Chemical EquilibriumHard

Question

When CO2(g) is dissolved in water, then the following equilibrium is established

CO2(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)?

Options

A.3.8 × 10–13
B.6.0
C.0.38
D.13.4

Solution

$K_{eq} = 3.8 \times 10^{- 7}\frac{10^{- 6} \times \left\lbrack HCO_{3}^{-} \right\rbrack}{\left\lbrack CO_{2} \right\rbrack} \Rightarrow \frac{\left\lbrack HCO_{3}^{-} \right\rbrack}{\left\lbrack CO_{2} \right\rbrack} = 0.38$

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