The solubility product of `BaCrO_(4)` is `2.4xx10^(-10)M^(2)`. The maximum concentration of `Ba(N0_(3))_(2)` possible without precipitation in a `6xx10^(-4)` M `K_(2)CrO_(4)` solution is :

The K_(sp) of BaCrO_(4) is 2.4xx10^(-10)M^(2) . The maximum concentration of Ba(NO_(3))_(2) possible without precipitation in a 6xx10^(-4)M K_(2)CrO_(4) solution is

The solubility product of BaCrO _(4) is 2.4 xx 10 ^(-10). The maximum concentration of Ba (NO _(3)) _(2) possible without precipitation in a 6 xx 10 ^(-4) M K _(2) Cr O _(4) 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 Ag CrO_(4) is 32xx10^(-12). What is the concentration of CrO_(4)^(2-) ions in that solution ?

Given that solubility product of BaSO_(4) is 1 xx 10^(-10) will be precipiate from when a. Equal volumes of 2 xx 10^(-3)M BaC1_(2) solution and 2 xx 10^(-4)M Na_(2)SO_(4) solution, are mixed? b. Equal volumes of 2 xx 10^(-8) M BaC1_(2) solution and 2 xx 10^(-3)M Na_(2)SO_(4) solution, are mixed? c. 100mL of 10^(-3)M BaC1_(2) and 400mL of 10^(-6)M Na_(2)SO_(4) are mixed.

The solubility product of BaSO_(4)" at " 25^(@) C " is " 1.0 xx 10^(-9) . What would be the concentration of H_(2)SO_(4) necessary to precipitate BaSO_(4) from a solution of 0.01" M Ba"^(+2) ions

The solubility product of BaSO_(4)" at " 25^(@) C " is " 1.0 xx 10^(-9) . What would be the concentration of H_(2)SO_(4) necessary to precipitate BaSO_(4) from a solution of 0.01" M Ba"^(+2) ions