What is the [CH₃COO^-]/[CH₃COOH] ratio necessary to make an aqueous buffer solution with a pH of 4.34?
K_a = 1.8 × 10^-5for CH3COOH.

Question

What is the [CH₃COO^-]/[CH₃COOH] ratio necessary to make an aqueous buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5for CH3COOH. A)0.39:1 B)0.91:1 C)1.09:1 D)2.5:1

Quizplus · Accepted Answer

The Henderson-Hasselbalch equation can be used to calculate the ratio of [CH3COO-]/[CH3COOH] necessary to make an aqueous buffer solution with a pH of 4.34. The equation is:pH = pKa + log([CH3COO-]/[CH3COOH])where pKa is the negative logarithm of the acid dissociation constant, Ka. For CH3COOH, Ka = 1.8 × 10^-5, so pKa = -log(1.8 × 10^-5) = 4.74.Substituting the given values into the Henderson-Hasselbalch equation, we get:4.34 = 4.74 + log([CH3COO-]/[CH3COOH])Solving for [CH3COO-]/[CH3COOH], we get:[CH3COO-]/[CH3COOH] = 10^(4.34 - 4.74) = 0.39Therefore, the [CH3COO-]/[CH3COOH] ratio necessary to make an aqueous buffer solution with a pH of 4.34 is 0.39:1.

What Is the [CH3COO-]/[CH3COOH] Ratio Necessary to Make an Aqueous

What Is the [CH₃COO^-]/[CH₃COOH] Ratio Necessary to Make an Aqueous