Given the equilibrium constants for the equilibria, H₂O(l) $\rightleftharpoons$ H₃O⁺(aq) ; K = $5.69 \times 10 ^ { - 10 }$ 2CH₃COOH(aq) + 2H₂O(l) $\rightleftharpoons$ 2CH₃COO?(aq) + 2H₃O⁺(aq) ; K = $3.06 \times 10 ^ { - 10 }$ determine K_c for the following equilibrium.
CH₃COOH(aq) + NH₃(aq) $\rightleftharpoons$ CH₃COO?(aq) + NH₄⁺(aq)

Question

Given the equilibrium constants for the equilibria, H₂O(l)

\rightleftharpoons

H₃O⁺(aq) ; K =

5.69 \times 10 ^ { - 10 }

2CH₃COOH(aq) + 2H₂O(l)

\rightleftharpoons

2CH₃COO?(aq) + 2H₃O⁺(aq) ; K =

3.06 \times 10 ^ { - 10 }

determine K_c for the following equilibrium.
CH₃COOH(aq) + NH₃(aq)

\rightleftharpoons

CH₃COO?(aq) + NH₄⁺(aq)

Quizplus · Accepted Answer

The equilibrium constant for the given equilibrium can be determined by multiplying the equilibrium constants for the two equilibria that are involved in the given equilibrium. Therefore, Kc = (K1 x K2) = (5.69 x 10^-10) x (3.06 x 10^-10) = 1.75 x 10^-19.

Given the Equilibrium Constants for the Equilibria, H2O(l) ⇌\rightleftharpoons⇌ H3O+(aq); K =

Given the Equilibrium Constants for the Equilibria, H₂O(l) $\rightleftharpoons$ H₃O⁺(aq); K =