If the solubility of AgCI (formula mass = 143 g/mole) in water at `25^(@)C` is `1.43 xx 10^(-4)` gm/100 ml of solution then the value of `K_(sp)` will be

K_(sp) of AgCl in water at 25^(@)C is 1.8xx10^(-10) . If 10^(-5) mole of Ag^(+) ions are added to this solution. K_(sp) will be:

K_(sp) of AgCl in water at 25^(@)C is 1.8xx10^(-10) . If 10^(-5) mole of Ag^(+) ions are added to this solution. K_(sp) will be:

The solubility of ML_2 (formula weight, 60 g/mol) in water is 2.4 xx 10^(-5) g/100 mL solution. Calculate solubility product constant for ML2.

The solubility of CuS in pure water at 25^(@)C is 3.3 xx 10^(-4)g L^(-1) . Calculate K_(sp) of CuS . The accurate value of K_(sp) of CuS was found to be 8.5 xx 10^(-36) at 25^(@)C .

The solubility of CuS in pure water at 25^(@)C is 3.3 xx 10^(-4)g L^(-1) . Calculate K_(sp) of CuS . The accurate value of K_(sp) of CuS was found to be 8.5 xx 10^(-36) at 25^(@)C .

The solubility of Ba_3(AsO_4)_2 (formula weight =690 ) is 6.9 xx 10^(-2) g//100 ml. what is the K_(sp) ?

The solubility of AgBrO_(3) (formula mass=236) is 0.0072 g in 1000 mL. What is the K_(sp) ?

The solubility of AgBrO_(3) (formula mass=236) is 0.0072 g in 1000 mL. What is the K_(sp) ?