Question

a Explain how (in procedures step format), the reaction of Ni(OH)2 with NH3 would enable you...

a Explain how (in procedures step format), the reaction of Ni(OH)2 with NH3 would enable you to separate a mixture of iron(III) and nickel(II) hydroxide.

I need help with question a but can you tell me if my answers are right for b and c Thank you

b Explain why you can dissolve Ni(OH)3 in aqueous ammonia.

The compound Ni(OH)2 is very much soluble in ammonia, since it will form a complex precipitate.

c. Could you use excess NaOH to separate a mixture of the precipitates of Fe(OH)3 and Ni(OH)2? Explain briefly why or why not.

You can not use excess NaOH to separate a mixture of the precipitates of Fe(OH)3 and Ni(OH)2 because both precipitates are not soluble in excess NaOH. They would not dissolve in the NaOH solution and both would stay precipitate.

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Homework Answers

Answer #1

a. [Fe(H2O)6]3+ + 3OH- = Fe(OH)3 + 6H2O

[Fe(H2O)6]3+ + 6NH3 = [Fe(NH3)6]3+ + 6H2O

Fe(OH)3 is insoluble in water and more stable than [Fe(H2O)6]3+ or [Fe(NH3)6]3+ so it is preferentially formed than the other two.

[Ni(H2O)6]2+ + 2OH- = Ni(OH)2 + 6H2O

[Ni(H2O)6]2+ + 6NH3 = [Ni(NH3)6]2+ + 6H2O

[Ni(NH3)6]2+ is a very stable complex and it is soluble in water and is preferentially formed than Ni(OH)2.

So when ammonia is added in a mixture of Fe(OH)3 and Ni(OH)2 , Ni(OH)2 will readily form [Ni(NH3)6]2+ but Fe(OH)3 will remain as a precipitate. The precipitate can be separated from the mixture.

b. [Ni(H2O)6]2+ + 2OH- = Ni(OH)2 + 6H2O

[Ni(H2O)6]2+ + 6NH3 = [Ni(NH3)6]2+ + 6H2O

The second equilibrium is more fast forward that the first equilibrium. This makes it possible to dissolve Ni(OH)3 in aqueous ammonia.

c. Your answer is right.

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