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 phosphate 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 c. Take a fresh 60mL of 0.50M pH 6.83 buffer and add 3.7 mL of 1.00 M NaOH. Using the Henderson Hasselback equation to calculate the new pH of the solution.

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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 phosphate 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

c. Take a fresh 60mL of 0.50M pH 6.83 buffer and add 3.7 mL of 1.00 M NaOH. Using the Henderson Hasselback equation to calculate the new pH of the solution. 

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