(A) What minimum NH 4 must be present to prevent precipitation of Mn(OH) 2 (s) from a solution that is 0 0050 M MnCl 2 and 0 025 M NH 3 For Mn(OH) 2 , K sp 1 9 x 10 13 (B) What is the molar solubility of Mg(OH) 2 (s) in a solution that is 0 250 M NH 3 and 0 100 M NH 4 Cl Use equation (18 4) Eq 18 4 2 Mg(OH)2(s) 2 H3O (aq) Mg (aq) 4HO(1) (18 4)

Question: (A) What minimum [NH 4 + ] must be present to prevent precipitation of Mn(OH) 2 (s) from a solution that is 0.0050 M MnCl

(A) What minimum [NH₄⁺] must be present to prevent precipitation of Mn(OH)₂(s) from a solution that is 0.0050 M MnCl₂ and 0.025 M NH₃? For Mn(OH)₂, K_sp = 1.9 x 10^-13.

(B) What is the molar solubility of Mg(OH)₂(s) in a solution that is 0.250 M NH₃ and 0.100 M NH₄Cl? Use equation (18.4).

Eq. 18.4

2+ Mg(OH)2(s) + 2 H3O+ (aq) = Mg+ (aq) + 4HO(1) (18.4)

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