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 concentration of 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)]

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

Solubility of AgCl in the solution containing 0.01 M NaCl is [given, K_sp (AgCL)= 1.6 x 10^-10]

The solubility of CH_(3)COOAg (K_(sp)=10^(-10)) in a buffer solution of pH equal to 5 is (sqrt(x))xx10^(-y) . Calculate the value of (x+y) Given : K_(b) (CH_(3)COO^(-)) = 10^(-9) . X and y are integer where 0 lt x lt 10 .

The standard reduction potential of a silver chloride electrode (metal -sparingly soluble salt electrode) is 0.209V and for silver electrode is 0.80V . If the moles of AgCl that can dissolve in 10L of a 0.01M NaCl solution is represented as 10^(-2) then find the value of z .

The solubility product of SrF_(2) in water is 8 xx 10^(-10) Calculate its solubility in 0.1 M of aqueous NaF solution. If its solubility is expressed as y xx 10^(-8) then what is the value of 'y' ?

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

When one litre of a saturated solution of PbCl_(2) (mol. Mass=278) is evaported, the residue is found to weight 2.78g. If K_(sp) of PbCl_(2) is represented as yxx10^(-6) then find the value of y.