Deck 7: Solutions and Colloids

Question 1

What volume of a 10.00% (w/v)solution of sugar is needed to provide 2.00 g of sugar?

A)0.200 liter
B)1.00 mL
C)20.0 mL
D)5.00 mL

Answer 1

20.0 mL

Question 2

How many moles of Na₂CO₃ are needed to react with 750 mL of 0.250 M H₂SO₄ solution? Na₂CO₃ + H₂SO₄ $\rightarrow$ Na₂SO₄ + CO₂ + H₂O

A)3.00* 10³
B)0.333
C)1.33
D)0.188

Answer 2

0.188

Question 3

As NH₄NO₃ dissolves in water,the resulting solution becomes colder.Which of the following expressions is most correct?

A)
B)
C)
D)

Answer 3

Question 4

A solution is made by dissolving 5.84 grams of NaCl in enough distilled water to give a final volume of 1.00 L.What is the molarity of the solution?

A)0.100
B)1.00
C)0.0250
D)0.400

Question 5

Which of the following statements relating to a solution is not correct?

A)A solution may contain more than one solute.
B)A solution may contain only one solute.
C)Water is always the solvent in a solution.
D)More than one correct response given.

Question 6

A solution is made by dissolving 15.0 mL of oil in enough gasoline to give 50.0 mL of solution.What is the % (v/v)of oil in the solution?

A)30.0
B)23.1
C)42.9
D)3.33

Question 7

You want to remove as much CO₂ gas as possible from a water solution.Which of the following treatments would be most effective?

A)cool the solution
B)filter the solution
C)boil the solution
D)aerate the solution

Question 8

A solution is made by dissolving a small amount of salt in a beaker of water.The water is referred to as the

A)precipitate.
B)filtrate.
C)solvent.
D)solute.

Question 9

How many mL of 6.00 M HCl are needed to prepare 1500 mL of 0.200 M HCl solution?

A)1.80 *10⁴
B)125
C)2.00 *10^-3
D)50.0

Question 10

Which of the following pairs can produce a homogeneous mixture?

A)water and sand
B)oil and vinegar
C)vinegar and glucose
D)calcium carbonate and water

Question 11

How many grams of solid KCl are needed to prepare 250 mL of 0.235 M solution?

A)9.32
B)31.3
C)15.6
D)4.38

Question 12

When solid NaOH is dissolved in water,the solution becomes hot.The solution process is

A)exothermic.
B)endothermic.
C)neither exothermic nor endothermic.
D)Can't be classified.

Question 13

Suppose a solution contains 200 g water and 15 g glucose.Which of the following statements is true?

A)Glucose would be classified as the solvent.
B)Water would be classified as the solvent.
C)Either component could be classified as the solvent.
D)More than one response is correct.

Question 14

What is the molarity of a solution containing 0.325 moles of solute in 250 mL of solution?

A)1.30 *10^-3
B)1.30
C)0.769
D)8.13 * 10^-2

Question 15

Iodine,I₂,is very slightly soluble in water,a polar solvent,but quite soluble in toluene,a nonpolar solvent.What can be inferred about the nature of the I₂ molecule?

A)It is ionic.
B)It is polar.
C)It is nonpolar.
D)Nothing can be inferred.

Question 16

A salt sample is placed into some water and nearly all of it dissolves without stirring or heating.The resulting solution is

A)saturated.
B)supersaturated.
C)unsaturated.
D)impossible to determine.

Question 17

When will carbon dioxide in a carbonated soft drink dissolve best?

A)after shaking the container
B)after heating the container
C)after cooling the container
D)after releasing the pressure

Question 18

A solution is made by combining 4.00 g of sugar and 100 mL of water (density = 1.00 g/mL).What is the concentration in % w/w?

A)26.0
B)4.00
C)0.0400
D)3.85

Question 19

A solution is produced in which water is the solvent and there are four solutes.Which of the solutes can dissolve better if the solution is heated?

A)oxygen
B)sodium bicarbonate
C)argon
D)more than one response is right

Question 20

Which compound is most soluble in a polar solvent?

A)silver nitrate
B)silver chloride
C)silver carbonate
D)all are of equal solubility

Question 21

Compared to pure water,a salt water solution will have a

A)lower vapor pressure,freezing point and boiling point.
B)higher vapor pressure,freezing point and boiling point.
C)lower vapor pressure and freezing point and a higher boiling point.
D)higher freezing point and a lower vapor pressure and boiling point.

Question 22

A solution is prepared by dissolving 4.66 g of KCl in enough distilled water to give 250 mL of solution.KCl is a strong electrolyte.How will the freezing point of the solution be different from that of pure water? (Note: K_f for water is 1.86°C/M.)

A)solution will be 0.930°C lower than water
B)solution will be 0.475°C lower than pure water
C)solution will be 0.930°C higher than pure water
D)solution will be 0.475°C higher than pure water

Question 23

A solution is prepared by adding 25.0 mL of 1.30 M AlCl₃ solution to a flask,and then adding enough water to give a final volume of 200.0 mL.What is the molarity of the solution?

A)0.260
B)0.163
C)6.50
D)1.24

Question 24

Calculate the number of moles of ZnCl,in 100 mL of 0.300 M solution.

A)3.00* 10^-2
B)0.300
C)30.0
D)3.00

Question 25

The rate of osmosis

A)can be increased by having larger pores in the membrane.
B)can be increased by removing the membrane.
C)can be increased by an increase in the atmospheric pressure.
D)cannot be increased by any of the responses.

Question 26

A 0.9% NaCl (w/w)solution in water is

A)produced by mixing 0.9 moles of NaCl in a 100 moles of water.
B)produced and has the same final volume as a 0.9% solution in ethyl alcohol.
C)a solution that boils at or above 100 $\degree$ C.
D)All of these responses are correct.

Question 27

Which of the following tend to stabilize colloids and prevent suspended particles from settling?

A)presence of emulsifying agents
B)absorption of charges by colloid particles
C)absence of ionic salts
D)more than one response is correct

Question 28

Changes in boiling point,freezing point,and vapor pressure are

A)the same for 2 M NaCl as they are for 2 M CaCl_2.
B)the same for 50 mL of 2 M NaCl as they are for 250 mL of 1 M NaCl.
C)the same for 75 mL of 2 M NaCl as they are for 50 mL of 2 M NaOH.
D)the same at 1 atm as at 1.55 atm.

Question 29

Which of the following pass through both osmotic and dialysis membranes?

A)solvent molecules
B)large molecules
C)cations
D)anions

Question 30

An isotonic salt solution is 0.90% (w/w)NaCl in water.How many grams of NaCl are contained in 1.00 kg of such a solution?

A)0.090
B)0.90
C)9.0
D)90

Question 31

Which of the following pairs correctly represent similar functions for a solution component and a colloid component?

A)solvent/dispersed phase
B)solute/dispersion medium
C)solvent/dispersion medium
D)more than one response is correct

Question 32

The boiling point of a solution of sugar water is

A)higher than that of pure solvent.
B)the same as that of pure solvent.
C)lower than that of pure solvent.
D)impossible to determine.

Question 33

Two solutions with concentrations of 2% sugar and 4% sugar,respectively,are separated by a semipermeable membrane.During osmosis,there is a net flow of

A)sugar molecules from the concentrated to the dilute solution.
B)sugar molecules from the dilute to the concentrated solution.
C)water molecules from the concentrated to the dilute solution.
D)water molecules from the dilute to the concentrated solution.

Question 34

In the colloid known as mayonnaise,the dispersed phase is _____ .

A)a gas
B)a liquid
C)a solid
D)unknown

Question 35

The spores from many molds produce an allergic reaction in many individuals.If mold spores in the air were to be considered a colloid,which technique would remove the spores best from a functioning air conditioner duct?

A)Place a filter made from woven fiberglass fibers in the duct.
B)Install an electrical device with both positive and negative poles.
C)Install an ultraviolet light producing device in the duct.
D)All of these responses work to the same extent.

Question 36

What is the underlying process involved in dialysis?

A)mixtures are homogenous.
B)osmosis is due to a difference in solution concentrations.
C)pressure is applied to the blood squeezing out the impurities.
D)an electrical potential separates the blood from the impurities.

Question 37

What is the osmotic pressure of a 0.050 M solution of AlCl₃ in water that is at 0.00 $\degree$ C? Consider AlCl₃ to be a strong electrolyte.

A)8.5 *10² torr
B)1.1 atm
C)2.2 atm
D)3.4 * 10³ torr

Question 38

The vapor pressure of a pure solvent is

A)higher than that of a solution.
B)impossible to determine.
C)the same as that of a solution.
D)lower than that of a solution.

Question 39

What volume of ethyl alcohol is contained in 35 mL (1 oz.)of 86 proof liquor,which is 43% (v/v)alcohol?

A)30 mL
B)43 mL
C)15 mL
D)37 mL

Question 40

You have a patient who is suffering from the "bends".What gas is in excess in the blood?

A)nitrogen
B)oxygen
C)helium
D)all of these

Question 41

The ability to see the scattering of light when passed through a colloid is known as

A)the dispersing effect.
B)a scattering ratio.
C)an emulsifying agent.
D)the Tyndall effect.

Question 42

The primary intermolecular attractions between CH₃-OH and H₂O are

A)hydrogen bonds.
B)dispersion forces.
C)covalent bonds.
D)dipolar forces.

Question 43

Polar substances tend to dissolve in non-polar solvents.

Question 44

Express the following concentration of solution in terms of molarity: 3.00 L of solution contains 1.75 mol of solute.

A)5.25 M
B)0.583 M
C)1.71 M
D)too little information to know

Question 45

Which of the following would be considered a strong electrolyte?

A)salt
B)sugar
C)acetic acid
D)all of the choices

Question 46

When sodium acetate dissolves in water,the following reaction occurs. This solution could be used

A)in a hot pack.
B)in a cold pack.
C)either a hot pack or cold pack.
D)neither a hot pack or cold pack.

Question 47

Drinking water can be purified by which of the following methods?

A)reverse osmosis
B)distillation
C)ion exchange
D)all of the choices

Question 48

A solution is prepared at 75 °C by dissolving 50.0 g of A in 100 g of water.When this solution is cooled to 15 °C what happens based on the following solubility plot for A.

A)Solid A crystallizes and the solution is unsaturated.
B)Solid A dissolves and the solution is supersaturated.
C)Solid A crystallizes and the solution is saturated.
D)Solid A dissolves and the solution is unsaturated.

Question 49

You discover that your roommate has left a half-full bottle of cola on the kitchen counter without replacing the cap - AGAIN!.Not surprisingly,the cola is now flat (all carbonation is gone).Why did this happen?

A)The solubility of the carbon dioxide gas in the cola has decreased due to it being left at a lower pressure.
B)Warm bottles of cola will lose their carbonation faster than cold ones,even if the lid had been left on.
C)Oxygen in the atmosphere reacts with the cola,eliminating the carbonation.
D)The solubility of the carbon dioxide gas diffuses through the wall of the bottle.

Question 50

Which of the following correctly arranges 1.00 M solutions of the strong electrolytes in order of increasing boiling point (lowest to highest)?

A)
B)
C)
D)All have the same boiling point.

Question 51

A solution is prepared at 75 °C by dissolving 50.0 g of A in 100 g of water.Which of the following correctly classifies this solution based on the solubility chart for A given below?

A)saturated
B)unsaturated
C)supersaturated
D)immiscible

Question 52

Citric acid,a natural food preservative,accounts for the tartness of citrus fruits.It is shown below.About 730 g of this material can be dissolved in water,making a liter of solution.However,only about 1.5% of it dissociates.As such,it would be considered a _____.

A)nonelectrolyte
B)strong electrolyte
C)pseudoelectrolyte
D)weak electrolyte

Question 53

An ion in solution that is surrounded by water is a(n)____ ion.

A)hydrated
B)osmotic
C)saturated
D)colloid

Question 54

Which of the following is not considered a colligative property?

A)vapor pressure
B)boiling point
C)conductivity
D)freezing point

Question 55

The cleaning action of soaps and detergents is attributable to

A)their ionic character.
B)the long hydrocarbon tail in their structure.
C)their ability to dissociate into ions.
D)all of the above.

Question 56

When making some iced tea,you find that you can dissolve 100 grams of table sugar in a liter of tea at 20 ^oC.Based on this,what did you learn?

A)Based on the solubility,tea must be a nonpolar solvent.
B)The solubility of table sugar in tea at 20 ^oC is 100 g/L
C)Table sugar must be a strong electrolyte.
D)You can dissolved 100 grams of sugar in tea at 20 ^oC

Question 57

A colligative property

A)will only occur for aqueous solutions.
B)depends only on the number of species added to a solution.
C)results from increasing vapor pressure as a solute is added to a solvent.
D)All of the choices.

Question 58

During a surgical procedure,a wound was accidentally irrigated with deionized water,instead of normal saline.What would one expect to happen?

A)There would be a net movement of water into the exposed tissue.
B)Water would move out of the exposed tissue.
C)Sodium ions would migrate out of the exposed cells.
D)There would be no net effect since the solution was added externally.

Question 59

When a patient's blood electrolyte levels are evaluated,sodium,chloride and bicarbonate ions are commonly measured and the difference in the total positive and negative charges calculated.This difference is called the

A)ionic ratio.
B)isoelectric point.
C)electromotive constant.
D)anion gap.

Question 60

One test to determine if a mixture is a true solution or a colloid is ____.

A)physical state of the mixture
B)boiling point elevation
C)light scattering
D)color

Question 61

Weight-volume percentage solutions must be made in 100 mL increments.

Question 62

The more soluble a substance is,the faster it will dissolve.

Question 63

Solvents and hydrated ions can usually pass though dialyzing membranes

Question 64

The solubility of a substance can be measured in grams substance dissolved per liter of water.This is the same as expressing solubility in moles per liter.

Question 65

All ionic compounds are soluble in water.

Question 66

Oil should be a good solvent for polar compounds.

Question 67

Emulsions are destroyed by adding salt.

Question 68

Light scattering is an effective way to distinguish between true solutions and colloidal dispersions.

Question 69

Dialysis and osmosis are used for the same purposes.

Question 70

Rock candy (large table sugar crystals)can be produced by allowing a hot,saturated solution of sugar in water to cool off.

Question 71

Ionic compounds are generally insoluble in non-polar solvents.

Question 72

Dialysis can be used to separate solutions from colloids.

Question 73

Attractive forces between solute and solvent molecules are an important factor in solution formation.

Question 74

The %(w/v)of a solution is defined as:

Question 75

There is a 12 M aqueous HCl solution in the stock room,but a 6 M solution is required for an experiment.Doubling the volume of a 12 M sample with water will produce a 6 M solution.

Question 76

A mixture of sand and water would be an example of a colloidal suspension.

Question 77

Colloids can be stabilized by emulsifying agents.

Question 78

Colloids are considered to be homogenous mixtures.

Question 79

Putting a celery stick in distilled water results in the uptake of water by the celery.

Question 80

The solubility of gases in water increases with increasing temperature.