Equal volumes of 0.02 M `AgNO_3` and 0.02 M HCN were mixed. Calculate `[Ag^+]` at equilibrium. Take `K_(a)(HCN)=9 xx 10^(-10), K_(sp) (AgCN)=4 xx 10^(-6)`

Equal volumes of 0.02M AgNO_(3) and 0.01M HCN are mixed. Calculate [Ag^(o+)] in solution after attaining equilibrium. K_(a) HCN = 6.2 xx 10^(-10) and K_(sp) of AgCN = 2.2 xx 10^(-16) .

Equal volumes of 0.02M AgNO_(3) and 0.01M HCN are mixed. Calculate [Ag^(o+)] in solution after attaining equilibrium. K_(a) HCN = 6.2 xx 10^(-10) and K_(sp) of AgCN = 2.2 xx 10^(-16) .

Equal volume of 0.02 M KCl and 0.02 M K[Ag(CN)_(2)] are mixed , then the precipitate of AgCl will Ksp AgCl = 1.5 xx 10^(-10) K (K[Ag (CN)_(2)]) = 4xx 10^(-22)

Equal volume of 0.02 M KCl and 0.02 M K[Ag(CN)_(2)] are mixed , then the precipitate of AgCl will Ksp AgCl = 1.5 xx 10^(-10) K (K[Ag (CN)_(2)]) = 4xx 10^(-22)

Equal volumes of 0.02M CaC1_(2) and 0.0004M Na_(2)SO_(4) are mixed. Will a precipitate form? K_(sp) for CaSO_(4) = 2.4 xx 10^(-5) ?