A solution containing both `Zn^(2+)` and `Mn^(2+)` ions at a concentration of `0.01M` is saturated with `H_(2)S`. What is pH at which MnS will form a ppt ? Under these conditions what will be the concentration of `Zn^(2+)` ions remaining in the solution ? Given `K_(sp)` of `ZnS is 10^(-22)` and `K_(sp)` of MnS is `5.6 xx 10^(-16), K_(1) xx K_(2)` of `H_(2)S = 1.10 xx 10^(-21)`.

A solution contains 0.10 M H_2S and 0.3 HCl Calculate the concentration of S^(2-) and HS^(-) ions in the solution . For H_2S , K_(a_1) = 1 xx 10^(-7) and K_(a_2) = 1.3 xx 10^(-13)

Calculate the concentration of silver ion, if water is saturated with AgCNS (K_(sp) =1 xx 10^(-12)) and AgBr (K_(sp) = 5 xx 10^(-13) ).

What is the minimum pH required to prevent the precipitation of Zn^(+2) in a solution that is 0.01 M ZnCl_(2) and saturated with 0.1 M H_(2) S (Given : K_(sp) ZnS = 10^(-21) and Ka_(1) xx Ka_(2) of H_(2)S = 10^(-20) )

What is the minimum pH required to prevent the precipitation of Zn^(+2) in a solution that is 0.05 M ZnCl_(2) and saturated with 0.2M H_(2)S (Given : K_(sp) ( ZnS) = 10^(-20) and Ka_(1) xx Ka_(2) of H_(2)S = 10^(-20) )

It is given that 0.001 mol each of Cd^(2+) and Fe^(2+) ions are contained in 1.0L of 0.02M HC1 solution. This solutions is now saturated with H_(2)S gas at 25^(@)C . a. Determine whether or not each of these ions will be precipitated as sulphide? b. How much Cd^(2+) ions remains in the solution at equilibrium? K_(1)(H_(2)S) = 1.0 xx 10^(-7), K_(2) (H_(2)S) = 1.0 xx 10^(-14) : ltbRgt K_(sp) (CdS) = 8 xx 10^(-27): K_(sp) (FeS) = 3.7 xx 10^(-19) .

It is given that 0.001 mol each of Cd^(2+) and Fe^(2+) ions are contained in 1.0L of 0.02M HC1 solution. This solutions is now saturated with H_(2)S gas at 25^(@)C . a. Determine whether or not each of these ions will be precipitated as sulphide? b. How much Cd^(2+) ions remains in the solution at equilibrium? K_(1)(H_(2)S) = 1.0 xx 10^(-7), K_(2) (H_(2)S) = 1.0 xx 10^(-14) : ltbRgt K_(sp) (CdS) = 8 xx 10^(-27): K_(sp) (FeS) = 3.7 xx 10^(-19) .