What is the [CH₃CO₂^-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.24? K_a = 1.8 × 10^-5for CH₃CO₂H. A)0.31:1 B)0.89:1 C)1.1:1 D)3.2:1

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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 into this equation, we get:[A-]/[HA] = 10^(4.24 - (-log(1.8 × 10^-5))) = 0.31Therefore, the correct answer is A) 0.31:1.

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

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