CHEM126 – CHAPTER 16 – REGULAR HOMEWORK / SOLUBILITY

 

CHAPTER 16 REGULAR HOMEWORK:

SOLUBILITY

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Question 1

 

At a certain temperature* (probably not 25 ºC), the solubility of silver sulfate, Ag2SO4, is 0.010 mol/L. Calculate its solubility product constant for this temperature. 4 SIG. FIG. (required because number is small)

*Solubility product constants are very temperature sensitive. They are generally reported at 25 ºC. Not necessarily using this temperature allows me some flexibility.

 

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Explanation

Question 2

At a certain temperature, the solubility of potassium iodate, KIO3, is 38.6 g/L. Calculate its solubility product constant for this temperature.

 

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Explanation

Question 3

At a certain temperature, the solubility of cadmium fluoride, CdF2, is 0.083 mol/L. Calculate its solubility product constant for this temperature.

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Explanation

Question 4

At a certain temperature, the solubility product constant* of copper (II) iodate, Cu(IO3)2, is 7.60×10-8 M3. Calculate the solubility of this compound for this temperature.

*Unless stated otherwise all solubility product constants are for water.

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Explanation

Question 5

Calculate the solubility of copper (II) iodate in 0.61 M copper (II) nitrate. Ksp* is 7.4×10-8 M3.

*You should know that the Ksp must refer to the copper iodate because all nitrate compounds are soluble and strong electrolytes!

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Explanation

Question 6

Warm UP Question. What is the initial (before any reaction takes place) lead nitrate concentration when 5.0 mL of 0.247 M lead nitrate is added to 15 mL of 0.0028 M sodium chloride?

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Explanation

Question 7

For the reaction: PbCl2(s) ↔ Pb2+(aq)+2Cl1-(aq), what is Q* when 2.4 mL of 0.098 M lead nitrate is added to 20 mL of 0.019 M sodium chloride?
Ksp of lead chloride is 1.6 x 10-5 M3.
Hint given in general feedback

*Recall: Q is compared to Ksp to determine whether a precipitate forms.

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Explanation

Remember each solution is diluted by the other solution.

Question 8

Does a precipitate form for the above conditions?

 

Select one:


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Explanation

Question 9

Pick the correct formula for sodium phosphate, calcium phosphate, and aluminum phosphate. (All must be correct to get credit.)

 

Select one or more:



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Explanation

Question 10

The Ksp of aluminum phosphate is 9.8×10-21 M2.
The Ksp of calcium phosphate is 1.3×10-32 M5.

Sodium phosphate is added to a solution that contains aluminum nitrate and calcium chloride. Their concentrations, which are necessary to do this problem, are given in the next question. Which begins to precipitate first?

 

Select one:

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Explanation

Question 11

Sodium phosphate is added to a solution that contains 0.0099 M aluminum nitrate and 0.021 M calcium chloride. The concentration of the first ion to precipitate (either Al3+ or Ca2+) decreases as its precipitate forms. What is the concentration of this ion when the second ion begins to precipitate?

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Explanation

Note that well over 99% of the first ion has precipitated before the second ion starts to precipitate.