What is the approximate value of the equilibrium constant,K_n,for the neutralization of acetic acid with potassium hydroxide,shown in the equation below? The K_a for acetic acid is 1.8 × 10^-5. CH₃CO₂H(aq)+ KOH(aq)⇌ H₂O(l)+ NaCH₃CO₂(aq) A)1.8 × 10^-19 B)5.6 × 10^-10 C)1.8 × 10^-8 D)1.8 × 10⁹

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Quizplus · Accepted Answer

The equilibrium constant for the neutralization reaction of a weak acid (acetic acid) with a strong base (potassium hydroxide) is very large because the reaction proceeds almost to completion. The given $K_a$ for acetic acid is $1.8 \times 10^{-5}$, but this value is not directly used to find the equilibrium constant for the neutralization reaction. Instead, knowing that neutralization reactions favor the production of water and the salt (in this case, sodium acetate), we can infer that the equilibrium constant ($K_{eq}$ or $K_{s}$) is very large, indicating a strong drive to products. Hence, $1.8 \times 10^{19}$ is a representation of a very large equilibrium constant, suitable for a reaction that goes almost to completion.

What Is the Approximate Value of the Equilibrium Constant,Kn,for the Neutralization

What Is the Approximate Value of the Equilibrium Constant,K_n,for the Neutralization