decrease to a value of 0.9 and 0.8, how much do I need to put?
Thanks! :)Anybody got info on manipulating pH and water activity in foods?
use the Pearson's chi square test
1. I can use ascorbic acid to decrease the pH but how do I know how much to add to decrease to a specific value eg. pH 4.5?
2. In terms of water activity, I was told to use either starch or whey. But again, to decrease to a value of 0.9 and 0.8, how much do I need to put?
Thanks! :)Anybody got info on manipulating pH and water activity in foods?
use the Pearson's chi square test
How do buffers reduce changes in pH when hydrogen ions or hydroxide ions are added to a solution?
I have a homework in Biology and this is one of the questions. Can you help me answer it?How do buffers reduce changes in pH when hydrogen ions or hydroxide ions are added to a solution?
Buffers are weak acids and their bases. When you add an acid, you change the base to the weak acid. When you add base, you change the acid to the weak base. There is a limit to their buffering capacity depending on the concentration of the buffer.
Buffers are weak acids and their bases. When you add an acid, you change the base to the weak acid. When you add base, you change the acid to the weak base. There is a limit to their buffering capacity depending on the concentration of the buffer.
How to calculate the amount of buffer needed to keep a solution at stable pH?
I have a solution (1.5L) that while it degrades changes its pH from 7 to about 3.5. I need to add a phosphate buffer {[(Na2HPO4 5.7g)+(KH2PO4 3.6g)]/L} to keep it stable at pH 7. How do I calculate the amount of buffer needed?How to calculate the amount of buffer needed to keep a solution at stable pH?
you can't, you can only determine it empirically. A buffer will only control the pH at up to1pH unit each side of a pKa value. Outside of that, it is not buffered.
you can't, you can only determine it empirically. A buffer will only control the pH at up to1pH unit each side of a pKa value. Outside of that, it is not buffered.
How do buffers reduce change in the pH of solutions? Why is this important to living organisms?
It's called the common-ion effect. On both sides of the equation we have conjugate pairs of molecules, and each push the reaction both ways, effectively limiting the range of pH change. In the example below, HCO3- pushes the reaction to the left, while CO2 pushes the reaction to the right. If we push the rxn to the right, we can see we are producing more H+ (lowering the pH). If we push the rxn to the left, we are _using up_ the H+ (raising pH). This equilibrium is what allows for the pH to remain relatively stable.
CO2 + H20 %26lt;-%26gt; H2CO3 %26lt;-%26gt; HCO3- + H+
Why is a buffer important? Many living organisms, organelles, and proteins require a certain pH level for optimum metabolism and activity. If there weren't a solid way for the pH to be monitored for changes, then the enzymes in your body would break down and be rendered useless. This can cause serious complications if very key enzymes are damaged.medium hair control there temperature
CO2 + H20 %26lt;-%26gt; H2CO3 %26lt;-%26gt; HCO3- + H+
Why is a buffer important? Many living organisms, organelles, and proteins require a certain pH level for optimum metabolism and activity. If there weren't a solid way for the pH to be monitored for changes, then the enzymes in your body would break down and be rendered useless. This can cause serious complications if very key enzymes are damaged.
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