What is the K of the reaction HC₂H₃O₂ ⇌ H⁺ + C₂H₃O₂^- , if [HC₂H₃O₂] = 0.15 M and the pH = 3.0?

Question

Quizplus · Accepted Answer

The equilibrium expression for the reaction is $K = \frac{[H^+][S^-][CS(OH)_3^-]}{[HCS(OH)_3]}.$ Given that $[HCS(OH)_3] = 0.15\,M$ and the pH is 3.0 (which means $[H^+] = 10^{-3}\,M$), and assuming the reaction goes to completion, $[S^-] = [CS(OH)_3^-] = 10^{-3}\,M.$ Thus, $K = \frac{(10^{-3})(10^{-3})(10^{-3})}{0.15} = 6.67 \times 10^{-6}.$

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What Is the K of the Reaction HC₂H₃O₂ ⇌ H⁺