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(D) Group $IV$ cations include $Co^{2+}, Ni^{2+}, Mn^{2+},$ and $Zn^{2+}$.When $H_2S$ is passed through a basic solution of $Zn^{2+}$,a white precipit

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$Zn^{2+}$

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(D) Group $IV$ cations include $Co^{2+}, Ni^{2+}, Mn^{2+},$ and $Zn^{2+}$.When $H_2S$ is passed through a basic solution of $Zn^{2+}$,a white precipitate of $ZnS$ is formed.This precipitate dissolves in dilute $HCl$ to form $ZnCl_2$: $ZnS + 2HCl \rightarrow ZnCl_2 + H_2S$.$ZnCl_2$ reacts with $NaOH$ to form a white precipitate of $Zn(OH)_2$: $Zn^{2+} + 2OH^{-} \rightarrow Zn(OH)_2 \downarrow$ (White).With potassium ferrocyanide $(K_4[Fe(CN)_6])$,$Zn^{2+}$ ions form a bluish-white precipitate of $K_2Zn_3[Fe(CN)_6]_2$: $3Zn^{2+} + 2K^{+} + 2[Fe(CN)_6]^{4-} \rightarrow K_2Zn_3[Fe(CN)_6]_2 \downarrow$ (Bluish-white).

$A$ solution containing a group $IV$ cation gives a precipitate on passing $H_2S$ gas. $A$ solution of this precipitate in dilute $HCl$ produces a white precipitate with $NaOH$ solution and a bluish-white precipitate with basic potassium ferrocyanide. The cation is:

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