A beaker with 180 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 . A student adds 5.80 mL of a 0.490 M solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.760.Adding a strong acid to a buffer?
Well, I'm bad at Chemistry but I can do a partial, concept answer.
A buffer is a chemical which stabilizes pH, so whether acid or base is added, the pH will tend to bend towards the original value.
Sorry, I can't complete the question.
An example of a buffer:
In order to stabilize the pH in blood, the body has an organic buffer of H[2]CO[3], which can decompose into HCO[3]- and H+ in response to a drop in pH and can recompose to H[2]CO[3] for a rise in pH. Since pH is a measure of the proton concentration (H+), the addition or removal of H+ changes the pH.Adding a strong acid to a buffer?
huh?
Subscribe to:
Post Comments
(Atom)
No comments:
Post a Comment