The ratio of amounts of H_2S needed to precip | vedclass

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(A) The precipitation reactions are as follows:For $AgNO_3$: $2Ag^+ + H_2S \rightarrow Ag_2S(s) + 2H^+$. Here,$2 \ mol$ of $Ag^+$ react with $1 \ mol$

Vedclass · Accepted Answer

$1:2$

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(A) The precipitation reactions are as follows:For $AgNO_3$: $2Ag^+ + H_2S \rightarrow Ag_2S(s) + 2H^+$. Here,$2 \ mol$ of $Ag^+$ react with $1 \ mol$ of $H_2S$.For $CuSO_4$: $Cu^{2+} + H_2S \rightarrow CuS(s) + 2H^+$. Here,$1 \ mol$ of $Cu^{2+}$ reacts with $1 \ mol$ of $H_2S$.Given $100 \ mL$ of $1 \ M$ $AgNO_3$ contains $0.1 \ mol$ of $Ag^+$,requiring $0.05 \ mol$ of $H_2S$.Given $100 \ mL$ of $1 \ M$ $CuSO_4$ contains $0.1 \ mol$ of $Cu^{2+}$,requiring $0.1 \ mol$ of $H_2S$.The ratio of $H_2S$ required is $0.05 : 0.1 = 1:2$.

The ratio of amounts of $H_2S$ needed to precipitate all the metal ions from $100 \ mL$ of $1 \ M$ $AgNO_3$ and $100 \ mL$ of $1 \ M$ $CuSO_4$ is

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