Calculate the concentration of `Mg^(2+)` ions and `OH^(-)` ions in a saturated soluton of `Mg(OH)_(2)`.The solubility product of `Mg(OH)_(2) " is " 9.0 xx 10^(-12)`

The solubility product of Mg(OH)_(2) may be written as :

The pH of an aqueous solution of Mg(OH)_(2) is 9.0. If the solubility product of Mg(OH)_(2) is 1xx10^(-11) , what is [Mg^(2+)] ?

Mg(OH)_(2) is precipitated when NaOH is added to a solution of Mg^(2+) . If the final concentration of Mg^(2+) is 10^(-10) .M, the concetration of OH^(-) (M) is the solution is b [Solubility product for Mg(OH)_(2)=5.6xx10^(-12) ]

Calculate pH of saturated solution Mg(OH)_(2),K_(sp) for Mg(OH)_(2) is 8.9 xx 10^(-12) .

Calculate pH of saturated solution Mg(OH)_(2),K_(sp) for Mg(OH)_(2) is 8.9 xx 10^(-12) .

Find the PH of saturated solution of Mg(OH)_2 [K_p of Mg(OH_2)= 8.9xx 10^(-12)]

A saturated solution of Mg(OH)_(2) in water at 25^(@)C contains 0.11g Mg(OH)_(2) per litre of solution . The solubility product of Mg(OH)_(2) is :-

A saturated soltion of Mg(OH)_(2) in water at 25^(@)C contains 0.11g Mg(OH)_(2) per litre of solution . The solubility product of Mg(OH)_(2) is :-

What is the pH of saturated solution of Mg(OH)_(2) ? Ksp for Mg(OH)2=1.8*10^-11

A saturated solution of Mg(OH)_2 in water at 25^oC contains 0.11 g Mg(OH)_2 per litre of solution. The solubility product of Mg(OH)_2 is :