Which of the following solutions is a buffer? (a) 0.10 M CH3COOH and 0.10 M CH3COONa, (b) 0.10 M CH3COOH, (c) 0.10 M HCl and 0.10 M NaCl, (d) both a and c, (e) all of a, b, and c.

Verified step by step guidance

Step 1: Understand what a buffer solution is. A buffer solution is one that can resist changes in pH when small amounts of acid or base are added. It typically consists of a weak acid and its conjugate base, or a weak base and its conjugate acid.

Step 2: Analyze option (a): 0.10 M CH3COOH and 0.10 M CH3COONa. CH3COOH is a weak acid and CH3COONa provides the conjugate base, CH3COO-. This combination can act as a buffer.

Step 3: Analyze option (b): 0.10 M CH3COOH. This is only a weak acid without its conjugate base, so it cannot act as a buffer on its own.

Step 4: Analyze option (c): 0.10 M HCl and 0.10 M NaCl. HCl is a strong acid, and NaCl is a neutral salt. This combination does not provide a weak acid/base pair, so it cannot act as a buffer.

Step 5: Determine which options are buffers. Based on the analysis, option (a) is a buffer solution. Option (c) is not a buffer, and option (b) is not a buffer. Therefore, the correct answer is (a).

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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. This equilibrium allows the buffer to neutralize added acids or bases, maintaining a relatively stable pH.

Weak Acids and Conjugate Bases

Weak acids are acids that do not completely dissociate in solution, meaning they establish an equilibrium between the undissociated acid and its ions. The conjugate base is formed when the weak acid donates a proton (H+). In the case of acetic acid (CH3COOH) and sodium acetate (CH3COONa), the acetic acid acts as the weak acid, while the acetate ion serves as its conjugate base.

Strong Acids vs. Weak Acids

Strong acids, such as hydrochloric acid (HCl), completely dissociate in solution, releasing all their protons, which leads to a significant change in pH. In contrast, weak acids only partially dissociate, allowing for a more controlled pH environment. This distinction is crucial when identifying buffer solutions, as only combinations of weak acids and their conjugate bases can effectively function as buffers.

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Calculating Percent Ionization of Weak Acids

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Textbook Question

(a) Calculate the percent ionization of 0.125 M lactic acid (K_a = 1.4 × 10^-4).

Textbook Question

(b) Calculate the percent ionization of 0.0075 M butanoic acid in a solution containing 0.085 M sodium butanoate.

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Textbook Question

(b) Calculate the percent ionization of 0.125 M lactic acid in a solution containing 0.0075 M sodium lactate.

Textbook Question

Which of the following solutions is a buffer? (a) A solution made by mixing 100 mL of 0.100 M CH3COOH and 50 mL of 0.100 M NaOH, (b) a solution made by mixing 100 mL of 0.100 M CH3COOH and 500 mL of 0.100 M NaOH, (c) A solution made by mixing 100 mL of 0.100 M CH3COOH and 50 mL of 0.100 M HCl, (d) A solution made by mixing 100 mL of 0.100 M CH3COOK and 50 mL of 0.100 M KCl.

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Textbook Question

(a) Calculate the pH of a buffer that is 0.12 M in lactic acid and 0.11 M in sodium lactate.

Textbook Question

(b) Calculate the pH of a buffer formed by mixing 85 mL of 0.13 M lactic acid with 95 mL of 0.15 M sodium lactate.