Question 1

Which of the following best describes Avogadro’s number?

Accepted Answer

The number of particles (atoms, molecules, or ions) in one mole of a substance.

Question 2

A solution is prepared by dissolving 10.0 g of NaCl in enough water to make 500.0 mL of solution. What is the molarity of the solution? (Molar mass of NaCl = 58.44 g/mol)

Accepted Answer

$$0.171\ \mathrm{M}$$

Question 3

Which of the following is the correct net ionic equation for the reaction between aqueous solutions of sodium sulfate and barium chloride?

Accepted Answer

$$\mathrm{SO_4$^{2-}(aq) + Ba$$^{2+}$$(aq) \rightarrow $$BaSO_4$$(s)}$$

Question 4

Which of the following statements about strong acids and bases is correct?

Accepted Answer

Strong acids and bases completely dissociate in water.

Question 5

A student mixes 50.0 mL of 2.00 M HCl with 50.0 mL of 2.00 M NaOH. What is the limiting reactant?

Accepted Answer

Neither; both are present in stoichiometric amounts.

Question 6

Which of the following is the correct balanced chemical equation for the reaction: 'Aqueous sodium sulfate reacts with aqueous silver nitrate to produce solid silver sulfate and aqueous sodium nitrate'?

Accepted Answer

$$\mathrm{Na_2SO_4(aq) + 2AgNO_3(aq) \rightarrow Ag_2SO_4(s) + 2NaNO_3(aq)}$$

Question 7

How many molecules are present in 0.250 mol of glucose ($$\mathrm{C_6H_{12}O_6$}$$)? ($$N_A = 6.022 	imes 10$$^{23}$$\ \mathrm{mol}^{-1})$$

Accepted Answer

$$1.51 	imes 10$$^{24}$$

Question 8

Which of the following best describes the role of the solvent in a solution?

Accepted Answer

The solvent is the substance present in the greatest amount and dissolves the solute.

Question 9

A chemist wants to prepare 250.0 mL of a 0.100 M NaOH solution from a 1.00 M NaOH stock solution. What volume of the stock solution should be used?

Accepted Answer

$$25.0\ \mathrm{mL}$$

Question 10

Which of the following is the correct oxidation number for sulfur in $$\mathrm{H_2SO_4}$$?

Accepted Answer

$$+6$$

Question 11

A reaction has a theoretical yield of 12.0 g and an actual yield of 9.0 g. What is the percent yield?

Accepted Answer

$$75\%$$

Question 12

Which of the following reactions is a precipitation reaction?

Accepted Answer

$$\mathrm{$$AgNO_3$$(aq) + NaCl(aq) \rightarrow AgCl(s) + $$NaNO_3$$(aq)}$$

Question 13

Which species is oxidized in the following reaction? $$\mathrm{Zn(s) + $$CuSO_4$$(aq) \rightarrow $$ZnSO_4$$(aq) + Cu(s)}$$

Accepted Answer

$$\mathrm{Zn}$$

Question 14

How many grams of $$\mathrm{Ca(OH)_2}$$ are required to react completely with 25.0 mL of 10.0 M acetic acid ($$\mathrm{HC_2H_3O_2}$$)? (Molar masses: $$\mathrm{Ca(OH)_2} = 74.09\ \mathrm{g/mol}$$, $$\mathrm{HC_2H_3O_2} = 60.05\ \mathrm{g/mol})$$

Accepted Answer

$$9.26\ \mathrm{g}$$

Question 15

Which of the following is the correct complete ionic equation for the reaction between aqueous sodium chloride and aqueous silver nitrate?

Accepted Answer

$$\mathrm{Na^+(aq) + Cl^-(aq) + Ag^+(aq) + NO_3$^-(aq) \rightarrow Na^+(aq) + NO_3$^-(aq) + AgCl(s)}$$

Question 16

A solution is made by diluting 10.0 mL of 6.00 M HCl to a final volume of 100.0 mL. What is the final concentration?

Accepted Answer

$$0.600\ \mathrm{M}$$

Question 17

Which of the following best explains why a net ionic equation is useful?

Accepted Answer

It shows only the species that actually participate in the chemical change.

Question 18

Which of the following is the correct stoichiometric factor (mole ratio) between $$\mathrm{HC_2H_3O_2}$$ and $$\mathrm{Ca(OH)_2} in $$the reaction: $$2\ \mathrm{HC_2H_3O_2(aq) + Ca(OH)_2(s) \rightarrow Ca(C_2H_3O_2)_2(aq) + 2H_2O(l)}$$?

Accepted Answer

$$2\ \mathrm{mol}\ \mathrm{HC_2H_3O_2} : 1\ \mathrm{mol}\ \mathrm{Ca(OH)_2}$$

Question 19

A reaction mixture contains 5.00 g of $$\mathrm{$$AgNO_3$$}$$ and 5.00 g of $$\mathrm{NaCl}. $$Which reactant is the limiting reactant? (Molar masses: $$\mathrm{$$AgNO_3$$} = 169.87\ \mathrm{g/mol}$$, $$\mathrm{NaCl} = 58.44\ \mathrm{g/mol})$$

Accepted Answer

$$\mathrm{$$AgNO_3$$}$$

CHEM103 Exam 2 Study Guide: Moles, Solutions, and Chemical Reactions

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