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.

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