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

Question

Given the equilibrium constants for the equilibria, NH₄⁺(aq) + H₂O(l)

\rightleftharpoons

NH₃(aq) + H₃O⁺(aq) ; K_c =

5.69 \times 10 ^ { - 10 }

2H₂O(l)

\rightleftharpoons

2H₃O⁺(aq) ; K_c =

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 reaction can be determined by multiplying the equilibrium constants for the two equilibria that add up to give the desired equilibrium. Thus,K_c = (K_c1)(K_c2) = (5.69 × 10^-10)(3.06 × 10^-10) = 1.75 × 10^-19

Given the Equilibrium Constants for the Equilibria, NH4+(aq) + H2O(l) ⇌\rightleftharpoons⇌

Given the Equilibrium Constants for the Equilibria, NH₄⁺(aq) + H₂O(l) $\rightleftharpoons$