Deck 9: Solutions

Question 1

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

A)NaOH
B)PbS
C)K₂SO₄
D)LiNO₃
E)MgCl₂

Answer 1

PbS

Question 2

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.

Answer 2

the K+ ions are attracted to the partially negative oxygen atoms of the water molecule.

Question 3

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.

Answer 3

increases the solubility of a solid solute in the solution.

Question 4

How many equivalents are present in 0.40 moles of SO₄ ^2-?

A)0.10 Eq
B)0.20 Eq
C)0.40 Eq
D)0.80 Eq
E)1.2 Eq

Question 5

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 6

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 7

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 8

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 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

Hydrogen bonds are a major factor in the structure of

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

Question 11

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.

Question 12

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 13

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 14

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 15

Which of the following molecules can form hydrogen bonds?

A)CH₄
B)NaH
C)NH₃
D)BH₃
E)HI

Question 16

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 17

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.

Question 18

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 19

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 20

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 21

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 22

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 23

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 24

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 25

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 26

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

A)AgNO₃
B)CaCl₂
C)NH₄Cl
D)CaCO₃
E)Pb(C₂H₃O₂)₂

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 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 29

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 30

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 31

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 32

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

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

Question 33

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

A)AgBr
B)Cu(OH)₂
C)NH₄Cl
D)CaCO₃
E)PbS

Question 34

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 35

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 36

When solutions of KCl and Pb(NO₃)₂ are 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)→ 2KNO₃(aq)+ PbCl₂(s)
E)KCl(aq)+ Pb(NO₃)₂(aq)→ KNO₃(aq)+ PbCl(s)

Question 37

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 38

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 39

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

A)LiOH
B)K₂S
C)BaSO₄
D)NaNO₃
E)MgCl₂

Question 40

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 41

How many mL of 0.246 M Pb(NO₃)₂ are needed to react with 36.0 mL of 0.322 M KCl ?
2KCl(aq) + Pb(NO₃)₂(aq) → 2KNO₃(aq) + PbCl₂(s)

A)36.0 mL
B)18.0 mL
C)72.0 mL
D)47.1 mL
E)23.6 mL

Question 42

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 43

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 44

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 45

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 46

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 47

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 48

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 49

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 50

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 51

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 52

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)34.3 mL
D)10.7 mL
E)53.4 mL

Question 53

The process that occurs in this system is

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

Question 54

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 55

How many grams of PbCl₂ are formed when 25.0 mL of 0.654 M KCl react with Pb(NO₃)₂ ?
2KCl(aq) + Pb(NO₃) 2(aq) → 2KNO₃(aq) + PbCl₂(s)

A)22.7 g
B)1.64 g
C)2.27 g
D)4.54 g
E)9.08 g

Question 56

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 57

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 58

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 59

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 60

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 61

What is the osmolarity of a solution made by dissolving 25.0 g of the strong electrolyte KCl in 1.0 L of solution?

A)0.168 Osm
B)0.335 Osm
C)0.250 Osm
D)0.670 Osm
E)1.34 Osm

Question 62

NaCl can be classified as a ________.

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

Question 63

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

Question 64

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

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

Question 65

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 66

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

Question 67

Methanol, CH₃OH, can be classified as a ________.

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

Question 68

1.0 mole of NaCl is added to 1.0 kg 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 69

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 70

A red blood cell will undergo hemolysis in

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

Question 71

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 72

A red blood cell will undergo crenation in

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

Question 73

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

Question 74

0.50 mole of NaCl is added to 1.0 kg of water. The freezing point of the solution will be ________.

A)0.00 °C
B)0.93 °C
C)1.86 °C
D)-0.93 °C
E)-1.86 °C

Question 75

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 76

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 77

0.50 mole of KCl is added to 2.0 kg of water. The boiling point of the solution will be ________ the boiling point of pure water.

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

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

What is the osmolarity of a solution made by dissolving 0.50 mole of the strong electrolyte CaCl₂ in 1.0 L of solution?

A)0.50 Osm
B)1.0 Osm
C)1.5 Osm
D)2.0 Osm
E)0.0 Osm

Question 80

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

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