The solubility of `PbI_2` in 0.1M `Pb(NO_3)_2 Solution is Xxx 10^(_2) then value of X is [Given `K_(sp) (PbI_2) = 8xx10^(-9)`

The molar solubility of PbI_(2) in 0.2 M Pb(NO_(3))_(2) solution in terms of solubility product, K_(sp)

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

The solubility of PbSO_(4) in 0.1M Na_(2)SO_(4) solution is ( K_(sp) of PbSO_(4) is 1.25 xx 10^(-9) )

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

If the solubility of Ag_(2)SO_(4) in 10^(-2)M Na_(2)SO_(4) solution be 2xx10^(-8)M then K_(sp) of Ag_(2)SO_(4) will be

The molar solubility of AgCl in 1.8 M AgNO_(3) solution is ( K_(sp) of AgCl = 1.8 xx 10^(-10) )

If solubility of AgCl in 0.2 M solution of AgNO_(3) is represented as yxx10^(-10) then find the value of y. ("Given": K_(sp(AgCl))=10^(-10))

The solubility of PbI_(2) is 0.0013 M. Then the solubility product of PbI_(2) is