In an aqueous solution `10^(-2)` M `Na_(2)SO_(4)` and `10^(-2)` M NaI are present. Now pure `Pb(NO_(3))_(2)` is added gradually then calculate concentration of `SO_(4)^(2-)` when `PbI_(2)` start precipitating in solution [`K_(sp) (PbI_(2))=10^(-9)` and `K_(sp)(PbSO_(4))=10^(-8)`].

A solution containing 10^(-2) M MgCl_(2) will just form precipitate when pH in the solution is : K_(sp)(Mg(OH)_(2))=10^(-12)

A solution of 0.1 M in Cl^(-) and 10^(-4) M CrO_(4)^(-2) . If solid AgNO_(3) is gradually added to this solution, what will be the concentration of Cl^(-) when Ag_(2)CrO_(4) begins to precipitate? [K_(sp)(AgCl)=10^(-10)M^(2),K_(sp)(Ag_(2)CrO_(4))=10^(-12) M^(3)]

Solid Na_(2)SO_(4) is slowly added to a solution which is 0.020 M in Ba(NO_(3))_(2) and 0.020 M is Pb(NO_(3))_(2) . Assume that there is no increase in volume on adding Na_(2)SO_(4) . There preferential precipitation takes place. What is the concentration of Ba^(2+) when PbSO_(4) starts to precipitate? [K_(sp)(BaSO_(4))=1.0xx10^(-10) and K_(sp)(PbSO_(4))=1.6xx10^(-8)]

Solid Na_(2)SO_(4) is slowly added to a solution which is 0.020 M in Ba(NO_(3))_(2) and 0.020 M is Pb(NO_(3))_(2) . Assume that there is no increase in volume on adding Na_(2)SO_(4) . There preferential precipitation takes place. What is the concentration of Ba^(2+) when PbSO_(4) starts to precipitate? [K_(sp)(BaSO_(4))=1.0xx10^(-10) and K_(sp)(PbSO_(4))=1.6xx10^(-8)]

What is minimum concentration of SO_(4)^(2-) required to precipitate BaSO_(4) in solution containing 1 xx 10^(-4) mole of Ba^(2+) ? ( K_(sp) of BaSO_(4) = 4 xx 10^(-10) )

What is minimum concentration of SO_(4)^(2-) required to precipitate BaSO_(4) in solution containing 1 xx 10^(-4) mole of Ba^(2+) ? ( K_(sp) of BaSO_(4) = 4 xx 10^(-10) )

Calculate the concentration of SO_4^(2-) ions necessary to cause the precipitation of BaSO_4 (K_(sp)=1.5xx10^(-9)) from solution of BaCl_2 (0.5 M)