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Calculate pH at which Mg(OH)(2) begins t...

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))`

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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) .

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Calculate pH of a saturated solution of Mg(OH)_(2) . (K_(SP)for Mg(OH)_(2)=8.9xx10^(-12))

Should Mg(OH)_(2) precipitate from a solution that is 0.01 M MgCl_(2) if the solution is also made 0.10 M in NH_(3)[K_((sp)[Mg(OH)_(2)])=1.8 xx10^(-11) , K_(b(NH_(4)OH))= 1.8 xx 10^(-5)]

Calculate [overset(o+)NH_(4)] (derived from NH_(4)C1) needed to prevent Mg(OH)_(2) from precipitating is 1.0L of solution which contins 0.01mol NH_(3) and 0.001 mol Mg^(2+). K_(sp) Mg(OH)_(2) = 1.2 xx 10^(-11), K_(b) NH_(3) = 1.8 xx 10^(-5) .

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) .