What is the [CH₃CO₂-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.34?
K_a = 1.8 × 10^-5for CH₃CO₂H.

Question

What is the [CH₃CO₂-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.34? K_a = 1.8 × 10^-5for CH₃CO₂H. A)0)39:1 B)0)91:1 C)1)09:1 D)2)5:1

Quizplus · Accepted Answer

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 into this equation, we get:[A-]/[HA] = 10^(4.34 - (-log(1.8 × 10^-5))) = 39:1Therefore, the correct answer is A) 0)39:1.

What Is the [CH3CO2-]/[CH3CO2H] Ratio Necessary to Make a Buffer

What Is the [CH₃CO₂-]/[CH₃CO₂H] Ratio Necessary to Make a Buffer