Find the solubility product of a saturated solution of `Ag_(2)CrO_(4)` in water at `298K`, if the `EMF` of the cell `:`
`Ag|Ag^(o+)(satAg_(2)CrO_(4)sol)||Ag(0.1M)|Agis 0.164V` at `298K`.

(A)Find the solubility product of a saturated solution of Ag_(2)CrO_(4) in water at 298 K if the emf of the cell Ag|Ag+ (saturated. Ag_(2)CrO_(4) solution) || Ag+ (0.1 M) | Ag is 0.164 V at 298 K. (B) What will be the resultant pH when 200 mL of an aqueous solution of HCl (pH = 2.0) is mixed with 300 mL of an aqueous of NaOH (pH = 12.0) ?

A saturated solution of Ag_(2)SO_(4) is 2.5 xx 10^(-2)M . The value of its solubility product is

The concentration of Ag^(o+) ions in a saturated solution of Ag_(2)C_(2)O_(4) is 2.2 xx 10^(-4)M . Calculate the solubility product of Ag_(2)C_(2)O_(4)

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Write the expressions of solubility products for the following salts . Ag_2CrO_4, Ca_3(PO_4) _2.

The K_(sp) of Ag_(2)CrO_(4) is 1.1xx10^(-12) at 298K . The solubility (in mol/L) of Ag_(2)CrO_(4) in a 0.1 M AgNO_(3) solution is

The solubility product of Ag CrO_(4) is 32xx10^(-12). What is the concentration of CrO_(4)^(2-) ions in that solution ?

The solubility product of PbCl_(2) at 298K is 1.7 xx 10^(-5) . Calculate the solubility of PbCl_(2) in g L^(-1) at 298K

At 20^(@)C , the Ag^(+) ion concentration in a saturated solution Ag_(2)CrO_(4) is 1.5 x10^(-4) mol // litre. At 20^(@)C , the solubility product of Ag_(2)CrO_(4) would be

The concentration of Ag^(o+) ions in a saturated solution of Ag_(2)C_(2)O_(4) is 2.0 xx 10^(-4)M . Calculate the solubility of Ag_(2)C_(2)O_(4) in a solution which is 0.01M in H_(2)C_(2)O_(4) .