`Ksp` of `M(OH)_(2)` is `5 xx 10^(-16)` at `25^(0)C`. The pH of its saturated solution at `25^(0)C` is

The K_(sp) of Ca(OH)_(2) is 4.42 xx 10^(-5) at 25^(@)C . A 500 ml of saturated solution of Ca(OH)_(2) is mixed with an equal volume of 0.4M NaOH . How much Ca(OH)_(2) in mg is precipitated ?

The K_(sp) of Mg(OH)_(2) is 8.9 xx 10^(-12) at 25^(2)C . the pH of solution is adjusted to 9 . How much Mg^(2+) ion will be precipitated as Mg(OH)_(2) from a 0.1M MgCl_(2) solution at 25^(@)C ? Assume that MgCl_(2) is completely dissociated.

The solubility product of Mn(OH)_2 at 25^@C is 1.9xx10^(-13) . What is the pOH of the saturated solution of Mn(OH)_2 at 25^@C .

The pH of a 0.02 M Ca(OH)_2 solution of 25^@C is :

The solubility product (K_sp) of Ca(OH)_2 at 25^(@)C is 4.42xx10^(-5) . A 500 mL of saturated solution of Ca(OH)2 is mixed with equal volume of 0.4(M) NaOH. How much Ca(OH)_2 in milligrams is precipitated?

K_(b) for NH_(4)OH is 1.81xx10^(-5) . The pH of 0.01 M NH_(4)Cl solution at 25^(@)C is :

The solubility product K_(sp) of Ca (OH)_2 " at " 25^(@) C " is " 4.42 xx 10 ^(-5) A 500 mL of saturated solution of Ca(OH)_2 is mixed with equal volume of 0.4 M NaOH . How much Ca(OH)_2 in milligrams is precipitated?

The pH of 0.25 M Ba(OH)_2 solution is: