Question

write the equilibrium constant expression for this reaction:
2h^{+}(aq)+c_{2}o_{4}^{2 - }(aq)\to h_{2}c_{2}o_{4}(aq)

Explanation:

Step1: Recall the formula for equilibrium constant

For a general 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 reactants and products

In the reaction \(2H^{+}(aq)+C_{2}O_{4}^{2 -}(aq)
ightleftharpoons H_{2}C_{2}O_{4}(aq)\), the reactants are \(H^{+}\) and \(C_{2}O_{4}^{2-}\), and the product is \(H_{2}C_{2}O_{4}\). The stoichiometric coefficient of \(H^{+}\) is \(a = 2\), of \(C_{2}O_{4}^{2-}\) is \(b=1\), and of \(H_{2}C_{2}O_{4}\) is \(c = 1\).

Step3: Write the equilibrium constant expression

Using the formula \(K=\frac{[Product]}{[Reactant1]^{a}[Reactant2]^{b}}\), we substitute the species. So \(K=\frac{[H_{2}C_{2}O_{4}]}{[H^{+}]^{2}[C_{2}O_{4}^{2-}]}\)

Answer:

\(K=\frac{[H_{2}C_{2}O_{4}]}{[H^{+}]^{2}[C_{2}O_{4}^{2-}]}\)