Q: A student dissolves $$0.67 g of$$ $$CaSO_4 in$$ $$1 L of $$water. The molar mass of $$CaSO_4 is$$ $$136.2 g/$$mol. What is the molar solubility ($$s) of$$ $$CaSO_4$$?

$$s = \frac{0.67}{136.2} = 4.9 \times 10$$^{-3}$$ mol/L

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

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

Q: Calculate the $$K_{sp}$$ for $$CaSO_4 if $$its molar solubility is $$4.9 \times 10$$^{-3}$$ mol/L.

$$K_{sp} = (4.9 \times 10$$^{-3}$$)^2 = 2.4$$ \times $$10^{-5}$

Q: A solution contains $$[Ag^+] = 0.010 M $$and $$[Cl^-] = 0.010 M. If$$ $$K_{sp}$$ for $$AgCl is$$ $$1.6 \times 10$$^{-10}$$, will a precipitate form?

Yes, because $$Q = 1.0 \times 10$$^{-4}$$ \u003e K_{sp}$$

Q: For $$CaF_2(s$$) \rightleftharpoons $$Ca^{2+}(aq) + 2F^-(aq$$)$$, if K$$_{sp} = 3.9 \times $$10^{-11}$$, what is the molar solubility ($$s) of$$ $$CaF_2$$?

$$s = \sqrt[3]{\frac{K_{sp}}{4}} = 2.1 \times 10$$^{-4}$$ mol/L

Q: A solution is prepared by mixing $$AgNO_3$$ and $$NaCl so $$that $$[Ag^+] = 1.0 \times 10$$^{-5}$$ M and $$[Cl^-] = 2.0 \times $$10^{-5} M. If$$ $$K_{sp}$$ for $$AgCl is$$ $$1.6 \times 10$$^{-10}$$, what is Q$ and will a precipitate form?

$$Q = 2.0 \times 10$$^{-10}$$; Yes, a precipitate will form.

Question 1

Which of the following best describes the solubility product constant ($$K_{sp}) $$for a slightly soluble salt?

Accepted Answer

It is the equilibrium constant for the dissolution of a slightly soluble salt into its ions.

Question 2

Given the dissolution of $$AgCl(s) \rightleftharpoons Ag^+(aq) + Cl^-(aq)$$, which is the correct $$K_{sp}$$ expression?

Accepted Answer

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

Question 3

A student dissolves $$0.67 g of$$ $$CaSO_4 in$$ $$1 L of $$water. The molar mass of $$CaSO_4 is$$ $$136.2 g/$$mol. What is the molar solubility ($$s) of$$ $$CaSO_4$$?

Accepted Answer

$$s = \frac{0.67}{136.2} = 4.9 	imes 10$$^{-3}$$ mol/L

Question 4

For the dissolution $$Ag_2CrO_4(s) \rightleftharpoons 2Ag^+(aq) + $$CrO_4$$^{2-}(aq)$$, what is the correct $$K_{sp}$$ expression?

Accepted Answer

$$K_{sp} = [Ag^+]^2[$$CrO_4$$^{2-}]$$

Question 5

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

Accepted Answer

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

Question 6

Calculate the $$K_{sp}$$ for $$CaSO_4 if $$its molar solubility is $$4.9 	imes 10$$^{-3}$$ mol/L.

Accepted Answer

$$K_{sp} = (4.9 	imes 10$$^{-3}$$)^2 = 2.4$$ 	imes $$10^{-5}$

Question 7

A solution contains $$[Ag^+] = 0.010 M $$and $$[Cl^-] = 0.010 M. If$$ $$K_{sp}$$ for $$AgCl is$$ $$1.6 	imes 10$$^{-10}$$, will a precipitate form?

Accepted Answer

Yes, because $$Q = 1.0 	imes 10$$^{-4}$$ \u003e K_{sp}$$

Question 8

Which of the following statements is TRUE regarding the relationship between $$Q$$ and $$K_{sp}$$ for precipitation?

Accepted Answer

A precipitate forms when $$Q \u003e K_{sp}.$$

Question 9

For $$CaF_2(s$$) ightleftharpoons $$Ca^{2+}(aq) + 2F^-(aq$$)$$, if K$$_{sp} = 3.9 	imes $$10^{-11}$$, what is the molar solubility ($$s) of$$ $$CaF_2$$?

Accepted Answer

$$s = \sqrt[3]{\frac{K_{sp}}{4}} = 2.1 	imes 10$$^{-4}$$ mol/L

Question 10

Which of the following is the correct $$K_{sp}$$ expression for $$Ca_3$$($$PO_4)_2(s$$) \rightleftharpoons $$3Ca^{2+}(aq) + 2PO$$_$$4^{3-}(aq$$)$$?

Accepted Answer

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

Question 11

A solution is prepared by mixing $$AgNO_3$$ and $$NaCl so $$that $$[Ag^+] = 1.0 	imes 10$$^{-5}$$ M and $$[Cl^-] = 2.0 	imes $$10^{-5} M. If$$ $$K_{sp}$$ for $$AgCl is$$ $$1.6 	imes 10$$^{-10}$$, what is Q$ and will a precipitate form?

Accepted Answer

$$Q = 2.0 	imes 10$$^{-10}$$; Yes, a precipitate will form.

Question 12

Which of the following best defines molar solubility?

Accepted Answer

The number of moles of solute dissolved in 1 L of a saturated solution.

Question 13

If the $$K_{sp}$$ for $$Ag_2CrO_4 is$$ $$9.3 	imes 10$$^{-12}$$ and its molar solubility is 1.3$$ 	imes $$10^{-4}$$ mol/L, what is the equilibrium concentration of $$Ag^+$$ ions?

Accepted Answer

$$[Ag^+] = 2 	imes 1.3 	imes 10$$^{-4}$$ = 2.6 	imes 10$$^{-4}$$ mol/L

Question 14

A solution is unsaturated with respect to $$AgCl if$$:

Accepted Answer

$$Q \u003c K_{sp}$$

Question 15

Which of the following would increase the likelihood of precipitation in a solution containing $$Ca^{2+}$$ and $$F^-$$ ions?

Accepted Answer

Increasing the concentration of either $$Ca^{2+} or$$ $$F^-$$ ions so that $$Q \u003e K_{sp}.$$

Question 16

If the $$K_{sp}$$ for $$CaF_2 is$$ $$3.9 	imes 10$$^{-11}$$, what is the equilibrium concentration of F$$^-$$ ions in a saturated solution?

Accepted Answer

$$[F^-] = 2s = 2 	imes 2.1 	imes 10$$^{-4}$$ = 4.2 	imes 10$$^{-4}$$ mol/L

Question 17

Which of the following is NOT a correct use of the solubility product constant ($$K_{sp}$$)?

Accepted Answer

Comparing the solubility of salts with different stoichiometry directly using $$K_{sp}$$ values.

Question 18

A patient receives an intravenous solution containing $$Ca^{2+}$$ and $$SO_4$$^{2-}$$ ions. If the product $$[$$Ca^{2+}$$][$$SO_4$$^{2-}]$$ exceeds the K$$_{sp}$$ for $$CaSO_4$$, what medical concern might arise?

Accepted Answer

Precipitation of $$CaSO_4 in $$the bloodstream, potentially causing blockages.

Solubility Equilibria and the Solubility Product Constant (Ksp)

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