Worksheet: Buffer pH Changes

In this worksheet, we will practice using ionization equilibrium constants to find the change in a buffer pH when an acid or base is introduced.


Acetate buffers are used in studies of enzymes to prevent pH changes that might affect biochemical reactions. The 𝐾a of acetic acid, the conjugate acid of acetate, is 1.8×10. Calculate to 2 decimal places the pH of an acetate buffer consisting of 0.10 M acetic acid and 0.10 M sodium acetate.


Acetate buffers are used in biochemical studies of enzymes and other chemical components of cells to prevent pH changes that might change the biochemical activity of these compounds.

An acetate buffer is made such that it is 0.10 M in acetic acid and 0.10 M in sodium acetate. By how much does the pH of the buffer change after 1.0 mL of 0.10MNaOH is added to 100 mL of this buffer, giving a solution with a volume of 101 mL? Take 𝐾a of CHCOH32 to be 1.8×10.


A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. The 𝐾a of acetic acid is 1.80×10. To 2 decimal places, what is the pH of the solution produced when 3.00 mL of 0.034 MHCl is added to 0.200 L of the buffer solution?

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