Selective precipitation of ions in a mixture in the form of salts can be adding common ions gradually. Let us condsider selective precipitation of `CI^(-)` and `CrO_(4)^(2-)`ions in the form of AgCl and `Ag_(2)Cro_(4)` form a mixture having having 0.01M `CI^(-)` and 0.01M `CrO_(4)^(2-)`. For this, salt having `Ag^(+)` [like `AgNO_(3)(s)`] is added gradually. Given : `K_(sp) [AgCI]=10^(-10)` and `K_(sp)[Ag_(2)CrO_(4)]=4xx10^(-14)`
Minimum concentration of `Ag^(+)` ion at which precipitation of at least one ion starts.

Selective precipitation of ions in a mixture in the form of salts can be adding common ions gradually. Let us condsider selective precipitation of CI^(-) and CrO_(4)^(2-) ions in the form of AgCl and Ag_(2)Cro_(4) form a mixture having having 0.01M CI^(-) and 0.01M CrO_(4)^(2-) . For this, salt having Ag^(+) [like AgNO_(3)(s) ] is added gradually. Given : K_(sp) [AgCI]=10^(-10) and K_(sp)[Ag_(2)CrO_(4)]=4xx10^(-14)] The percentage of one ion precipitated when another ion starts precipitation is : (Given: (1)/(sqrt2)=0.7 )

The solubility product of Ag CrO_(4) is 32xx10^(-12). What is the concentration of CrO_(4)^(2-) ions in that solution ?

The solubility product of Ag CrO_(4) is 32xx10^(-12). What is the concentration of CrO_(4)^(2-) ions in that solution ?

A solution is 0.1 M in Cl^(-) and 0.001 M in CrO_(4)^(2-) . Solid AgNO_(3) is gradually added to it. Assuming that the addition does not change in volume and K_(SP) (AgCl) = 1.7 xx 10^(-10) M^(2) and K_(SP)(Ag_(2)CrO_(4)) = 1.9 xx 10^(-12) M^(3) . Select correct statement from the following:

A solution contains 0.05M of each of NaCl and Na_(2),CrO_(4) ,. Solid AgNO_(3) , is gradually added to it. Whichof the following facts true (Given: K_(sp)(AgCl) = 1.7xx 106(-10) M^(2) and K_(sp)(Ag_(2),CrO_(4),) = 1.9 xx 10^(-12) M^(3) :

To an aqueous solution of Ag_(2)CrO_(4) above its own precipitate , CrO_(4)^(2-) ions are added in the form of solution. This results in