Textbook Question
A buffer contains significant amounts of acetic acid and sodium acetate. Write equations showing how this buffer neutralizes added acid and added base.
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Ch.17 - Aqueous Ionic Equilibrium
Chapter 17, Problem 38
Use the Henderson–Hasselbalch equation to calculate the pH of each solution in Problem 30.
Verified step by step guidance1
Identify the components of the buffer solution: the weak acid (HA) and its conjugate base (A^-).
Determine the concentrations of the weak acid [HA] and its conjugate base [A^-] in the solution.
Find the pKa of the weak acid. This can often be found in a table of acid dissociation constants.
Use the Henderson–Hasselbalch equation: \( \text{pH} = \text{pKa} + \log \left( \frac{[A^-]}{[HA]} \right) \).
Substitute the values of pKa, [A^-], and [HA] into the equation to calculate the pH.
Related Practice
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Use the Henderson–Hasselbalch equation to calculate the pH of each solution in Problem 29.
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Use the Henderson–Hasselbalch equation to calculate the pH of each solution. c. a solution that contains 10.0 g of HC2H3O2 and 10.0 g of NaC2H3O2 in 150.0 mL of solution
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Calculate the pH of the solution that results from each mixture. b. 125.0 mL of 0.10 M NH3 with 250.0 mL of 0.10 M NH4Cl
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