Solubility of AgCl in 0.2 M NaCl is x and that in 0.1 M `AgNO_(3)` is y. Then which of the following is correct?

If S_(0), S_(1), S_(2) , and S_(3) are the solubility of AgCI in water, 0.01M CaCI_(2), 0.01M NaCI 1, and 0.5M AgNO_(3) solutions, respectively, then which of the following is true ?

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

A sol of Agl is prepared by mixing equal volumes of 0.01 M AgNO_(3) and 0.2 M Kl , which of the following statement is correct ?

The solubility of AgCl in 0.1 M NaCl is ( K_(sp) of AgCl = 1.2 xx 10^(-10) )

Solubility of AgBr in water is S_(1), in "0.01 M "CaBr_(2) is S_(2) in 0.01 M NaBr is S_(3) and in 0.05 M AgNO_(3) is S_(4) . The correct order of these solubilities is :

If the solubility of AgCl in 0.1 M NaCl is ( K_(sp) of AgCl = 1.2 xx 10^(-10) )

If solubility of AgCl(s) in water is 10^-5 M then the solubility of AgCl in 0.1 M AgNO_3 will be

If solubility of AgCl(s) in water is 10^-5 M then the solubility of AgCl in 0.1 M AgNO_3 will be