Consider a buffer solution prepared by dissolving 0.15 mol of benzoic acid (C6H5COOH) and 0.30 mol of sodium benzoate (NaC6H5COO) in 1.00 L of solution. (Ka of Benzoic acid  = 6.3 x 10-5). If 0.05 mol of HCl is added to this buffer solution the pH of the solution will drop slightly. The pH does not drastically decrease because the HCl reacts with the ____ present in the buffer solution.Question 8

Calculate the pH of a buffer solution prepared by dissolving 0.25 mol benzoic acid (C6H5COOH) and 0.15 mol sodium benzoate (C6H5COONa) in 1.00 L of solution. (Ka = 6.3 x 10-5)Question 8Select one:a.4.41b.2.39c.3.98d.10.03

The pH of a buffer solution prepared by using 0.04 M of C6H5COONa and 0.02 M C6H5COOHsolutions is(Note: Ka of acid is 6.4 × 10−5 at 25°C)A. 3.89B. 4.19C. 4.49D. 6.19

How will diluting a buffer solution affect its pH?Question 4AnswerThe pH will remain the same as the concentrations of both weak acid and weak base components remain unchangedThe pH will remain the same as the amounts of both weak acid and weak base components remain unchangedThe pH will decrease as the concentration of the weak acid component will increaseThe pH will increase as the concentration of the weak base component will increase

A chemist prepared a buffer by mixing stock solutions of acetic acid and sodium acetate together to obtain concentrations of [acetic acid] = 0.10 M and [sodium acetate] = 0.15 M in the final solution.However, when they measured the pH of the prepared buffer solution, the pH turned out to be higher than expected according to their calculation. What should the chemist do to fix the pH of the buffer? Question 6AnswerAdd more acetic acidAdd a small amount of waterAdd a small amount of solid NaOHAdd more sodium acetateReduce the volume of the buffer solution by boiling off some solvent

Calculate the number of moles of HCl (g) that must be added to 1.0L of 1.0M NaC2H302 to produce a solution buffered at each pH. (Ka for HC2H3O2 = 1.8X10^-5)a) pH=pKab) pH=3.92c) pH=5.49