Question

write the equilibrium constant expression for this reaction:
h_{2}co_{3}(aq) \to 2h^{+}(aq)+co_{3}^{2 - }(aq)

Explanation:

Step1: Recall the formula for equilibrium constant

For a reaction \(aA + bB
ightleftharpoons cC + dD\), the equilibrium constant \(K=\frac{[C]^c[D]^d}{[A]^a[B]^b}\), where \([X]\) represents the molar concentration of species \(X\).

Step2: Identify the coefficients and species

In the reaction \(H_{2}CO_{3}(aq)
ightleftharpoons2H^{+}(aq)+CO_{3}^{2 - }(aq)\), the coefficient of \(H_{2}CO_{3}\) is \(1\), the coefficient of \(H^{+}\) is \(2\), and the coefficient of \(CO_{3}^{2 - }\) is \(1\).

Step3: Write the equilibrium constant expression

Substitute into the formula: \(K=\frac{[H^{+}]^{2}[CO_{3}^{2 - }]}{[H_{2}CO_{3}]}\)

Answer:

\(K=\frac{[H^{+}]^{2}[CO_{3}^{2 - }]}{[H_{2}CO_{3}]}\)