`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 A_2B_(3) in water at 25^(@) C . is 1.1 xx 10^(-23) concentration of A^(+) ions is

The solubility of AgCl in water at 10^@C is 6.2 xx 10^-6 mol/litre. The K_sp of AgCl is:

The solubility product (K_(sp)) of AgCI is 1.1 xx 10^(-10) and the concentration of Ag^(+) ions in given solution is 1.0 xx 10^(-7) mole per litre. The concentration CI^(-) for precipitation to occur will be

K_sp of AgCl at 18^@C is 1.8 xx 10^-10. If Ag^+ of solution is 4 xx 10^-3 mol/litre. The Cl^- that must exceed before AgCl is precipitated would be: