An aqueous solution contains `Ni^(2+), Co^(2+), Pb^(2+)` ions at equal concentrations. The solubility product of NiS, PbS and CoS in water at `25^@C` are respectively given below. Indicate which of these ions will be precipitated first and last when sulphide concentration is progressively increased from zero ?`[K_(sp) of NiS=3xx10^(-19), K_(sp) of CoS=4xx10^(-21), K_(sp) of PbS=3xx10^(-28)`

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) ).

Ag^(+) ion concentration in saturated solution of Ag_(3)PO_(4) (K_(sp)=2.7xx10^(-19)) :

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 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) .

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) .

Sodium chromate solution is gradually added to a mixture containing 0.05 M Pb^(2+) ions and 0.10 M Ba^(2+) ions. The concentration of the ion precipitating first when the second ion begins to form a percipitate is [Note: K_(sp) of BaCrO_(4)=2.4xx10^(-10) and K_(sp) of PbCrO_(4)=1.8xx10^(-14) ]