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 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 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) ]

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).

A solution containing 10^(-2) M MgCl_(2) will just form precipitate when pH in the solution is : K_(sp)(Mg(OH)_(2))=10^(-12)

What will be the value of pH at which Mg(OH)_2 starts to precipitate from 0.1(M) of MgCl_2 solution? [K_(sp)[Mg(OH)_2]=1.0xx10^(-11) )

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) .

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) .

Calculate pH at which Mg(OH)_(2) begins to precipitate from a solution containing 0.10M Mg^(2+) ions. (K_(SP)of Mg(OH)_(2)=1xx10^(-11))

Calculate pH at which Mg(OH)_(2) begins to precipitate from a solution containing 0.10M Mg^(2+) ions. (K_(SP)of Mg(OH)_(2)=1xx10^(-11))