Deck 8: Solution Chemistry: How Sweet Is Your Tea

Question 1

Of the following, which can serve as the solute in a solution?

A)A liquid
B)A solid
C)A gas
D)All of the above

Answer 1

All of the above

Question 2

A homogeneous mixture consists of 12% ethanol, 28% methanol and 60% water. Which of these is the solvent for the mixture?

A)Ethanol
B)Methanol
C)Water
D)Ethanol and methanol

Answer 2

Water

Question 3

A homogeneous mixture consists of 34% ethanol and 66% isopropanol. Which of these is the solute of the mixture?

A)Isopropanol
B)Ethanol
C)Both ethanol and isopropanol
D)Neither ethanol nor isopropanol

Answer 3

Ethanol

Question 4

In a solution, the solute is:

A)the substance in the greatest amount
B)the substance that is dissolved
C)always water
D)always a gas

Question 5

In a solution, the solvent is:

A)always water
B)the substance in the greatest amount
C)the substance that is dissolved
D)always a gas

Question 6

Which of the following statements best describes the phrase "like dissolves like"?

A)The only true solutions are formed when water dissolves a polar solute.
B)A solvent and a solute with similar intermolecular forces will easily make a solution.
C)The only true solutions are formed when water dissolves a nonpolar solute.
D)A solvent will dissolve a solute that has a similar mass.

Question 7

Which of the following can be classified as a colloid?

A)Grape juice
B)Homogenized milk
C)Blood
D)Kool-Aid

Question 8

Which of the following is an example of a true solution?

A)Blood
B)Homogenized milk
C)Apple juice
D)Mayonnaise

Question 9

You have been given an unknown liquid that is soluble in water but not in benzene (a nonpolar solvent). Which type of intermolecular forces does this unknown have?

A)Polar
B)Nonpolar
C)Neither polar nor nonpolar
D)Both polar and nonpolar

Question 10

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

A)CH₃OH
B)CH₃CH₂OH
C)CH₃CH₂CH₂OH
D)CH₃CH₂CH₂CH₂OH

Question 11

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

A)CH₃NH₂
B)CH₃CH₂OH
C)CH₃CHO
D)CH₃OCH₃

Question 12

The exchange of oxygen and carbon dioxide in the lungs is an example of which law involving gases?

A)Boyle's law
B)Charles' law
C)Avogadro's law
D)Henry's law

Question 13

Which one of the following compounds will be most soluble in hexane, a nonpolar solvent?

A)CH₃CH₂ OH
B)CH₃CH₂CH₂OH
C)CH₃CH₂CH₂CH₂CH₃
D)CH₃OH

Question 14

A water solution of sucrose, table sugar, does not conduct electricity. Due to this property, sucrose is classified as a(n):

A)weak electrolyte
B)strong electrolyte
C)non-electrolyte
D)semi-electrolyte

Question 15

A water solution of acetic acid, vinegar, barely lights a light bulb. This property means that vinegar is a(n):

A)weak electrolyte
B)strong electrolyte
C)non-electrolyte
D)semi-electrolyte

Question 16

Which of the following is a typical chemical equation that represents a hydration reaction?

A)
B)C₆H₁₂O₆ (s)+ 6 O₂ (g)? 6 CO₂ (g)+ 6 H₂O (l)
C)2 KClO₃ (s)? 2 KCl (s)+ 3 O₂ (g)
D)HCl (aq)+ NaOH (aq)? NaCl (aq)+ H₂O (l)

Question 17

What is the correct balanced hydration equation for (NH₄)₂CO₃?

A)
B)
C)
D)

Question 18

Which one of these substances will exist in solution only as molecules?

A)CH₃OH
B)LiOH
C)NH₄OH
D)CH₃NH₂

Question 19

Which of the following is an example of a weak electrolyte?

A)MgCl₂
B)HC₂H₃O₂
C)HNO₃
D)Na₂CO₃

Question 20

Which of the following is an example of a nonelectrolyte?

A)MgCl₂
B)HC₂H₃O₂
C)C₁₂H₂₂O₁₁
D)Na₂SO₄

Question 21

How many equivalents of Li⁺ are present in a solution that contains 5.75 mol of Li⁺?

A)0)575 eq
B)5)75 eq
C)2)88 eq
D)11.5 eq

Question 22

How many equivalents of Mg⁺² are present in a solution that contains 2.75 mol of Mg⁺²?

A)1)38 eq
B)2)75 eq
C)5)50 eq
D)27.5 eq

Question 23

Which of the following equation is a correct balanced hydration equation for the hydration of Na₂SO₄?

A)
B)
C)
D)

Question 24

What is 75% of 375?

A)281
B)28,125
C)2)81
D)0)281

Question 25

45 is what percent of 150?

A)0)30
B)30
C)0)0030
D)3000

Question 26

Calculate the mass percent of a solution prepared by dissolving 17.2 g of NaCl in 149 g of water.

A)10.3%
B)11.5%
C)0)103%
D)0)115%

Question 27

What is the percent mass/volume (%m/v)of a solution that is made from putting 25.0 g of NaCl in water to make 275 mL of solution?

A)0)0909%m/v
B)9)09%m/v
C)8)33%m/v
D)10.9%m/v

Question 28

What is the %v/v concentration of a sample of wine that contains 15 mL of ethyl alcohol in 200 mL of wine?

A)0)075%v/v
B)7)0%v/v
C)7)5%v/v
D)0)070%v/v

Question 29

What is the %v/v concentration of a solution made by adding 25 mL of acetone to 75 mL of water?

A)0.25%v/v
B)25%v/v
C).33%v/v
D)33%v/v

Question 30

What is the glucose concentration in ppm of a solution made by mixing 23.2 mg glucose with 2.000 L?

A)8)62 ppm
B)11.6 ppm
C)1)16 ppm
D)0)862 ppm

Question 31

What is the lead concentration in ppb of a water sample that contains 28 ?g of lead in 44 L?

A)0)064 ppb
B)0)64 ppb
C)64 ppb
D)640 ppb

Question 32

Calculate the volume (in L)of a solution that contains 3.12 moles of NaCl if the concentration of this solution is 6.67 M NaCl?

A)2)14 L
B)20.8 L
C)46.8 L
D)0)468 L

Question 33

What is the molarity of a solution formed by dissolving 45 g NaOH in water to give a final volume of 250 mL?

A)0)0045 M
B)0)18 M
C)4)5 M
D)9)0 M

Question 34

What is the molarity of a solution that contains 36 mEq Ca²⁺ per liter?

A)0)018 M
B)0)036 M
C)18 M
D)36 M

Question 35

Calculate the volume (in mL)of a 2.75 M solution that must be used to make 1.25 L of a 0.150 M solution.

A)0)0682 mL
B)68.2 mL
C)0)0330 mL
D)33.0 mL

Question 36

What volume of 8.25 M NaOH solution must be diluted to prepare 2.40 L of 0.500 M NaOH solution?

A)39.6 L
B)0)356 L
C)438 mL
D)145 mL

Question 37

What is the molarity of the solution obtained by diluting 125 mL of 2.50 M NaOH to 575 mL?

A)0)272 M
B)0)543 M
C)1)84 M
D)11.5 M

Question 38

How much water must be added when 125 mL of a 2.00 M solution of HCl is diluted to a final concentration of 0.400 M?

A)125 mL
B)500 mL
C)625 mL
D)750 mL

Question 39

In order to prevent the process of either crenation or hemolysis with red blood cells an intravenous solution concentration should be ________ to the concentration of blood.

A)hypotonic
B)hypertonic
C)isotonic
D)all of these

Question 40

The process of crenation occurs when the concentration outside a cell is ________ and is said to be ________.

A)lower in concentration; hypotonic
B)lower in concentration; hypertonic
C)higher in concentration; hypotonic
D)higher in concentration; hypertonic

Question 41

The transport of nitrogen molecules across a cell membrane occurs via:

A)passive diffusion
B)facilitated transport
C)active transport
D)all of the above

Question 42

The transport of glucose molecules across a cell membrane occurs via:

A)passive diffusion
B)facilitated transport
C)active transport
D)all of the above

Question 43

A solution is also known as a ________ mixture.

Question 44

In a solution the particles are ________ distributed.

Question 45

Blood is not a colloid but a ________.

Question 46

Homogenized milk is not a solution but a ________.

Question 47

In a colloid the suspended particles do or do not settle out over time?

Question 48

In a suspension the particles do or do not settle out over time?

Question 49

A solution consists of 150 mL of isopropanol and 50 mL of water. Which is the solute?

Question 50

The golden rule of solubility states that, "like dissolves ________."

Question 51

Henry's law states that the solubility of a gas in a liquid ________ with increasing ________.

Question 52

The solubility of a gas in water ________ with increasing temperature.

Question 53

A solution that contains all the solute that it can contain is called a ________ solution.

Question 54

Identify the following as weak, strong or non-electrolytes.

-KNO₃

A)strong
B)weak
C)Non

Question 55

Identify the following as weak, strong or non-electrolytes.

-HCl

A)strong
B)weak
C)Non

Question 56

Identify the following as weak, strong or non-electrolytes.

-C₂H₅OH

A)strong
B)weak
C)Non

Question 57

Identify the following as weak, strong or non-electrolytes.

-NH₃(aq)

A)strong
B)weak
C)Non

Question 58

Identify the following as weak, strong or non-electrolytes.

-NaOH

A)strong
B)weak
C)Non

Question 59

Identify the following as weak, strong or non-electrolytes.

-C₂H₅COOH

A)strong
B)weak
C)Non

Question 60

Identify the following as weak, strong or non-electrolytes.

-C₁₂H₂₂O₁₁

A)strong
B)weak
C)Non

Question 61

Soluble covalent compounds do not conduct electricity and are therefore called ________.

Question 62

K₂CO₃ dissolves in water and produces ________ and ________ ions.

Question 63

NH₂CONH₂ is a ________electrolyte.

Question 64

A solution that contains 3.0 moles of Mg²⁺ ions contains ________ Eq Mg²⁺.

Question 65

Ethylene glycol (C₂H₆O₂), a nonelectrolyte, is used as antifreeze in car radiators. A solution containing 86.0 g of ethylene glycol dissolved in 465 g of water has a density of 1.35 g/mL at 25 °C. Calculate the following:

A)the %m/m of the ethylene glycol in this solution.
B)the molarity of the ethylene glycol in this solution.

Question 66

An aqueous solution is made by dissolving 45.0 g of H₂SO₄ in 850. g of water. The density of water is 1.00 g/mL.

A)What is the concentration of the starting solution in percent by mass (%m/m)?
B)What is the molarity of the H₂SO₄ solution?
C)If 25.0 mL of this solution is diluted to 500. mL, what is the resulting molarity?

Question 67

Calculate the molarity of a solution prepared by dissolving 14.7 g of Ca(NO₃)₂ in enough water to make 750. mL of solution.

Question 68

Calculate the grams of solute in 25.0 mL of a 2.50%m/v solution of fructose.

Question 69

What is the %m/m of a solution made from 21.0 g NaCl in 5.00 × 10² mL of solution? (Density of the solution is 1.14 g/mL)

Question 70

A cup of coffee may contain as much as 300. mg of caffeine, C₈H₁₀O₂. Calculate the molarity of caffeine in one cup of coffee. (4 cups = 1 L)

Question 71

An intravenous electrolyte solution has a Na⁺ ion concentration of 154 mEq/L. If a patient in the hospital receives 1500 mL of this solution how many equivalents have they received?

Question 72

An intravenous maintenance solution that is 5.0% dextrose contains 15 mEq/L HPO₄^2-. If a patient receives 1750 mL of this solution to maintain their electrolyte solution, how many equivalents of the HPO₄^2- are in this amount?

Question 73

What is the concentration in ppm and ppb of a solution that contains 45 mg of lead in 1750 mL of solution?

Question 74

How much of a 2.75 M solution of AgNO₃ in mL is needed to make 1.25 L of a 0.150 M solution of this same compound?

Question 75

50.0 mL of a 0.250 M sucrose solution was diluted to 4.00 × 10² mL. What is the concentration of the new solution?

Question 76

Define the terms isotonic, hypotonic and hypertonic solutions in relationship to a cell.

Question 77

Osmosis is the passage of water molecules through a semi-permeable membrane from a solution of ________ concentration to ________ concentration.

Question 78

Define the term "semipermeable."

Question 79

Why do your fingers wrinkle after you spend a lot of time swimming in the ocean?

Question 80

If physiological saline has a concentration of 0.90% (m/v)NaCl, identify the following solutions as isotonic, hypotonic or hypertonic:

A)0.25% (m/v)NaCl
B)0.90% (m/v)NaCl
C)1.8% (m/v)NaCl