The solubility of `PbSO_(4)` in `0.1M Na_(2)SO_(4)` solution is (`K_(sp)` of `PbSO_(4)` is `1.25 xx 10^(-9)`)

What is the solubility of PbSO_(4) in 0.01M Na_(2)SO_(4) solution if K_(sp) for PbSO_(4) = 1.25 xx 10^(-9) ?

What is the solubility of PbSO_(4) in 0.01M Na_(2)SO_(4) solution if K_(sp) for PbSO_(4) = 1.25 xx 10^(-9) ?

The solubility of PbSO_4 "in" 0.01 M Na_2SO_4 solution is (K_(sp) of PbSO_4 is 1.25 xx 10^(-9) )

If the solubility of Ag_(2)SO_(4) in 10^(-2)M Na_(2)SO_(4) solution be 2xx10^(-8)M then K_(sp) of Ag_(2)SO_(4) will be

If the solubility of Ag_(2)SO_(4) in 10^(-2)M Na_(2)SO_(4) solution be 2xx10^(-8)M then K_(sp) of Ag_(2)SO_(4) will be

If the solubility of Ag_(2)SO_(4) in 10^(-2)M Na_(2)SO_(4) solution be 2xx10^(-8)M then K_(sp) of Ag_(2)SO_(4) will be

STATEMENT-1: Solubility of BaSO_(4) in 0.1 M Na_(2)SO_(4)is 10^(-9) M hence its K_(sp) is 10^(-18). STATEMENT-2: In aqueous solution, solubility product of BaSO_(4)=S^(2). (Where S is solubility of BaSO_(4) )

STATEMENT-1: Solubility of BaSO_(4) in 0.1 M Na_(2)SO_(4)is 10^(-9) M hence its K_(sp) is 10^(-18). STATEMENT-2: In aqueous solution, solubility product of BaSO_(4)=S^(2). (Where S is solubility of BaSO_(4) )

Solubility of Ag_(2)CrO_(4) ( K_(sp)=4xx10^(-13) ) in 0.1 M K_(2)CrO_(4) solution will be :