Will a precipitate of Mg(OH)2 be formed in a 0.002 M solution of Mg(NO

1.	Will a precipitate of Mg(OH)2 be formed in a 0.002 M solution of Mg(NO3)2, if the pH of solution is adjusted to 9 ? Ksp of Mg(OH)2 = 8.9 × 10–12.
Answer» pH = 9 ∴ [H⁺ ] = 10^–9 M or [OH^–] = 10^–5 M Now if Mg(NO₃)₂ is present in a solution of [OH^–] = 10^–5 M, then, Product of ionic conc. = [Mg⁺²] [OH^– ]² = [0.002] [[10^–5]² = 2 × 10^–13 lesser than K_sp of Mg(OH)₂ i.e, 8.9 × 10^–12 ∴ Mg(OH)₂ will not precipitate.

Will a precipitate of Mg(OH)2 be formed in a 0.002 M solution of Mg(NO3)2, if the pH of solution is adjusted to 9 ? Ksp of Mg(OH)2 = 8.9 × 10–12.

Answer»

pH = 9

∴ [H⁺ ] = 10^–9 M

or [OH^–] = 10^–5 M

Now if Mg(NO₃)₂ is present in a solution of [OH^–] = 10^–5 M, then,

Product of ionic conc. = [Mg⁺²] [OH^– ]² = [0.002] [[10^–5]²

= 2 × 10^–13 lesser than K_sp of Mg(OH)₂ i.e, 8.9 × 10^–12

∴ Mg(OH)₂ will not precipitate.

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Will a precipitate of Mg(OH)2 be formed in a 0.002 M solution of Mg(NO3)2, if the pH of solution is adjusted to 9 ? Ksp of Mg(OH)2 = 8.9 × 10–12.

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