Deck 8: Solutions

Question 1

Oil does not dissolve in water because

A) oil is polar.
B) oil is nonpolar.
C) water is nonpolar.
D) water is saturated.
E) oil is hydrated.

Answer 1

oil is nonpolar.

Question 2

When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is

A) dilute.
B) polar.
C) nonpolar.
D) saturated.
E) unsaturated.

Answer 2

saturated.

Question 3

Which one of the following compounds will NOT be soluble in water?

A) LiOH
B) K₂S
C) BaSO₄
D) NaNO₃
E) MgCl₂

Answer 3

BaSO₄

Question 4

Hydrogen bonds are a major factor in the structure of

A) DNA.
B) hydrogen chloride.
C) dry ice.
D) air.
E) table salt.

Question 5

In a solution, the solvent

A) is a liquid.
B) can be a liquid or gas.
C) can be a solid, liquid, or gas.
D) is never a solid.
E) is the substance present in the smallest concentration.

Question 6

A solution is prepared by dissolving 2 g of KCl in 100 g of H₂O. In this solution, H₂O is the

A) solute.
B) solvent.
C) solution.
D) solid.
E) ionic compound.

Question 7

A hydrogen bond is

A) an attraction between a hydrogen atom attached to N, O, or F and an N, O, or F atom on another molecule.
B) a covalent bond between H and O.
C) an ionic bond between H and another atom.
D) a bond that is stronger than a covalent bond.
E) the polar O-H bond in water.

Question 8

The solubility of KI is 50 g in 100 g of H₂O at 20 °C. If 110 grams of KI are added to 200 grams of H₂O,

A) all of the KI will dissolve.
B) the solution will freeze.
C) the solution will start boiling.
D) a saturated solution will form.
E) the solution will be unsaturated.

Question 9

In water, a substance that ionizes completely in solution is called a

A) weak electrolyte.
B) nonelectrolyte.
C) semiconductor.
D) nonconductor.
E) strong electrolyte.

Question 10

In water, a substance that partially ionizes in solution is called a

A) weak electrolyte.
B) nonelectrolyte.
C) semiconductor.
D) nonconductor.
E) strong electrolyte.

Question 11

Water is a polar solvent and hexane (C₆H₁₄) is a nonpolar solvent. Which of the following correctly describes the solubility of the solute?

A) mineral oil, soluble in water
B) CaCl₂, soluble in hexane
C) NaHCO₃, soluble in water
D) CCl₄ , soluble in water
E) octane, soluble in water

Question 12

An equivalent is

A) the amount of ion that has a 1+ charge.
B) the amount of ion that has a 1- charge.
C) the amount of ion that carries 1 mole of electrical charge.
D) 1 mole of any ion.
E) 1 mole of an ionic compound.

Question 13

The O-H bond in water is polar because

A) it is an ionic bond.
B) oxygen is much more electronegative than hydrogen.
C) oxygen occupies more space than hydrogen.
D) hydrogen is much more electronegative than oxygen.
E) it is a hydrogen bond.

Question 14

An increase in the temperature of a solution usually

A) increases the boiling point.
B) increases the solubility of a gas in the solution.
C) increases the solubility of a solid solute in the solution.
D) decreases the solubility of a solid solute in the solution.
E) decreases the solubility of a liquid solute in the solution.

Question 15

How many equivalents are present in 5.0 moles of Al³⁺?

A) 15 Eq
B) 1.3 Eq
C) 5.0 Eq
D) 0.67 Eq
E) 3.0 Eq

Question 16

Which of the following molecules can form hydrogen bonds?

A) CH₄
B) NaH
C) NH₃
D) BH₃
E) HI

Question 17

When KCl dissolves in water

A) the Cl- ions are attracted to dissolved K+ ions.
B) the Cl- ions are attracted to the partially negative oxygen atoms of the water molecule.
C) the K+ ions are attracted to Cl- ions on the KCl crystal.
D) the K+ ions are attracted to the partially negative oxygen atoms of the water molecule.
E) the K+ ions are attracted to the partially positive hydrogen atoms of the water molecule.

Question 18

Which one of the following compounds will NOT be soluble in water?

A) NaOH
B) PbS
C) K2SO₄
D) LiNO₃
E) MgCl₂

Question 19

An intravenous replacement solution contains 4.0 mEq/L of Ca²⁺ ions. How many grams of Ca²⁺ are in 3.0 L of the solution?

A) 0.24 g
B) 0.80 g
C) 0.40 g
D) 240 g
E) 4.0 g

Question 20

How many equivalents are present in 5.0 g of Al³⁺?

A) 15 Eq
B) 0.56 Eq
C) 0.19 Eq
D) 0.37 Eq
E) 3 Eq

Question 21

What is the molarity of a solution that contains 3.25 moles of NaNO₃ in 250. mL of solution?

A) 3.25 M
B) 6.50 M
C) 0.0130 M
D) 13.0 M
E) 2.60 M

Question 22

According to Henry's law, the solubility of a gas in a liquid

A) decreases as the gas pressure above the liquid increases.
B) increases as the gas pressure above the liquid increases.
C) remains the same as the temperature increases.
D) depends on the liquid polarity.
E) depends on the liquid density.

Question 23

What volume (mL) of a 15% (m/v) NaOH solution contains 120 g NaOH?

A) 18 mL
B) 0.13 mL
C) 13 mL
D) 120 mL
E) 8.0 × 10² mL

Question 24

The molarity (M) of a solution refers to

A) moles of solute/L of solution.
B) moles of solute/L of solvent.
C) moles of solute/100 mL of solution.
D) grams of solute/100 mL of solution.
E) grams of solute/L of solution.

Question 25

Which one of the following compounds will be soluble in water?

A) AgBr
B) Ca(OH)₂
C) (NH)₄Cl
D) CaCO₃
E) PbS

Question 26

What is the molarity of a solution containing 5.0 moles of KCl in 2.0 L of solution?

A) 2.5 M
B) 1.0 M
C) 5.0 M
D) 10. M
E) 2.0 M

Question 27

A patient needs to receive 85 grams of glucose every 12 hours. What volume of a 5.0%(m/v) glucose solution needs to be administered to the patient each 12 hours?

A) 1700 mL
B) 60 mL
C) 6000 mL
D) 17 mL
E) 204 mL

Question 28

When 200. mL of water are added to 100. mL of 12% KCl solution the final concentration of KCl is (Assume the volumes add.)

A) 12%.
B) 4.0%.
C) 36%.
D) 6.0%.
E) 8.0%.

Question 29

What is the concentration, in mass percent, of a solution prepared from 50.0 g NaCl and 150.0 g of water?

A) 0.250%
B) 33.3%
C) 40.0%
D) 25.0%
E) 3.00%

Question 30

What is the concentration, in m/v percent, of a solution prepared from 50. g NaCl and 2.5 L of water?

A) 5.0%
B) 2.0%
C) 0.020%
D) 0.050%
E) 20.%

Question 31

How many grams of glucose are needed to prepare 400. mL of a 2.0%(m/v) glucose solution?

A) 800. g
B) 0.0050 g
C) 8.0 g
D) 2.0 g
E) 200. g

Question 32

The mass percent concentration refers to

A) grams of solute in 1 kg of solvent.
B) grams of solute in 1 kg of solution.
C) grams of solute in 100 g of solvent.
D) grams of solute in 100 g of solution.
E) grams of solvent in 100 g of solution.

Question 33

Which one of the following compounds will be soluble in water?

A) AgCl
B) Cu(OH)₂
C) LiCl
D) CaSO₄
E) PbCO₃

Question 34

The mass/volume percent concentration refers to

A) grams of solute in 1 L of solvent.
B) grams of solute in 1 L of solution.
C) grams of solute in 100 mL of solvent.
D) grams of solute in 100 mL of solution.
E) grams of solvent in 100 mL of solution.

Question 35

Rubbing alcohol is 70.% isopropyl alcohol by volume. How many mL of isopropyl alcohol are in a 1 pint (473 mL) container?

A) 70. mL
B) 0.15 mL
C) 680 mL
D) 470 mL
E) 330 mL

Question 36

When solutions of NaCl and AgNO₃ are mixed,

A) a precipitate of AgCl forms.
B) a precipitate of NaNO₃ forms.
C) no precipitate forms.
D) precipitate of NaNO₃ and AgCl form.
E) a precipitate of AgCl₂ forms.

Question 37

How many milliliters of a 25% (m/v) NaOH solution would contain 75 g of NaOH?

A) 25 mL
B) 75 mL
C) 33 mL
D) 19 mL
E) 3.0 × 10² mL

Question 38

What is the molarity of a solution that contains 17 g of NH₃ in 0.50 L of solution?

A) 34 M
B) 2.0 M
C) 0.50 M
D) 0.029 M
E) 1.0 M

Question 39

What is the molarity of a solution which contains 58.5 g of sodium chloride dissolved in 0.500 L of solution?

A) 0.500 M
B) 1.00 M
C) 1.50 M
D) 2.00 M
E) 4.00 M

Question 40

When solutions of KCl and Pb(NO₃)₂are mixed, a precipitate forms. Which of the following is the balanced equation for the double replacement reaction that occurs?

A) KCl(aq) + Pb(NO₃)₂(aq) → KNO₃(aq) + PbCl₂(s)
B) KNO₃(aq) + PbCl₂(s) → KCl(aq) + Pb(NO₃)₂(aq)
C) K+(aq) + NO₃-(aq) → KNO₃(aq)
D) 2KCl(aq) + Pb(NO₃)₂(aq) → 2 KNO₃(aq) + PbCl₂(s)
E) KCl(aq) + Pb(NO₃)₂(aq) → KNO₃(aq) + PbCl(s)

Question 41

A homogeneous mixture that does not settle out upon standing is

A) an element.
B) a colloid.
C) a suspension.
D) homogeneous.
E) hydrated.

Question 42

For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane.
A solution with the same osmotic pressure as the blood is

A) isotonic to the blood.
B) hypotonic to the blood.
C) hypertonic to the blood.
D) nontonic to the blood.
E) molar to the blood.

Question 43

What volume of 2.5% (m/v) KOH can be prepared from 125 mL of a 5.0% KOH solution?

A) 0.0040 mL
B) 63 mL
C) 0.10 mL
D) 125 mL
E) 250 mL

Question 44

During the process of diluting a solution to a lower concentration,

A) the amount of solute does not change.
B) the amount of solvent does not change.
C) there is more solute in the concentrated solution.
D) the volume of the solution does not change.
E) water is removed from the concentrated solution.

Question 45

For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane.
Which of the following occurs in this system?

A) Water flows equally in both directions.
B) There is a net flow of water from the 4% starch solution into the 10% starch solution.
C) There is a net flow of water from the 10% starch solution into the 4% starch solution.
D) Water does not cross the membrane at all.
E) Starch moves out of the 10% starch solution into the 4% starch solution.

Question 46

What volume of a 1.5 M KOH solution is needed to provide 3.0 moles of KOH?

A) 3.0 L
B) 0.50 L
C) 2.0 L
D) 4.5 L
E) 0.22 L

Question 47

How many moles of CaCl₂ are in 250 mL of a 3.0 M of CaCl₂ solution?

A) 750 moles
B) 1.3 moles
C) 83 moles
D) 0.75 mole
E) 3.0 moles

Question 48

For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane.
A red blood cell will undergo crenation in

A) water.
B) 0.5% NaCl.
C) 3% glucose.
D) 5% glucose.
E) 7% NaCl.

Question 49

In the process known as osmosis, __________ moves through a semipermeable membrane into an area of __________ concentration.

A) solute; lower solute
B) solute; higher solute
C) solvent; lower solute
D) solvent; lower solvent
E) solvent; higher solvent

Question 50

For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane.
Which starch solution will decrease in volume as osmosis occurs?

A) 4%
B) 10%
C) Neither exerts osmotic pressure.
D) They exert equal osmotic pressures.
E) They exert opposite osmotic pressures.

Question 51

Use the reaction: 2AgNO₃(aq) + H₂SO₄(aq) → Ag₂SO₄(s) + 2H₂O(l) What volume of 0.123 M AgNO₃(aq) is needed to form 0.657 g of Ag₂SO₄(s)?

A) 34.2 L
B) 17.1 mL
C) 34.2 mL
D) 10.7 mL
E) 53.4 mL

Question 52

For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane.
The process that occurs in this system is

A) filtration.
B) hydration.
C) neutralization.
D) dialysis.
E) osmosis.

Question 53

For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane.
Which solution is isotonic to a red blood cell?

A) water
B) 0.5% NaCl
C) 2% glucose
D) 0.9% NaCl
E) 10% glucose

Question 54

For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane.
A solution that has an osmotic pressure less than that of red blood cells is called

A) saturated.
B) hypertonic.
C) isotonic.
D) hypotonic.
E) unsaturated.

Question 55

What volume of 0.10 M NaOH can be prepared from 250. mL of 0.30 M NaOH?

A) 0.075 L
B) 0.25 L
C) 0.75 L
D) 0.083 L
E) 750 L

Question 56

For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane.
A red blood cell will undergo hemolysis in

A) water.
B) 0.9% NaCl.
C) 5% glucose.
D) 5% NaCl.
E) 10% glucose.

Question 57

The process by which a semipermeable membrane allows water molecules, small molecules, and ions to pass through while retaining large particles is called

A) osmotic pressure.
B) dialysis.
C) solvation.
D) dilution.
E) hydration.

Question 58

What is the new mass/volume (m/v)% of a KOH solution that is prepared by diluting 110 mL of a 6% (m/v) KOH solution to 330 mL?

A) 2%
B) 1%
C) 6%
D) 12%
E) 18%

Question 59

What is the molarity of a KCl solution made by diluting 75.0 mL of a 0.200 M solution to a final volume of 100. mL?

A) 0.267 M
B) 0.150 M
C) 0.200 M
D) 6.67 M
E) 0.100 M

Question 60

What volume of a 2.00 M KCl solution is required to prepare 500. mL of a 0.100 M KCl solution?

A) 0.0400 mL
B) 25.0 mL
C) 2.00 mL
D) 1.00 × 10⁴ mL
E) 5.00 × 10² mL

Question 61

Identify the term defined in each description.
the major attraction between water molecules

A)hypotonic
B)unsaturated
C)hydrogen bonding
D)saturated
E)hypertonic
F)hydration

Question 62

NaCl can be classified as a __________.

A) gas
B) liquid
C) weak electrolyte
D) strong electrolyte
E) nonelectrolyte

Question 63

Using a kidney machine to remove waste products from the blood is known as __________.

A) osmosis
B) osmolysis
C) autolysis
D) hemolysis
E) hemodialysis

Question 64

In the following equation, __________ will form a precipitate.
BaCl₂ + H₂SO₄ → BaSO₄ + 2HCl

Question 65

A mixture in which one component settles is called a(n) __________.

A) solution
B) colloid
C) suspension
D) electrolyte
E) nonelectrolyte

Question 66

A solution of sodium carbonate, Na₂CO₃, that has a molarity of 0.0100 M contains __________ equivalents of carbonate per liter of the solution.

Question 67

Is barium sulfate, BaSO₄, soluble or insoluble in water?

Question 68

Methanol, CH₃OH, can be classified as a __________.

A) gas
B) solid
C) weak electrolyte
D) strong electrolyte
E) nonelectrolyte

Question 69

Substances whose particles in solution scatter light and pass through filters but cannot pass through semipermeable membranes are called __________.

Question 70

1.0 mole of NaCl is added to 1.0 L of water. The freezing point of the solution will be __________ the freezing point of pure water.

A) higher than
B) lower than
C) the same as

Question 71

A substance that produces only a small number of ions in solution is known as a __________ electrolyte.

Question 72

Acetic acid can be classified as a(n) __________.

A) gas
B) solid
C) weak electrolyte
D) strong electrolyte
E) ionic compound

Question 73

A solution of sodium carbonate, Na₂CO₃, that has a molarity of 0.0100 M contains __________ equivalents of sodium ions per liter of the solution.

Question 74

An aqueous mixture containing starch (a colloid), NaCl, glucose, and albumin (a colloid) is placed in a dialyzing bag and immersed in distilled water. Which of the following correctly describes the location of the indicated substance after dialysis?

A) albumin, inside
B) starch outside
C) albumin inside and outside
D) water inside only
E) starch inside and outside

Question 75

The molarity of a solution of 5.0 g of KCl in 100. mL of solution is __________.

A) 0.038 M
B) 0.067 M
C) 0.67 M
D) 0.13 M
E) 1.3 M

Question 76

A substance that carries an electric current when dissolved in water is called a(n) __________.

Question 77

Identify the term defined in each description.
a solution that contains the highest amount of solute that dissolves at a given temperature

A)hypotonic
B)unsaturated
C)hydrogen bonding
D)saturated
E)hypertonic
F)hydration

Question 78

If 100. mL of water is added to 25 mL of 5.0 M NaCl, the final concentration is __________.

A) 25 M
B) 1.0 M
C) 5.0 M
D) 2.0 M
E) 1.3 M

Question 79

In the following equation, __________ will form a precipitate.
NaCl + AgNO₃ → AgCl + NaNO₃

Question 80

The number of moles of a compound dissolved in one liter of a solution is called the __________.