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}

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).

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) ?

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) ?

Which of the following concentration of NH_(4)^(+) will be sufficient to present the precipitation of Mg(OH)_(2) form a solution which is 0.01 M MgCl_(2) and 0.1 M NH_(3)(aq) . Given that K_(sp)Mg(OH)_(2)=2.5xx10^(-11) and K_(b) for NH_(3) = 2xx10^(-5) .