`K_(sp)` of `Mg(OH)_(2)` is `1xx10^(-12).0.01` M `MgCl_(2)` will show precipitation is a solution of pH greater than :

The K_(sp) of Mg(OH)_(2) is 1xx10^(-12) . 0.01 M Mg(OH)_(2) will precipitate at the limiting pH

The K_(sp) of Mg(OH)_(2) is 1xx10^(-12) . 0.01 M Mg(OH)_(2) will precipitate at the limiting pH

The K_(sp) of Mg(OH)_(2) is 1xx10^(-12). 0.01M Mg^(2+) will precipitate tate at the limiting pH of

The K_(sp) of Mg(OH)_(2) is 1xx10^(-12). 0.01M Mg^(2+) will precipitate at the limiting pH of

a. Will a precipitate of Mg(OH)_(2) be formed in a 0.001M solution of Mg(NO_(3))_(2) if the pH of solution is adjusted to 9.K_(sp) of Mg(OH)_(2) = 8.9 xx 10^(-12) . b. Calculate pH at which Mg(OH)_(2) begin to precipitae form a solution containing 0.1M Mg^(2+) ions. K_(sp) of Mg(OH)_(2) =1 xx 10^(-11) . c. Calculate [overset(Theta)OH] of a solution after 100mL of 0.1M MgC1_(2) is added to 100mL of 0.2M NaOH. K_(sp) Mg(OH)_(2) = 1.2 xx 10^(-11) .

K_(sp) of Mg(OH)_(2) is 4.0xx10^(-6) . At what minimum pH, Mg^(2+) ions starts precipitating 0.01 MgCl