If s is the molar solubility of `Ag_2SO_4`, then

Sparingly soluble salts maintains their solubility product value in their saturated solutions irrespective of the sources of the ions . what is the molar solubility of AgNO_3 in a 0.1 M H_2S solution buffered at pH= 2 (K_1 and K_2 " of " H_2S " are " 10^(4) and 10^(-8) respectively) (K_(sp) " of " Ag_2S = 4xx 10^(-13) ) (Note : No Ag_2S precipitate should be formed)

If the solubility of AI_2(SO_4) is S , then its solubility product is

If the solubility of Al_2(SO_4)_3 is S , then its solubility product is

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

Determine the molar solubility of MgF_(2) from its solubility product K_(sp)=4xx10^(-9) :

If the solubility of Ag_(2)CrO_(4) in water is C mole/litre, Its solubility product will be

The K_(sp) for a sparingly soluble Ag_2CrO_4 is 4xx10^(-12) . The molar solubility of the salt is

The K_(sp) for a sparingly soluble Ag_2CrO_4 is 4xx10^(-12) . The molar solubility of the salt is