What is the `K_(sp)` of `AgCl` if it is given that solubility of `AgCl` at `20^(@)C` is `1.435xx10^(-5)g//L`?

K_(sp) of AgCl is

The concentration of Ag^(+) ion in a given saturated solution of AgCl at 25^(@)C is 1.06xx10^(-5)g ion per litre. Thus, the solubility product of AgCl is :

The concentration of Ag^(+) ions in a given saturated solution of AgCl at 25^(@)C is 1.06 xx 10^(-5) g ion per litre. The solubility product of AgCl is

What will be the solubility of AgCl in 0.05 M NaCl aqueous solution if solubility product of AgCl is 1.5xx10^(-10) ?

What will be the solubility of AgCl in 0.05 M NaCl aqueous solution if solubility product of AgCl is 1.5xx10^(-10) ?

The solubility of AgCl in 0.2 M NaCl is [K_(sp) AgCl =1.8 xx 10^(-10)]

K_(sp) of AgCl is 1xx10^(-10) . Its solubility in 0.1 M KNO_(3) will be :

K_(sp) of AgCl is 1xx10^(-10) . Its solubility in 0.1 M KNO_(3) will be :