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

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) )

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

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) )

What is the molar solubility of Ag_(2)CO_(3)(K_(sp)=4xx10^(-13)) in 0.1M Na_(2)CO_(3) solution ?

What is the molar solubility of Ag_(2)CO_(3)(K_(sp)=4xx10^(-13)) in 0.1M Na_(2)CO_(3) solution ?

What is the molar solubility of Ag_(2)CO_(3)(K_(sp)=4xx10^(-13)) in 0.1M Na_(2)CO_(3) solution ?

Given that solubility product of BaSO_(4) is 1 xx 10^(-10) will be precipiate from when a. Equal volumes of 2 xx 10^(-3)M BaC1_(2) solution and 2 xx 10^(-4)M Na_(2)SO_(4) solution, are mixed? b. Equal volumes of 2 xx 10^(-8) M BaC1_(2) solution and 2 xx 10^(-3)M Na_(2)SO_(4) solution, are mixed? c. 100mL of 10^(-3)M BaC1_(2) and 400mL of 10^(-6)M Na_(2)SO_(4) are mixed.

If the solubility of CaSO_(4) in H_(2)O is 10^(-5)M , Calculate the solubility in 0.005M solution of H_(2)SO_(4) .