In aqueous solution, sulfuric acid dissociates as follows. $\text{H}_2\text{SO}_4 \rightarrow \text{HSO}_4^- + \text{H}^+$ (this reaction goes to completion) $\text{HSO}_4^- \rightleftharpoons \text{SO}_4^{2-} + \text{H}^+$ (this reaction reaches equilibrium with constant $K_c$) An analysis of a $2.00\,\text{mol dm}^{-3}$ solution of $\text{H}_2\text{SO}_4$ gave a $\text{HSO}_4^-$ concentration of $1.988\,\text{mol dm}^{-3}$. What is $K_c$?
- A$1.381 \times 10^{5}\,\text{dm}^3\,\text{mol}^{-1}$
- B$82.34\,\text{dm}^3\,\text{mol}^{-1}$
- C$1.214 \times 10^{-2}\,\text{mol dm}^{-3}$
- D$7.244 \times 10^{-5}\,\text{mol dm}^{-3}$