What is the pH of a solution containing 0.31 M HCOOH and 0.63 M HCOOK? The K_a f

Question

What is the pH of a solution containing 0.31 M HCOOH and 0.63 M HCOOK? The K_a for HCOOH is 1.7 Times 10^-4. Describe the effect on pH (increase, decrease, or no change) that results from each of the following additions: (a) potassium acetate to an acetic acid solution (b) ammonium nitrate to an ammonia solution (c) sodium formats (HCOONa) to a formic acid (HCOOH) solution (d) potassium chloride to a hydrochloric acid solution (e) barium iodide to a hydroiodic acid solution 3. Determine the pH of (a) a 0.40 M CH_3COOH solution (b) a solution that is 0.40 M CH_3COOH and 0.20 MCH_3COONa.

Explanation / Answer

this is abuffer so

pH = pKa + log(conjugate/acid)

pKa = -logKa = -log(1.7*10^-4) = 3.76955

then

pH = 3.76955 + log(0.63/0.61) = 3.7835

ph = 3.7835

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