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30 Jun 2020

Zinc hydroxide with Ksp = 3.0 x 10-17 starts to precipitate from a 8.57 x 10-3 M solution of zinc nitrate. What is the pH of the solution?

 

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AP Chemistry
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Solve problems involving solubility equilibria
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Related questions

1. A solution is prepared so that the concentrations of manganese(II) nitrate, zinc(II) nitrate, mercury(II) nitrate, and copper(II) nitrate are all 0.100 M. If the solution is slowly titrated with 0.100 M sodium sulfide, which metal sulfide will precipitate first?

zinc sulfide, Ksp = 1.8???10?25

copper(II) sulfide, Ksp = 5.4???10?37

manganese(II) sulfide, Ksp = 2.4???10?14

mercury(II) sulfide, Ksp = 1.8???10?53

2. Calculate molar solubilities, concentrations of constituent ions, and solubilities in grams per liter for the following compounds at 25°C:

[Sn2+] =

[S2?] =

solubility = g SnS/Liter

[Cd2+] =

[PO43?] =

solubility = g Cd3(PO4)2/Liter

tin(II) sulfide, SnS, Ksp = 9.00???10?27

cadmium(II) phosphate, Cd3(PO4)2, Ksp = 2.50???10?33

A solution contains 1.47×10-2 M zinc nitrate and 8.59×10-3 M silver acetate.
Solid ammonium cyanide is added slowly to this mixture.

What is the concentration of silver ion when zinc ion begins to precipitate?
[Ag+] = M

You are investigating the effect of strong base on the solubility of zinc hydroxide, Zn(OH)2 (s).

(Ksp= 3 x 10- 15 for Zn(OH)2 (s))

You prepare 1.0 L solution of 0.10M NaOH and add excess zinc hydroxide, Zn(OH)2 (s).

Instead of suppresing the solubility, you observe extra solubility.

Your research advisor tells you that zinc ions react with four hydroxide ions in a solution to form the complex ion Zn(OH)42- (aq).

(Kf = 2 x 10 15 for Zn(OH)42- (aq))

Calculate the pH of your solution.

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