General chemistry, Chapter 5: Introductions to Aqueous Solutions and Aqueous Reactions

What is a solution?

A) A heterogeneous mixture
B) A homogeneous mixture
C) A pure substance
D) A compound

B) A homogeneous mixture

In a solution, the substance in greater amount is called the:
A) Solute
B) Solvent
C) Precipitate
D) Reactant

B) Solvent

Molarity is defined as:
A) Moles of solute per kilogram of solvent
B) Moles of solute per liter of solution
C) Grams of solute per liter of solution
D) Grams of solute per kilogram of solvent

B) Moles of solute per liter of solution

Which factor does NOT affect solubility?
A) Temperature
B) Pressure
C) Nature of solute and solvent
D) Volume of solvent

D) Volume of solvent

What is the process of reducing the concentration of a solution by adding more solvent called?
A) Dilution
B) Saturation
C) Precipitation
D) Evaporation

A) Dilution

Which unit is used to express molality?
A) Moles of solute per liter of solution
B) Moles of solute per kilogram of solvent
C) Grams of solute per liter of solution
D) Grams of solute per kilogram of solvent

A) Moles of solute per liter of solution

What is the maximum amount of solute that can dissolve in a solvent at a given temperature called?
A) Concentration
B) Solubility

C) Saturation
D) Molarity

B) Solubility

Percent composition by mass is calculated as:
A) (Mass of solute / Mass of solution) x 100
B) (Mass of solute / Volume of solution) x 100
C) (Volume of solute / Volume of solution) x 100
D) (Volume of solute / Mass of solution) x 100

A) (Mass of solute / Mass of solution) x 100

What is an aqueous reaction?
A) A reaction that occurs in air
B) A reaction that occurs in water
C) A reaction that occurs in a solid state
D) A reaction that occurs in a gaseous state

B) A reaction that occurs in water

Which type of reaction involves the formation of an insoluble product?
A) Acid-base reaction
B) Redox reaction
C) Precipitation reaction
D) Combustion reaction

C) Precipitation reaction

What is a spectator ion?
A) An ion that participates in the reaction
B) An ion that does not participate in the reaction
C) An ion that is formed during the reaction
D) An ion that is consumed during the reaction

B) An ion that does not participate in the reaction

Which of the following is a strong acid?
A) HCl
B) CH₃COOH
C) NH₃
D) H₂O

A) HCl

The pH scale measures:
A) The concentration of solute in a solution
B) The acidity or basicity of a solution
C) The solubility of a solute
D) The temperature of a solution

B) The acidity or basicity of a solution

In a redox reaction, the substance that loses electrons is:
A) Reduced
B) Oxidized
C) Neutralized
D) Precipitated

B) Oxidized

Which of the following is a common soluble compound?
A) AgCl
B) NaCl
C) PbSO₄
D) BaSO

B) NaCl

What is the term for the transfer of protons between reactants?
A) Redox reaction
B) Precipitation reaction
C) Acid-base reaction
D) Combustion reaction

A) Redox reaction

Which of the following is an example of a weak base?
A) NaOH
B) KOH
C) NH₃
D) H₂SO₄

C) NH₃

What is the first step in writing a net ionic equation?
A) Identify the spectator ions
B) Write the balanced molecular equation
C) Write the complete ionic equation
D) Balance the charges

B) Write the balanced molecular equation

19. Calculate the molarity of a solution containing 5.85 g of NaCl dissolved in 500 mL of water.
(Molar mass of NaCl = 58.5 g/mol)
a) 0.1 M
b) 0.2 M
c) 0.5 M
d) 1.0 M

b) 0.2 M

20. If 100 g of water is mixed with 10 g of NaCl, what is the mass percent of NaCl in the
solution?
a) 9%
b) 10%
c) 11%
d) 12%

b) 10%

21. How many moles of solute are present in 1 L of a 0.5 M Na₂SO₄ solution?
a) 0.25 mol
b) 0.5 mol
c) 1.0 mol
d) 2.0 mol

b) 0.5 mol

22. A solution has 2 moles of HCl dissolved in 1 kg of water. What is the molality of the
solution?
a) 1 m
b) 2 m
c) 0.5 m
d) 4 m

b) 2 m

23. How many grams of KCl are needed to prepare 500 mL of a 0.5 M solution? (Molar mass of
KCl = 74.5 g/mol)
a) 18.625 g
b) 37.25 g
c) 14.9 g
d) 29.8 g

a) 18.625 g

24. How many molecules of sucrose (C12H22O11, molar mass = 342.30 g/mol) are contained in
14.3 mL of 0.140 M sucrose solution?
A) 8.29 × 1022 molecules C12H22O11
B) 1.21 × 1021 molecules C12H22O11
C) 6.15 × 1022 molecules C12H22O11
D) 1.63 × 1023 molecules C12H22O11
E) 5.90 × 1024 molecules C12H22O11

B) 1.21 × 1021 molecules C12H22O11

25. According to the following reaction, how many moles of Fe(OH)2 can form from 175.0 mL
of 0.227 M LiOH solution? Assume that there is excess FeCl2.
FeCl2(aq) + 2 LiOH(aq) → Fe(OH)2(s) + 2 LiCl(aq)
A) 3.97 × 10-2 moles
B) 2.52 × 10-2 moles
C) 1.99 × 10-2 moles
D) 5.03 × 10-2 moles
E) 6.49 × 10-2 moles

C) 1.99 × 10-2 moles

26. Determine the number of grams H2 formed when 250.0 mL of 0.743 M HCl solution reacts
with 3.41 × 1023 atoms of Fe according to the following reaction.
2 HCl(aq) + Fe(s) → H2(g) + FeCl2(aq)
A) 0.374 g
B) 1.33 g
C) 1.14 g
D) 0.187 g
E) 1.51 g

D) 0.187 g

Choose the statement below that is TRUE.

A) A weak acid solution consists of mostly nonionized acid molecules.
B) The term "strong electrolyte" means that the substance is extremely reactive.
C) A strong acid solution consists of only partially ionized acid molecules.
D) The term "weak electrolyte" means that the substance is inert.
E) A molecular compound that does not ionize in solution is considered a strong electrolyte.

A) A weak acid solution consists of mostly nonionized acid molecules.

28. Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions
of lithium sulfide and copper (II) nitrate are mixed.
A) Li+(aq) + SO42-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + Li+(aq) + NO3-(aq)
B) Li+(aq) + S-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + LiNO3(aq)
C) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → Cu2+(aq) + S2-(aq) + 2 LiNO3(s)
D) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq)
E) No reaction occurs.

D) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq)

29. Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of
Na2CO3 and HCl are mixed.
A) 2 H+(aq) + CO32-(aq) → H2CO3(s)
B) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 NaCl(aq)
C) 2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g)
D) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 Na+(aq) + 2 Cl-(aq)
E) No reaction occurs.

C) 2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g)

30. The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of
0.218 M KOH solution. What is the concentration of the H3PO4 solution (in M)?
A) 1.03 M
B) 0.343 M
C) 0.114 M
D) 0.138 M
E) 0.0461 M

A) 1.03 M

31. What element is undergoing reduction (if any) in the following reaction?
Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s)
A) Zn
B) N
C) O
D) Ag
E) This is not an oxidation-reduction reaction.

D) Ag

32. Determine the oxidizing agent in the following reaction.
Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s)
A) Ag
B) Ni
C) Cl

D) O
E) This is not an oxidation-reduction reaction.

A) Ag