Question 1

When KCl dissolves in water, what happens at the molecular level?

Accepted Answer

K+ and Cl- ions dissociate and become surrounded by water molecules.

Question 2

Which of the following compounds is most likely to be soluble in water?

Accepted Answer

(NH$$_4$$)$$_3PO$_4$$

Question 3

What is the concentration (in molarity) when 0.010 mol of NaCl is dissolved in enough water to make 100. mL of solution?

Accepted Answer

$$0.10\ \mathrm{M}$$

Question 4

When 0.10 mol of CaCl$$_2 is $$dissolved in enough water to make 1.00 L of solution, what is the concentration of Cl$$^-$$ ions?

Accepted Answer

$$0.20\ \mathrm{M}$$

Question 5

Which of the following is NOT a strong electrolyte?

Accepted Answer

CH$$_3OH(aq)$$

Question 6

Would you expect distilled water to conduct electricity?

Accepted Answer

Yes, but very weakly because water self-ionizes to a small extent.

Question 7

Which of the following best describes a precipitation reaction?

Accepted Answer

A reaction where a cation and anion combine to form an insoluble solid.

Question 8

When aqueous solutions of MgBr$$_2$$ and Na$$_2SO$_4$$ are mixed together, what happens?

Accepted Answer

Nothing precipitates.

Question 9

Which of the following compounds would you expect to be insoluble in water?

Accepted Answer

PbSO$$_4$$

Question 10

What is the net ionic equation for the reaction between AgNO$$_3(aq) $$and Na$$_2S(aq$$)?

Accepted Answer

$$2\mathrm{Ag}^+(aq) + \mathrm{S}^{2-}(aq) \rightarrow \mathrm{Ag}_2\mathrm{S}(s)$$

Question 11

If 100. mL of 0.100 M AgNO$$_3(aq) is $$mixed with 200. mL of 0.100 M Na$$_2S(aq$$), what is the limiting reactant for the formation of Ag$$_2S(s$$)?

Accepted Answer

AgNO$$_3$$

Question 12

Which of the following ions would increase the conductivity of water the most when dissolved at equal molar concentrations?

Accepted Answer

Ca$$^{2+}$$

Question 13

Which statement best explains why most Group I cation compounds are soluble in water?

Accepted Answer

Group I cations do not form strong lattice energies, making their salts more easily dissociated.

Question 14

A student mixes solutions of Pb(NO$$_3$$)$$_2(aq) $$and KI(aq). What is the identity of the yellow solid formed?

Accepted Answer

PbI$$_2$$

Question 15

Which of the following is a weak electrolyte?

Accepted Answer

CH$$_3$$COOH(aq)

Question 16

Which of the following best describes a nonelectrolyte?

Accepted Answer

A substance that dissolves in water but does not dissociate into ions.

Question 17

Which of the following compounds is most likely to form a precipitate when mixed with Na$$_2CO$_3(aq$$)?

Accepted Answer

CaCl$$_2(aq)$$

Question 18

What is the molarity of Ag$$^+$$ ions after mixing 100. mL of 0.100 M AgNO$$_3$$ with 200. mL of 0.100 M Na$$_2S$$, assuming complete precipitation of Ag$$_2S$$?

Accepted Answer

$$0.000\ \mathrm{M}$$

Question 19

Which of the following best explains why Ag$$_2S $$forms a precipitate when AgNO$$_3(aq) is $$mixed with Na$$_2S(aq$$)?

Accepted Answer

Ag$$^+$$ and S$$^{2-}$$ ions combine to form an insoluble solid due to low solubility product ($$K_{sp}).$$

Dissolving Ionic Compounds and Electrolytes: Solubility, Precipitation, and Net Ionic Reactions

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