Calculate the solubility of `A_2X_3` in pure water, assuming that neither kind of ion reacts with water. The solubility product of `A_2X_3,K_sp = 1.1 xx 10^(-23)`

Calculate the molar solubility of Ni(OH)_2 in 0.10 M NaOH. The solubility product of Ni(OH)_2 is 2.0 xx 10^(-15) .

The solubility of A_2X_3 is 'y' mol dm^(-3) its solubility product is -

AgCl is dissolved separately in pure water and in 0.025(M) NaCl solution. Find the ratio of concentrations of Ag^(+) ion in pure water and in the NaCl solution. The solubility product of AgCl is 1.75xx10^(-10) .

Calculate the solubility of SrSO_4 in water in mol*L^(-1) at 25^(@)C . ( solubility product of SrSO_4 at 25^(@)C=7.6xx10^(-7)mol^2.L^(-2) )

The solubility of Ag_2CrO_4 in an aqueous solution of AgNO_3 is ___________ than its solubility in pure water.

Solubility of ZnSO_(4) in water is x mol * L^(-1) . Give the mathematical expression of solubility product of the compound .

Determine the solubilities of silver chromate, barium chromate, ferric hydroxide, lead chloride and mercurous iodide at 298K from their solubility product constant given in the standard table. Determine also the molarities of individual ions. Silver chromate, 1.1×10 −12 Barium chromate, 1.2×10 −10 Ferric hydroxide, 1.0×10 −38 Lead dichloride, 1.6×10 −5 Mercurous iodide, 4.5×10 −29

If the solubility of Ca_3(PO_4)_2 in water be y mol L^(-1) , the solubility product of the salt will be -