What is the minimum pH of a solution of 0.1 M in `Mg^(2+)` from which `Mg(OH)_(2)` will not precipitate `K_(sp) =1.2 xx 10^(-11) M^(3).`

The maximum pH of a solution which is 0.10 M is Mg^(2+) from which Mg(OH)_(2) is not precipitated is [ K_(sp) of Mg(OH)_(2) = 1.2 xx 10^(-11) M^(3) ]

The maximum pH of a solution which is 0.10 M in Mg ^(2+ ) from which Mg (OH) _ 2 is not precipitated is : ( Given K_(sp) " of " Mg (OH)_2 =1.2 xx 10^(-11) M)

The maximum pH of a solution which is having 0.10M in Mg^(2+) and from which Mg(OH)_(2) is not precipated is: (Given K_(sp)Mg(OH)_(2)=4xx10^(-11)M^(3)){log2=0.30}

The maximum pH of a solution which is having 0.10M in Mg^(2+) and from which Mg(OH)_(2) is not precipated is: (Given K_(sp)Mg)(OH)_(2)=4xx10^(11)M^(3)){log2=0.30}

If K_(sp) of Mg(OH)_(2) is 1.2 xx 10^(-11) . Then the highest pH of the 0.1 M solution of Mg^(2+) ion from which Mg(OH)_(2) is not precipitated is

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

What is the solubility of Mg(OH)_2 in mole per litre if K_p = 1.0 xx 10^-11 ?

What is the pH value at which Mg(OH)_(2) begins to precipitate from a solution containing 0.2 M Mg^(+2) ions ? K_(SP) of Mg(OH)_(2) is 2 xx 10^(-13) M^(2) ?