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Ch.17 - Applications of Aqueous Equilibria
McMurry - Chemistry 8th Edition
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Capitolo 17, Problema 70b

Calculate the pH of 0.375 L of a 0.18 M acetic acid–0.29 M sodium acetate buffer before and after the addition of (b) 0.0060 mol of HBr. Assume that the volume remains constant.

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Identify the components of the buffer system: acetic acid (CH₃COOH) and sodium acetate (CH₃COONa).
Use the Henderson-Hasselbalch equation to calculate the initial pH of the buffer: \( \text{pH} = \text{pK}_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \), where \( \text{pK}_a \) of acetic acid is approximately 4.76.
Calculate the moles of acetic acid and acetate in the buffer: \( \text{moles of CH}_3\text{COOH} = 0.375 \times 0.18 \) and \( \text{moles of CH}_3\text{COONa} = 0.375 \times 0.29 \).
Determine the change in moles of acetic acid and acetate after adding 0.0060 mol of HBr, which reacts with acetate to form acetic acid: \( \text{CH}_3\text{COO}^- + \text{H}^+ \rightarrow \text{CH}_3\text{COOH} \).
Recalculate the pH using the Henderson-Hasselbalch equation with the new concentrations of acetic acid and acetate after the reaction.

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Buffer Solutions

A buffer solution is a system that resists changes in pH upon the addition of small amounts of acid or base. It typically consists of a weak acid and its conjugate base, or a weak base and its conjugate acid. In this case, acetic acid (a weak acid) and sodium acetate (its conjugate base) form a buffer that helps maintain a stable pH when HBr is added.
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Buffer Solutions

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a mathematical formula used to calculate the pH of a buffer solution. It is expressed as pH = pKa + log([A-]/[HA]), where pKa is the negative logarithm of the acid dissociation constant, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the weak acid. This equation is essential for determining the pH before and after the addition of HBr.
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Henderson-Hasselbalch Equation

Acid-Base Neutralization

Acid-base neutralization is a chemical reaction where an acid reacts with a base to produce water and a salt. In this scenario, the addition of HBr (a strong acid) to the buffer will react with the acetate ions from sodium acetate, reducing the concentration of the conjugate base and affecting the overall pH. Understanding this concept is crucial for predicting how the buffer will respond to the added acid.
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Lewis Acids and Bases
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Domanda del libro di testo

Calculate the pH of 0.375 L of a 0.18 M acetic acid–0.29 M sodium acetate buffer before and after the addition of (a) 0.0060 mol of KOH. Assume that the volume remains constant.

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Domanda del libro di testo
Use the Henderson–Hasselbalch equation to calculate the pH of a buffer solution that is 0.25 M in formic acid (HCO2H) and 0.50 M in sodium formate (HCO2Na).
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