Deck 13: Solutions

Question 1

Steel is an example of a solid solution.

Answer 1

True

Question 2

Tap water contains dissolved nitrogen and oxygen.

Answer 2

True

Question 3

Salt water is an example of a strong electrolyte solution.

Answer 3

True

Question 4

The minor component in a solution is called the solvent.

Question 5

When a chunk of gold is melted and poured into the shape of an ingot,an aqueous solution of gold has been created.

Question 6

Air is an example of a gaseous solution.

Question 7

A sugar solution is an example of a weak electrolyte solution.

Question 8

A supersaturated solution is unstable and crystallization usually occurs.

Question 9

Sugar solutions conduct electricity because the dissolved particles are molecules.

Question 10

The solubility of solids in water generally increases with increasing temperature.

Question 11

Vitamin C is a water-soluble vitamin,so it is likely that this vitamin is polar.

Question 12

Ionic solutes typically dissolve in nonpolar solvents.

Question 13

The tragedy at Lake Nyos in Cameroon,West Africa was due to the sudden release of excessive amounts of nitrogen dissolved in the lake water.

Question 14

The tragedy at Lake Nyos in Cameroon,West Africa,was due to the sudden release of excessive amounts of carbon monoxide dissolved in the lake water.

Question 15

It would be expected that methanol (CH₃OH)would be more soluble in water than methane (CH₄)would be.

Question 16

A solution is a homogeneous mixture of two or more substances.

Question 17

The fact that the oceans contain salt water shows that polar solvents dissolve ionic solutes.

Question 18

A saturated solution holds the maximum amount of solute under the solution conditions.

Question 19

The major component in a solution is called the solute.

Question 20

Solubility is formally defined as the amount of a compound that can be dissolved in water.

Question 21

Warm beer goes flat quicker than cold beer.

Question 22

A semipermeable membrane allows only half the amount of a substance to pass through it.

Question 23

Colligative properties are independent of the amount of solute in solution.

Question 24

One liter of 6.0 M HNO₃ contains the same number of H⁺ ions as does one liter of 6.0 M H₂SO₄.

Question 25

A stock solution is a more concentrated form than what is typically used in a lab.It often requires further dilution.

Question 26

Upon completing a dilution from a stock solution,you will always have more volume of solution than you started with and it will have a lower concentration than the stock solution.

Question 27

A 0.10 molality solution of the sugar glucose (molecular weight = 180.10 g/mol)and a 0.10 molality solution of sucrose (molecular weight = 342.34 g/mol)would both boil at the same temperature.

Question 28

Osmosis is the process in which a solvent moves from an area of low solute concentration to an area of high solute concentration.

Question 29

The solubility of gases in water decreases with increasing temperature.

Question 30

A solution that is 13.58 percent by mass of sugar contains 13.75 grams of sugar dissolved in 87.5 grams of water.

Question 31

The solubility of gases in water increases with increasing pressure above the water.

Question 32

One liter of a 2.0 M NaOH (aq)solution contains the same number of Na⁺ ions as does one liter of a 1.0 M Na₂CO₃ (aq)solution.

Question 33

The molarity of a solution prepared by dissolving 15.0 grams of NaCl in 1000 mL water is 0.15M .

Question 34

Molarity is defined as the moles of solute per liter of solution.

Question 35

A sample of salt water will freeze at a higher temperature than a sample of pure water.

Question 36

Molality is calculated by dividing grams of solute by kilograms of solution.

Question 37

Adding a nonvolatile solute to a liquid will cause boiling point depression and freezing point elevation.

Question 38

A solution that is 35 percent by mass NaCl contains 35 grams of NaCl dissolved in 100 grams of water.

Question 39

If 50 grams of salt dissolves into 250 grams of water,the resulting solution must have a mass of 300 grams.

Question 40

The terms "molarity"and "molality" are considered identical and can always be used interchangeably.

Question 41

The solubility of Pb(NO₃)₂ is 55 grams per 100 g H₂O at 20°C.Which term would properly describe a solution where 44 grams of Pb(NO₃)₂ is added to 100 grams of water at this temperature?

A)insoluble
B)unsaturated
C)saturated
D)supersaturated
E)none of the above

Question 42

Which of the following compounds is a strong electrolyte?

A)HCl
B)NaCl
C)NH₄Cl
D)NaC₂H₃O₂
E)all of the above

Question 43

The solubility of solids in water:

A)is independent of pressure above solution.
B)increases with increasing pressure above solution.
C)decreases with increasing pressure above solution.
D)Solids are not soluble in water.
E)none of the above

Question 44

The solubility of solids in water:

A)is independent of the temperature.
B)increases with increasing temperature.
C)decreases with increasing temperature.
D)Solids are not soluble in water.
E)none of the above

Question 45

Which of the following substances is NOT a solution?

A)air
B)brass
C)vodka
D)copper
E)All of the above are solutions.

Question 46

If you put a living cell into seawater containing a higher concentration of sodium chloride,the cell loses water through osmosis.

Question 47

The oxygen in the air we breath is classified as:

A)the solute in a homogeneous gas mixture.
B)the solvent in a homogeneous gas mixture.
C)the solute in a heterogeneous gas-liquid mixture.
D)the solvent in a simple mixture.
E)none of the above

Question 48

Which of the following substances is NOT a solution?

A)homogenized milk
B)bronze
C)sea water
D)soda
E)All of the above are solutions.

Question 49

If you prepare a solution by adding sufficient amount of solute so that after heating and cooling the solution there is a visible amount of solid solute left in the bottom of the beaker,the solution would be considered ________.

A)unsaturated
B)saturated
C)supersaturated
D)thermally saturated
E)none of the above

Question 50

Which of the following compounds is a strong electrolyte?

A) C₆H₁₂O₆
B) C₇H₁₄O₅
C) C₄H₈O₂
D) NaC₂H₃O₂
E)all of the above

Question 51

Which compound below forms an electrolyte solution when dissolved in water?

A)Cl₂
B)KOH
C)CH₃CH₂OH
D)C₁₂H₂₂O₁₁ (sucrose)
E)none of the above

Question 52

Which of the following substances is NOT a solution?

A)humid air
B)beer
C)oxygen
D)steel
E)All of the above are solutions.

Question 53

If the solubility of sodium chloride is 36 grams per 100 grams of water,which of the following solutions would be considered unsaturated?

A)5.8 moles of NaCl dissolved in 1 L of water
B)3.25 moles of NaCL dissolved in 500 ml of water
C)1.85 moles of NaCl dissolved in 300 ml of water
D)none of the above

Question 54

In order for a solute to dissolve in solution:

A)the solute-solvent forces must be greater than the solute-solute forces.
B)the solute-solute forces must be greater than the solute-solvent forces.
C)the solute-solvent forces must equal the solute-solute forces.
D)the polarity of the solute and solvent must be opposite.
E)none of the above

Question 55

Which of these compounds would you expect to be least soluble in water?

A)CH₃OH
B)NaCl
C)N₂
D)NH₃
E)not enough information

Question 56

Suppose a vodka martini contains 30% alcohol with the remaining portion of the drink composed of water.What is the solute in this type of martini?

A)water
B)alcohol
C)ice
D)olive
E)none of the above

Question 57

Osmotic pressure is the pressure required to completely reverse the direction of solvent movement in osmosis.

Question 58

If the solubility of sodium acetate (Molar mass = 82 g/mol)is 76 grams per 100 grams of water,which of the following solutions would be considered supersaturated?

A)8.5 moles of sodium acetate dissolved in 1 L of water
B)5.5 moles of sodium acetate dissolved in 500 mL of water
C)1.8 moles of sodium acetate dissolved in 300 mL of water
D)1.2 moles of sodium acetate dissolved in 200 mL of water
E)none of the above

Question 59

The tragedy at Lake Nyos in Cameroon,West Africa,was caused by:

A)the release of excessive amounts of nitrogen gas that had been dissolved in the water at the bottom of the lake.
B)the release of excessive amounts of oxygen gas that had been dissolved in the water at the bottom of the lake.
C)the release of excessive amounts of carbon dioxide that had been dissolved in the water at the bottom of the lake.
D)the release of excess water stored in the volcanic lake which flooded the village below.
E)none of the above

Question 60

Hexane,a nonpolar solvent,will dissolve which of the following substances?

A)sodium chloride
B)oil
C)ammonium acetate
D)vinegar (acetic acid)
E)none of the above

Question 61

What is the molarity of a solution prepared by dissolving 10.7 grams NaI in 0.250L ?

A)42.8
B)0.0714
C)2.86
D)0.286
E)none of the above

Question 62

How many moles of NaF are in 34.2 grams of a 45.5% by mass NaF solution?

A)0.814
B)75.2
C)15.6
D)0.371
E)none of the above

Question 63

How many grams of LiF would be present in 575 mL of 0.750 M LiF solution?

A)11.2
B)0.0338
C)1.12 × 10⁴
D)19.9
E)33.8

Question 64

How many grams of a 23.4% by mass NaF solution is needed if you want to have 1.33 moles of NaF?

A)55.9
B)31.1
C)13.1
D)239
E)none of the above

Question 65

You need to prepare 2.00 L of 0.100 M Na₂CO₃ solution.The best procedure is to weigh out:

A)10.6 g Na₂CO₃ and add 2.00 L of water to it.
B)21.2 g Na₂CO₃ and add 2.00 L of water to it.
C)10.6 g Na₂CO₃ and add water until the final solution has a volume of 2.00 L.
D)21.2 g Na₂CO₃ and add water until the final solution has a volume of 2.00 L.

Question 66

A solution contains 100.0 g water,10.0 g NaCl,and 15.0 g methanol.What is the mass percent of methanol in the solution?

A)8.00%
B)10.0%
C)12.0%
D)15.0%
E)none of the above

Question 67

Given that you wished to use exactly 0.325 mole of NaCl to prepare a 2.50 M NaCl solution,how many milliliters of solution must you prepare?

A)130.mL
B)0.130 mL
C)7.69 mL
D)0.813 mL
E)none of the above

Question 68

What is the mass percent of an ammonium carbonate solution prepared by dissolving 33.2 grams of solid into 39.5 grams of water?

A)84.1%
B)72.7%
C)45.7%
D)54.3%
E)none of the above

Question 69

A solution is saturated in both nitrogen gas (N₂)and sodium iodide (NaI)at 50°C.When the solution is cooled to 25°C,which of the following is most likely to occur?

A)Some nitrogen gas bubbles out of solution.
B)Some sodium iodide will precipitate out of solution.
C)Both A and B will happen.
D)Nothing will happen.
E)not enough information

Question 70

What is the mass percent of a sodium fluoride solution prepared by dissolving 0.64 moles of sodium fluoride into 63.5 grams of water?

A)26.9%
B)42.3%
C)70.3%
D)29.7%
E)none of the above

Question 71

What is the mass percent of a solution prepared by dissolving 18.9 grams of solid into 39.5 grams of water?

A)47.8%
B)58.4%
C)32.4%
D)The identity of the compound must be known.
E)none of the above

Question 72

We dissolve 2.45 g of sugar in 200.0 g water.What is the mass percent of sugar in the solution?

A)1.21%
B)1.23%
C)2.42%
D)123%
E)none of the above

Question 73

The solubility of a gas in a liquid can always be increased by:

A)increasing the temperature of the solvent.
B)decreasing the polarity of the solvent.
C)decreasing the pressure of the gas above the solvent.
D)increasing the pressure of the gas above the solvent.
E)none of the above

Question 74

The solubility of gases in water:

A)is independent of temperature.
B)increases with increasing temperature.
C)decreases with increasing temperature.
D)gases are not soluble in water.
E)none of the above

Question 75

How many moles of KOH are contained in 750.mL of 5.00 M KOH solution?

A)6.67 mol
B)3.75 × mol
C)56.1 mol
D)3.75 mol
E)none of the above

Question 76

Which among the following is NOT true about the solubility of a solid in water?

A)The solubility is not affected by pressure.
B)The solubility generally increases as temperature increases.
C)Solid crystallizes when a saturated solution is prepared at a higher temperature and then cooled.
D)A saturated solution prepared at a lower temperature becomes unsaturated when heated to a higher temperature.
E)none of the above

Question 77

How many grams of KCl are needed to make 50.0 mL of 2.45M KCl?

A)9.13
B)1.52
C)91.3
D)0.123
E)none of the above

Question 78

Solubility of gases in water:

A)is independent of pressure above solution.
B)increases with increasing pressure above solution.
C)decreases with increasing pressure above solution.
D)Gases are not soluble in water.
E)none of the above

Question 79

When preparing sodium hydroxide solution,it is best to use water that does not contain any dissolved carbon dioxide as it reacts with the sodium hydroxide.Removing the carbon dioxide can be accomplished by:

A)vigorously stirring the solution.
B)using water fresh out of the purification system.
C)boiling the water.
D)Nothing can be done to remove dissolved gases.
E)none of the above

Question 80

What is the molarity of a solution prepared by dissolving 54.3 g of Ca(NNO₃)₂ into 355 mL of water?

A)0.331 M
B)0.932 M
C)0.117 M
D)1.99 M
E)none of the above