Q: Calculate the molar solubility $$s of$$ $$\mathrm{AgCl} if$$ $$K_{sp} = 1.6 \times 10$$^{-10}$$.

$$s = \sqrt{1.6 \times 10$$^{-10}$$} = 1.3 \times 10$$^{-5}$$

Q: Calculate the concentration of $$\mathrm{Sr$$^{2+}$$} in $$equilibrium with $$[\mathrm{$$CrO_4$$^{2-}}] = 2.0 \times 10$$^{-3}$$ \ \mathrm{M} if$$ $$K_{sp,\mathrm{$$SrCrO_4$$}} = 3.7 \times 10$$^{-5}$$.

$$[\mathrm{Sr$$^{2+}$$}] = \frac{3.7 \times 10$$^{-5}$$}{2.0 \times 10$$^{-3}$$} = 1.85 \times 10$$^{-2}$$ \ \mathrm{M}$$

Q: What is the molar solubility of $$\mathrm{AgCl} in a$$ $$6.5 \times 10$$^{-3}$$ \ \mathrm{M}$$ $$\mathrm{$$AgNO_3$$}$$ solution if $$K_{sp} = 1.6 \times 10$$^{-10}$$?

$$s = \frac{1.6 \times 10$$^{-10}$$}{6.5 \times 10$$^{-3}$$} = 2.5 \times 10$$^{-8}$$

Q: If the solubility of $$\mathrm{CdS} is$$ $$4.1 \times 10$$^{-12}$$ \ \mathrm{g/L}$$ and its molar mass is $$144.4 \ \mathrm{g/mol}$$, what is its $$K_{sp}$$?

$$K_{sp} = s^2$ = 8.1 \times 10$$^{-28}$$

Question 1

Which of the following best describes a saturated solution?

Accepted Answer

A solution that contains the maximum amount of solute that will dissolve in a given solvent at a specific temperature.

Question 2

Given the solubility equilibrium $$\mathrm{AgCl(s) \rightleftharpoons Ag^+(aq) + Cl^-(aq)}$$, why do solids not appear in the equilibrium constant expression?

Accepted Answer

Solids have a constant concentration and do not affect the equilibrium.

Question 3

Calculate the molar solubility $$s of$$ $$\mathrm{AgCl} if$$ $$K_{sp} = 1.6 	imes 10$$^{-10}$$.

Accepted Answer

$$s = \sqrt{1.6 	imes 10$$^{-10}$$} = 1.3 	imes 10$$^{-5}$$

Question 4

A solution contains $$[\mathrm{Sr$$^{2+}$$}] = 1.0 	imes 10$$^{-3}$$ \ \mathrm{M}$$ and $$[\mathrm{$$CrO_4$$^{2-}}] = 3.0 	imes 10$$^{-5}$$ \ \mathrm{M}. If$$ $$K_{sp,\mathrm{$$SrCrO_4$$}} = 3.6 	imes 10$$^{-5}$$, will a precipitate form?

Accepted Answer

No, because $$Q \u003c K_{sp}.$$

Question 5

What is the effect of adding a common ion to a solution containing an ionic compound?

Accepted Answer

It decreases the solubility of the ionic compound.

Question 6

Calculate the concentration of $$\mathrm{Sr$$^{2+}$$} in $$equilibrium with $$[\mathrm{$$CrO_4$$^{2-}}] = 2.0 	imes 10$$^{-3}$$ \ \mathrm{M} if$$ $$K_{sp,\mathrm{$$SrCrO_4$$}} = 3.7 	imes 10$$^{-5}$$.

Accepted Answer

$$[\mathrm{Sr$$^{2+}$$}] = \frac{3.7 	imes 10$$^{-5}$$}{2.0 	imes 10$$^{-3}$$} = 1.85 	imes 10$$^{-2}$$ \ \mathrm{M}$$

Question 7

Which factor increases the solubility of an ionic compound in water?

Accepted Answer

Formation of a complex ion.

Question 8

What is the molar solubility of $$\mathrm{AgCl} in a$$ $$6.5 	imes 10$$^{-3}$$ \ \mathrm{M}$$ $$\mathrm{$$AgNO_3$$}$$ solution if $$K_{sp} = 1.6 	imes 10$$^{-10}$$?

Accepted Answer

$$s = \frac{1.6 	imes 10$$^{-10}$$}{6.5 	imes 10$$^{-3}$$} = 2.5 	imes 10$$^{-8}$$

Question 9

A 200 mL sample of $$0.20 \ \mathrm{M}$$ $$\mathrm{NaOH} is $$added to $$1.0 \ \mathrm{L} of$$ $$0.10 \ \mathrm{M}$$ $$\mathrm{$$CaCl_2$$}. $$Will a precipitate of $$\mathrm{Ca(OH)_2}$$ form if $$K_{sp} = 8.0 	imes 10$$^{-6}$$?

Accepted Answer

Yes, because $$Q \u003e K_{sp}.$$

Question 10

Which equation correctly represents the solubility product constant ($$K_{sp}) $$for $$\mathrm{Cu(OH)_2}$$?

Accepted Answer

$$K_{sp} = 4s^3$

Question 11

If the solubility of $$\mathrm{CdS} is$$ $$4.1 	imes 10$$^{-12}$$ \ \mathrm{g/L}$$ and its molar mass is $$144.4 \ \mathrm{g/mol}$$, what is its $$K_{sp}$$?

Accepted Answer

$$K_{sp} = s^2$ = 8.1 	imes 10$$^{-28}$$

Question 12

Which of the following statements about complex ion formation is correct?

Accepted Answer

Complex ion formation increases the solubility of ionic compounds.

Question 13

What is the effect of pH on the solubility of a basic salt?

Accepted Answer

A basic salt is more soluble in acidic solutions.

Question 14

Which of the following is the correct expression for the ion product $$Q$$ for $$\mathrm{AgCl}$$?

Accepted Answer

$$Q = [Ag^+][Cl^-]$$

Question 15

A solution is unsaturated if:

Accepted Answer

It contains less solute than the capacity it can dissolve.

Question 16

Which of the following best explains why heating increases solubility?

Accepted Answer

Heating increases the kinetic energy of molecules, allowing more solute to dissolve.

Question 17

What is the new equilibrium constant $$K'$$ for the reaction $$\mathrm{AgCl + 2NH_3 ightleftharpoons Ag(NH_3$)_2^+ + Cl^-} if$$ $$K_{sp} = 1.6 	imes 10$$^{-10}$$ and K_f = 1.5$$ 	imes $$10^7$$?

Accepted Answer

$$K' = K_{sp} 	imes K_f = 2.4 	imes 10$$^{-3}$$

Question 18

Which of the following is a real-life application of solubility equilibria?

Accepted Answer

Predicting the formation of kidney stones in the human body.

Solubility and Complex Ions: Principles, Calculations, and Applications

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