Consider the equilibrium,
`AgCl_(s) harr Ag^+ + Cl_-` the solubility of AgCl is `1.06 xx 10^-5 molL^-1` at 298K. Find out its `K_sp` at this temperature.

When some sodium acetate is added to a solution of acetic acid, the concentration of unionised acetic acid increases. consider the equilibrium, AgCl(s) harr Ag^+(aq) + Cl^-(aq) The solubility AgCl is 1.06xx10^-5 mol//L at 298K. Find out its K_(sp) at this temperature.

The solubility product of PbCl_2 is 1.68xx10^-6 at 298K. Calculate its solubility at this temperature.

Lead chloride has a solubility product of '1.7 xx 10^(-5)' at '298 K .' Calculate its solubility at this temperature.

Calculate the solubility (S) of CaSO_4 at 298K if its solubility product constant (K_(sp)) at this temperature is 9xx10^-6

For the equilibrium, PCl_(5(g)) rarr PCl_(3(g)) + Cl_(2(g)) , (K = 1.8x10^-7) . DeltaG^0 for the reaction at 298K?

The solubility of AgCl in water at '25^circ C' is found to be '1.06 xx 10^(-5)' moles per litre. Calculate the solubility product of AgCl at this temperature.

The solubility product of silver chloride is 1.2xx10^(-10) at 298K. Calculate the solubility of AgCI at 298K.

The solubility of Mg(OH)_2 at 298K is 1.5xx10^-4 . Calculate the solubility product.

Consider the cell Ag| AgBr Br^(-) ||CI|AgCl Ag at 25^(@) C the solubility product of AgCl and AgBr are 1xx10^(@) and 5xx10^(-13) respectively. At which ratio of concentration of Br and Clions would the emf of cell be zero?