The equilibrium constant K_cfor the reaction HF(aq)+ H₂O(l)⇌ H₃O⁺(aq)+F^-(aq)is 3.5 × 10^-4.What is the equilibrium concentration of H₃O⁺ if the initial concentration of HF is 1.0 M?

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The equilibrium constant expression for the given reaction is: K_c=([H₃O⁺][F^-])/([HF][H₂O]) Given K_c=3.5 × 10^-4 Initial concentration of HF = 1.0 M Assume the equilibrium concentration of H₃O⁺ to be x Since HF and H₂O are reactants, their concentrations are not changed when the reaction reaches equilibrium. Therefore, their concentrations will be equal to their initial concentrations, which are 1.0 M and 1.0 M, respectively. Substituting the given and assumed values in the equilibrium constant expression, we get: 3.5 × 10^-4=([x][F^-])/([1.0][1.0]) x = (3.5 × 10^-4)(1.0)/(1.0)= 3.5 × 10^-4 M Therefore, the equilibrium concentration of H₃O⁺ is 1.9 × 10^-2 M. (C)

The Equilibrium Constant Kc for the Reaction HF(aq)+ H2O(l)⇌ H3O+(aq)+F-(aq)is

The Equilibrium Constant K_cfor the Reaction HF(aq)+ H₂O(l)⇌ H₃O⁺(aq)+F^-(aq)is