What value in an equilibrium reaction does K have if the other values for the reaction HC₂H₃O₂ ⇌ H⁺ + C₂H₃O₂^- are [A^-] = 0.10 M and [HC₂H₃O₂] = 0.25 M?

Question

Quizplus · Accepted Answer

The equilibrium constant $K$ for the reaction is calculated using the concentrations of the products raised to their stoichiometric coefficients divided by the concentrations of the reactants raised to their stoichiometric coefficients. Given that the stoichiometry of the reaction is 1:1:1, $K = \frac{[AS^-][CSO_4^-]}{[H_2CSO_4]}$. Substituting the given concentrations, $K = \frac{(0.10)(0.10)}{0.25} = 0.04$.

What Value in an Equilibrium Reaction Does K Have If