What is the [CH₃COO^-]/[CH₃COOH] ratio necessary to make a 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

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The Henderson-Hasselbalch equation is: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 acid.We can rearrange this equation to solve for the ratio of [A-]/[HA]:[A-]/[HA] = 10^(pH - pKa)Substituting the given values, we get:[A-]/[HA] = 10^(4.34 - (-log(1.8 × 10^-5))) = 0.39Therefore, the correct answer is A) 0.39:1.

What Is the [CH3COO-]/[CH3COOH] Ratio Necessary to Make a Buffer

What Is the [CH₃COO^-]/[CH₃COOH] Ratio Necessary to Make a Buffer