What is the pH at which `Mg(OH)_(2)` begins to precipitate from a solution containing 0.1 M `Mg^(2+)` ions ? `[K_(sp)" for "Mg(OH)_(2)=1.0xx10^(-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))

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) .

What is the ratio of moles of Mg(OH)_(2) and Al(OH)_(3) , present in 1L saturated solution of Mg(OH)_(2) and Al(OH)_(3) K_(sp) of Mg(OH)_(2)=4xx10^(-12) and K_(sp) of Al(OH)_(3)=1xx10^(-33) .[Report answer by multiplying 10^(-18)]

What is the concentration of Ba^(2+) when BaF_(2) (K_(sp)=1.0xx10^(-6)) begins to precipitate from a solution that is 0.30 M F^(-) ?

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

pH of a saturated solution of M (OH)_(2) is 13 . Hence K_(sp) of M(OH)_(2) is :

What is the concentration of Pb^(2+) when PbSO_(4) (K_(sp)=1.8xx10^(-8)) begins to precipitate from a solution that is 0.0045 M in SO_(4)^(2-) ?

Will a precipitate of Mg(OH)_(2) be formed in a 0.001 M solution of Mg(NO_(3)) , if the pH of solution is adjusted to 9 ? K_(sp) of Mg(OH)_(2)= 8.9 xx 10^(-12) .

A solution has 0.05M Mg^(2+) and 0.05M NH_(3) . Calculate the concentration of NH_(4)CI required to prevent the formation of Mg(Oh)_(2) in solution. K_(SP) for Mg(OH)_(2)=9.0xx10^(-12) and ionisation constant of NH_(3) is 1.8xx10^(-5) .