7.92*10^-15 M solution of Hg^2+ and a saturated solution of H2S at a pH of 0.5. predict whether a precipitate will form.
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5. Use the equilibrium expression for the dissociation of H2S to calculate the concentration of H2S. Show more…
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What must the $\mathrm{pH}$ of a buffered solution saturated with hydrogen sulfide $\left(\left[\mathrm{H}_{2} \mathrm{~S}\right]=0.10 \mathrm{M}\right)$ be at $25^{\circ} \mathrm{C}$ in order to precipitate $\mathrm{PbS}(s)$ leaving $\left[\mathrm{Pb}^{2+}\right]=$ $1.0 \times 10^{-6} \mathrm{M}$, without precipitating any $\mathrm{MnS}(s) ?$ The original solution is $0.025 \mathrm{M}$ in both $\mathrm{Pb}^{2+}(a q)$ and $\mathrm{Mn}^{2+}(a q)$.
A $0.125-M$ solution of $\mathrm{Mn}\left(\mathrm{NO}_{3}\right)_{2}$ is saturated with $\mathrm{H}_{2} \mathrm{S}\left(\left[\mathrm{H}_{2} \mathrm{S}\right]=0.10 \mathrm{M}\right) .$ At what pH does MnS begin to precipitate? $$ \operatorname{Mn} S(s) \rightleftharpoons \operatorname{Mn}^{2+}(a q)+S^{2-}(a q) \quad K_{\mathrm{sp}}=4.3 \times 10^{-22} $$ $$ \mathrm{H}_{2} \mathrm{S}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons 2 \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{S}^{2-(a q)} \qquad K=1.0 \times 10^{-26} $$
A 0.125-M solution of Mn(NO 3)2 is saturated with H_S ([H_S] = 0.10 M). At what pH does MnS begin to precipitate? $$\operatorname{MnS}(s) \rightleftharpoons \mathrm{Mn}^{2+}(a q)+\mathrm{S}^{2-}(a q) \quad K_{\mathrm{sp}}=4.3 \times 10^{-22}$$ $$\mathrm{H}_{2} \mathrm{S}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons 2 \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{S}^{2-}(a q) \quad K=1.0 \times 10^{-26}$$
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