When CO2(g) is dissolved in water, then the following equilibrium is establishedCO2(aq) + 2H2O(l) $\

Question

When CO2(g) is dissolved in water, then the following equilibrium is establishedCO2(aq) + 2H2O(l) $\rightleftharpoons$H3O+ (aq) + HCO3– (aq) for which the equilibrium constant is 3.8 × 10–7. If the pH of solution is 6.0, then what would be the ratio of concentration of HCO3– (aq) to CO2(aq)?

Accepted Answer

$K_{eq} = 3.8 	imes 10^{- 7}\frac{10^{- 6} 	imes \left\lbrack HCO_{3}^{-} ightbrack}{\left\lbrack CO_{2} ightbrack} \Rightarrow \frac{\left\lbrack HCO_{3}^{-} ightbrack}{\left\lbrack CO_{2} ightbrack} = 0.38$

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