Two sparnigly soluble salts AX and BX_(2) have their solubility product constant equal . Which of the following is (are) correct deduction(s) ?

Two sparnigly soluble salts AX and BX_(2) have their solubility produc

1.	Two sparnigly soluble salts AX and BX_(2) have their solubility product constant equal . Which of the following is (are) correct deduction(s) ?
Answer» Solubility of `AX` ISW greater than solubility of `BX_(2)`. If `S_(1)` and `S_(2)` are molar solubility of `AX` and `BX_(2)` then `S_(1) = (S_(2))^(3//2)` If X is a conjugate BASE of a weak acid, addition of `HNO_(3)` will increase solubility of both AX with `BX_(2)`. INCREASING the temperature, increase the solublity of both `AX` and `BX_(2)`. Solution :`K_(sp) = (AX) = S_(1)^(2)` `K_(sp) = (BX)_(2) = 4S_(2)^(3)` If `S_(1)^(2) = 4S_(2)^(3)`, then `S_(1) = sqrt(4S_(2)^(3)) = 2(S_(2))^(3//2)` `S_(1) gt S_(2)`