Buffer capacity refers to the amount of acid or base a buffer can absorb without a significant pH change. It is governed by the concentrations of the conjugate acid and base components of the buffer. A 0.5 M buffer can “absorb” five times as much acid or base as a 0.1 M buffer for a given pH change. In the next three problems you begin with a buffer of known pH and concentration and calculate the new pH after a particular quantity of acid or base is added. You are given 60 mL of 0.50 M p2hosphate buffer, pH = 6.83, to test. The starting composition of the buffer, both in terms of the concentration and the molar quantity of the two major phosphate species, is: Concentration of HPO42−: 0.304 M Molar quantity of HPO42−: 18.2 mmol Concentration of H2PO4−: 0.196 M Molar quantity of H2PO4−: 11.8 mmol a. You add 1.7 mL of 1.00 M HCl to the buffer. Calculate the molar quantity of H3O+ added as HCl, and the final molar quantity of HPO42- and H2PO42- at equilibrium.
Buffer capacity refers to the amount of acid or base a buffer can absorb without a significant pH change. It is governed by the concentrations of the conjugate acid and base components of the buffer. A 0.5 M buffer can “absorb” five times as much acid or base as a 0.1 M buffer for a given pH change. In the next three problems you begin with a buffer of known pH and concentration and calculate the new pH after a particular quantity of acid or base is added. You are given 60 mL of 0.50 M p2hosphate buffer, pH = 6.83, to test. The starting composition of the buffer, both in terms of the concentration and the molar quantity of the two major phosphate species, is: Concentration of HPO42−: 0.304 M Molar quantity of HPO42−: 18.2 mmol Concentration of H2PO4−: 0.196 M Molar quantity of H2PO4−: 11.8 mmol a. You add 1.7 mL of 1.00 M HCl to the buffer. Calculate the molar quantity of H3O+ added as HCl, and the final molar quantity of HPO42- and H2PO42- at equilibrium.
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 16.78QE
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Buffer capacity refers to the amount of acid or base a buffer can absorb without a significant pH change. It is governed by the concentrations of the conjugate acid and base components of the buffer. A 0.5 M buffer can “absorb” five times as much acid or base as a 0.1 M buffer for a given pH change. In the next three problems you begin with a buffer of known pH and concentration and calculate the new pH after a particular quantity of acid or base is added.
You are given 60 mL of 0.50 M p2hosphate buffer, pH = 6.83, to test. The starting composition of the buffer, both in terms of the concentration and the molar quantity of the two major phosphate species, is:
| Concentration of HPO42−: 0.304 M | Molar quantity of HPO42−: 18.2 mmol |
| Concentration of H2PO4−: 0.196 M | Molar quantity of H2PO4−: 11.8 mmol |
a. You add 1.7 mL of 1.00 M HCl to the buffer. Calculate the molar quantity of H3O+ added as HCl, and the final molar quantity of HPO42- and H2PO42- at equilibrium.
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