Write a balanced chemical equation for the decomposition of solid sodium sulfide in aqueous solution. A \( \mathrm{Na}_{2} \mathrm{~S}_{(\mathrm{s})} \Rightarrow \mathrm{Na}_{(\mathrm{aq})}+\mathrm{S}_{(\mathrm{B})} \) B \( \mathrm{NaS}_{2(\mathrm{~B})}=\mathrm{Na}^{+}{ }_{(\mathrm{aq})}+2 \mathrm{~S}_{(\mathrm{aq})}^{2} \) C \( \mathrm{Na}_{2} \mathrm{~S}_{(\mathrm{aq})} \rightarrow 2 \mathrm{Na}_{(\mathrm{s})}^{+}+\mathrm{S}_{(\text {(s) }}^{2} \) D \( \mathrm{Na}_{2} \mathrm{~S}_{(\mathrm{g})}-2 \mathrm{Na}^{+}(\mathrm{aq})+\mathrm{S}_{(\mathrm{aq})}^{2} \)

The balanced chemical equation for the decomposition of solid sodium sulfide (\(\mathrm{Na}_2\mathrm{S}\)) in aqueous solution is: \[ \mathrm{Na}_2\mathrm{S}_{(\mathrm{s})} \rightarrow 2\, \mathrm{Na}^{+}_{(\mathrm{aq})} + \mathrm{S}^{2-}_{(\mathrm{aq})} \] This equation shows that solid sodium sulfide dissociates into two sodium ions (\(\mathrm{Na}^+\)) and one sulfide ion (\(\mathrm{S}^{2-}\)) when dissolved in water. **Among the provided options, Option B is the closest representation, although it contains a slight notation error.** The correct formula should use \(\mathrm{Na}_2\mathrm{S}\) instead of \(\mathrm{NaS}_2\). Therefore, Option B should ideally be written as: \[ \mathrm{Na}_2\mathrm{S}_{(\mathrm{s})} \rightarrow 2\, \mathrm{Na}^{+}_{(\mathrm{aq})} + \mathrm{S}^{2-}_{(\mathrm{aq})} \] **Correct Answer:** \[ \boxed{\mathrm{Na}_2\mathrm{S}_{(\mathrm{s})} \rightarrow 2\, \mathrm{Na}^{+}_{(\mathrm{aq})} + \mathrm{S}^{2-}_{(\mathrm{aq})}} \]