Q: A saturated solution of $$CaSO_4$$ has a solubility of 0.67 g/L. The molar mass of $$CaSO_4 is 136 g/$$mol. What is the value of $$K_{sp}$$ for $$CaSO_4$$?

$$K_{sp} = 2.4 \times 10$$^{-5}$$

Q: Given $$K_{sp}$$ for $$AgCl is$$ $$1.6 \times 10$$^{-10}$$, what is the molar solubility of $$AgCl$$ in pure water?

$$1.3 \times 10$$^{-5}$$\ \mathrm{mol/L}$$

Q: The $$K_{sp}$$ for $$CaF_2 is$$ $$3.9 \times 10$$^{-11}$$. What is the molar solubility of $$CaF_2$$ in pure water?

$$2.1 \times 10$$^{-4}$$\ \mathrm{mol/L}$$

Question 1

Which of the following is the correct solubility product ($$K_{sp}) $$expression for $$Ca_3$$($$PO_4)_2$?

Accepted Answer

$$K_{sp} = [Ca$$^{2+}$$]^3[PO_4$^{3-}]^2$$

Question 2

A saturated solution of $$CaSO_4$$ has a solubility of 0.67 g/L. The molar mass of $$CaSO_4 is 136 g/$$mol. What is the value of $$K_{sp}$$ for $$CaSO_4$$?

Accepted Answer

$$K_{sp} = 2.4 	imes 10$$^{-5}$$

Question 3

Given $$K_{sp}$$ for $$AgCl is$$ $$1.6 	imes 10$$^{-10}$$, what is the molar solubility of $$AgCl$$ in pure water?

Accepted Answer

$$1.3 	imes 10$$^{-5}$$\ \mathrm{mol/L}$$

Question 4

Which of the following best describes the effect of adding NaBr to a saturated solution of $$AgBr$$?

Accepted Answer

The solubility of $$AgBr$$ decreases due to the common ion effect.

Question 5

Which of the following compounds will be more soluble in acidic solution than in pure water?

Accepted Answer

$$CaCO_3$$

Question 6

A solution is prepared by mixing 0.050 L of $$2.0 	imes 10$$^{-2}$$\ \mathrm{M}$$ NaF with 0.010 L of $$1.0 	imes 10$$^{-2}$$\ \mathrm{M}$$ $$Ca(NO_3$)_2$$. $$K_{sp}$$ for $$CaF_2 is$$ $$3.9 	imes 10$$^{-11}$$. Will a precipitate of $$CaF_2$$ form?

Accepted Answer

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

Question 7

What is the $$K_{sp}$$ expression for $$Ag_2CO_3$$?

Accepted Answer

$$K_{sp} = [Ag^+]^2[CO_3$^{2-}]$$

Question 8

The $$K_{sp}$$ for $$CaF_2 is$$ $$3.9 	imes 10$$^{-11}$$. What is the molar solubility of $$CaF_2$$ in pure water?

Accepted Answer

$$2.1 	imes 10$$^{-4}$$\ \mathrm{mol/L}$$

Question 9

Which of the following statements about $$K_{sp} is $$correct?

Accepted Answer

$$K_{sp} is $$constant for a given salt at a given temperature.

Question 10

Which of the following will NOT affect the solubility of $$AgCl in $$water?

Accepted Answer

Adding $$NaNO_3$$

Question 11

If the initial concentrations of $$Ag^+$$ and $$Cl^- in a $$solution are such that $$Q = [Ag^+][Cl^-] \u003c K_{sp}$$ for $$AgCl$$, what will happen?

Accepted Answer

No precipitate will form and more $$AgCl$$ can dissolve.

Question 12

Which of the following best explains why $$Mg(OH)_2 is $$more soluble in acidic solution?

Accepted Answer

Acid reacts with $$OH^-$$, shifting the equilibrium to dissolve more $$Mg(OH)_2.$$

Question 13

A student adds $$0.010\ \mathrm{M}$$ NaF to a saturated solution of $$CaF_2. $$What happens to the solubility of $$CaF_2$$?

Accepted Answer

The solubility of $$CaF_2$$ decreases due to the common ion effect.

Question 14

Which of the following salts will have its solubility unaffected by a change in pH?

Accepted Answer

$$NaCl$$

Question 15

A solution contains $$[Ag^+] = 1.0 	imes 10$$^{-5}$$\ \mathrm{M}$$ and $$[Cl^-] = 2.0 	imes 10$$^{-5}$$\ \mathrm{M}$$. $$K_{sp}$$ for $$AgCl is$$ $$1.6 	imes 10$$^{-10}$$. Will a precipitate form?

Accepted Answer

Yes, because $$Q = 2.0 	imes 10$$^{-10}$$ \u003e K_{sp}$$

Question 16

Which of the following best describes the relationship between $$K_{sp}$$ and molar solubility for a salt $$MX_2$$?

Accepted Answer

$$K_{sp} = 4s^3$, where s$ is the molar solubility

Question 17

Which of the following is a correct real-life application of precipitation reactions?

Accepted Answer

Water softening by removing $$Ca^{2+}$$ and $$Mg^{2+}$$ ions as insoluble salts

Solubility and Solubility Equilibria (General Chemistry Study Notes)

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