A student added 501 mL of 0.35 M HCl to a buffer solution made up of 0.500 mol of citrate (A-), 0.500 mol of citric acid to 1.5 L of water (total volume = 1.5 L) (Ka = 7.41 x 10-4). A.) Calculate the pH of the initial buffer solution (before the addition of the acid). B.) Calculate the pH of the solution after the addition of HCl referenced above. C.) Did the buffer solution exceed its buffer capacity?
A student added 501 mL of 0.35 M HCl to a buffer solution made up of 0.500 mol of citrate (A-), 0.500 mol of citric acid to 1.5 L of water (total volume = 1.5 L) (Ka = 7.41 x 10-4). A.) Calculate the pH of the initial buffer solution (before the addition of the acid). B.) Calculate the pH of the solution after the addition of HCl referenced above. C.) Did the buffer solution exceed its buffer capacity?
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Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.142QP: K4 for acetic acid is 1.7 105 at 25C. A buffer solution is made by mixing 52.1 mL of 0.122 M acetic...
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A student added 501 mL of 0.35 M HCl to a buffer solution made up of 0.500 mol of citrate (A-), 0.500 mol of citric acid to 1.5 L of water (total volume = 1.5 L) (Ka = 7.41 x 10-4).
A.) Calculate the pH of the initial buffer solution (before the addition of the acid).
B.) Calculate the pH of the solution after the addition of HCl referenced above.
C.) Did the buffer solution exceed its buffer capacity?
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This question is answered by using the simple concept of calculation of ph a weak acid anf the its buffere solution using the Henderson hasselbach equation.
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