The equilibrium 2 Cu^{+} rightleftharpoons Cu | vedclass

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(A) The equilibrium $2 Cu^{+} \rightleftharpoons Cu + Cu^{2+}$ shifts to the left if the concentration of $Cu^{+}$ is increased or the concentration o

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$(B, C, D)$

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(A) The equilibrium $2 Cu^{+} \rightleftharpoons Cu + Cu^{2+}$ shifts to the left if the concentration of $Cu^{+}$ is increased or the concentration of $Cu^{2+}$ is decreased,or if $Cu^{+}$ is removed from the solution by precipitation or complexation.$Cu(I)$ forms insoluble compounds such as $CuCl$,$CuCN$,and $CuSCN$.When $Cl^{-}$,$CN^{-}$,or $SCN^{-}$ are added,they react with $Cu^{+}$ to form these insoluble precipitates,effectively removing $Cu^{+}$ from the equilibrium mixture.According to Le Chatelier's principle,removing a product (or in this case,a reactant $Cu^{+}$) shifts the equilibrium to the left (backward direction) to counteract the change.Therefore,the presence of $Cl^{-}$,$SCN^{-}$,and $CN^{-}$ shifts the equilibrium to the left.

The equilibrium $2 Cu^{+} \rightleftharpoons Cu + Cu^{2+}$ in aqueous medium at $25^{\circ} C$ shifts towards the left in the presence of
$(A)$ $NO_3^{-}$ $(B)$ $Cl^{-}$ $(C)$ $SCN^{-}$ $(D)$ $CN^{-}$

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The equilibrium $2 Cu^{+} \rightleftharpoons Cu + Cu^{2+}$ in aqueous medium at $25^{\circ} C$ shifts towards the left in the presence of$(A)$ $NO_3^{-}$ $(B)$ $Cl^{-}$ $(C)$ $SCN^{-}$ $(D)$ $CN^{-}$