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))`

A solution is saturated in SrCO_(3) and SrF_(2) The CO_(3)^(2-) was found to be 10^(-3) mol/L. If the concentratuonof F^(-) in solution is represented as yxx10^(-2) M then what is the value of y ? ["Given" : K_(sp)(SrCO_(3))=2.5xx10^(-10),K_(sp)(SrF_(2))=10^(-10)]

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

Solubility of AgCl in 0.1 M CaCl_2 solution will be ( K_(sp) of AgCl= 1.8×(10)^(-10) )

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

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

Determine the solubility of AgCl in 0.1 M BaCl_2 [K_(sp)" for "AgCl=1 xx 10^(-10)]

Solubility of AgCl in 0.2 M magnesium chloride will be (K_sp of AgCl = 1.8 x 10^(-10))

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?