You made a buffer solution by combining 250.0 mL of a 0.20 M sodium acetate solution with 50.0 mL of 1.0 M acetic acid (pKa = 4.7). To this solutio you then add 100.0 mL of 0.25 M NaOH. What is the final pH of the resulting solution?

An analytical chemist is titrating 205.5 mL of a 0.5600M solution of hydrazoic acid (HN3) with a 1.100M solution of NaOH. The pK of hydrazoic acid is 4.72. Calculate the pH of the acid solution after the chemist has added 111.8 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = 0

Complete the following table, which lists information about the measured acid dissociation constants of three unknown weak acids. Note: be sure each number you put in the table has the correct number of significant digits. acid K Κα PK relative strength a a ☐ x10 A B C 1.2 × 10 3. 10 4 ☐ 11.539 ×

A buffer contains 0.015 mol of lactic acid (pK₁ = 3.86) and 0.080 mol of sodium lactate per liter. H₂C OH Lactic acid OH Calculate the pH of the buffer. H₂C. Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of the buffer. O OH Sodium lactate Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of pure water. O Na+ buffer pH: buffer pH change: water pH change: units units