\textbf{230-} Considering the reaction: $\mathrm{CN^-(aq) + HSO_4^-(aq) \rightarrow HCN(aq) + SO_4^{2-}(aq)}$, which statement is correct?
\begin{enumerate}
\item[1)] The $\mathrm{HSO_4^-}$ ion acts as the conjugate base of the sulfate ion in this reaction.
\item[2)] According to the Lowry--Brønsted theory, $\mathrm{HCN}$ acts as a base in this reaction.
\item[3)] The conjugate acid of the sulfate ion is stronger than the conjugate acid of cyanide.
\item[4)] Phenolphthalein indicator in a dilute solution of $\mathrm{CN^-}$ ion in water is colorless.
\end{enumerate}
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\textbf{Calculation Space}
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