Calculate the pH of a buffer solution consists of 0.10 M acetic acid and 0.15 M sodium acetate. Suppose 10.0 mL of 0.02 M HCl solution is added to 90.0 mL of HO buffer system. Calculate the final pH. (pKa = 4.74)

An analytical chemist is titrating 68.1 mL of a 0.6500M solution of propionic acid (HC,H,CO,) with a 0.4500M solution of KOH. The p K, of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 114. mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.

A 1.0 liter solution contains 0.745 M hydrogen fluoride (HF) and 0.786  M sodium fluoride (NaF).  What is the pH of this solution? (Ka for HF is 7.2 x 10 –4) How many moles of solid sodium acetate would have to be added to 2.0 L of 0.293  M acetic acid solution to achieve a buffer of pH 4.77? Assume there is no volume change.      Ka for HC2H3O2 is 1.8  × 10 –5 What molar ratio of sodium acetate to acetic acid,  is required to create a buffer solution having a pH of 4.58 at 25°C?     Ka for HC2H3O2 is 1.8  × 10 –5.

Calculate the pH of 2.0 L of a buffer solution that is 0.531 M acetic acid (CH3COOH) and 0.531 M sodium acetate (NaCH3COO) after 0.30 moles of NaOH is added to the buffer. (Ka for acetic acid = 1.8 × 10−5)