Consider exactly one litre of a propanoic acid buffer solution, containing 0.600 M C3H50OH and 0.252 M C3H500. 3 3.1 Determine the pH of the buffer solution. You may use "HA" to denote the formula of the acid. - You may make certain assumptions to simplify your calculations Ka for hydrofluoric acid is 1.3 * 10-5. Determine by means of a full calculation the change in pH of the buffer solution that will result when 100. mL of a 1.00 x 10-2 M HCl solution is added to it. You must indicate all the 3.2 relevant reaction equations in your working.

Consider exactly one litre of a propanoic acid buffer solution, containing 0.600 M C3H50OH and 0.252 M C3H500. 3 3.1 Determine the pH of the buffer solution. You may use "HA" to denote the formula of the acid. - You may make certain assumptions to simplify your calculations Ka for hydrofluoric acid is 1.3 * 10-5. Determine by means of a full calculation the change in pH of the buffer solution that will result when 100. mL of a 1.00 x 10-2 M HCl solution is added to it. You must indicate all the 3.2 relevant reaction equations in your working.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.89QE

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A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?