The solubility product of `Cr(OH)_(3)` at 298 K is `6.0xx10^(-31)`. The concentration of hydroxide ions in a saturated solution of `Cr(OH)_(3)` will be :

The solubility product of HgCl_(2) at room temperature is 4.0 xx 10^(-5) . The concentration of Cl^(-) ion in the saturated solution will be

The solubility of Pb (OH)_2 in pure water in pure water is 20/3xx10^(-6)M . Calculate concentration of OH^(-) ion in a buffer solution of P^(H)=8 .

The solubility of Mg(OH)_2 at 298K is 1.5xx10^-4 . Calculate the solubility product.

Solubility product of Ba(OH)_2 is 5.0.* 10^(-7) . pOH of saturated solution of Ba(OH)_2 is

Solubility product of Ba(OH)_2 is 5.01×10^(-7) ,pOH of saturated solution of Ba(OH)_2 is

the solubility product of Al(OH)_3 is 1xx10^-36 . Calculate the solubility of Al(OH)_3.

The solubility product of Fe(OH)_3 is 1xx10^(-36) What is the minimum concentration of OH^- ions required to precipitate Fe(OH)_3 from a 0.001 M solution of FeCl_3 ?

The solubility product of Fe(OH)_3 is 1xx10^(-36) What is the minimum concentration of OH^- ions required to precipitate Fe(OH)_3 from a 0.001 M solution of FeCl_3 ?

The solubility of Sr(OH)_(2) at 298K is 19.23 g/L of solution. Calculate the concentrations of stronium and hydroxyl ions and the pH of the solution.

The solubility of Sr(OH)_2 at 298 K is 19.23g//L of solution. Calculate the concentration of strontium and hydroxyl ions and the pH of the solution.