Deck 9: Solutions

Question 1

Which is not an example of a solution?

A)the mixture of gases in a SCUBA diving tank
B)a coin made from nickel and copper
C)spring water purchased at a supermarket
D)antifreeze in a car radiator
E)none of the above

Answer 1

none of the above

Question 2

Which of the following has the least effect on the solubility of a solid in a liquid solvent?

A)temperature
B)pressure
C)nature of the solvent
D)nature of the solute
E)concentration of solute

Answer 2

pressure

Question 3

A supersaturated solution

A)contains as much solvent as it can hold.
B)contains no double bonds.
C)contains dissolved solute in equilibrium with undissolved solid.
D)will rapidly precipitate if a seed crystal is added.
E)none of the above

Answer 3

will rapidly precipitate if a seed crystal is added.

Question 4

Which homogeneous mixture is opaque and has particles large enough to be filtered?

A)colloid
B)solution
C)suspension
D)both colloids and suspensions
E)none of the above

Question 5

When a solid dissolves,each molecule is removed from the crystal by interaction with the solvent.This process of surrounding each ion with solvent molecules is called

A)dilution.
B)solvation.
C)electrolysis.
D)hemolysis.
E)crenation.

Question 6

The dissolving process is exothermic when the energy

A)released in solvation exceeds the energy used in breaking up solute-solute and solvent-solvent interactions.
B)used in solvation exceeds the energy released in breaking up solute-solute and solvent-solvent interactions.
C)released in solvation is about the same as the energy used in breaking up solute-solute and solvent-solvent interactions.
D)used in solvation is less than the energy released in breaking up solute-solute and solvent-solvent interactions.
E)used in solvation is about the same as the energy released in breaking up solute-solute and solvent-solvent interactions.

Question 7

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

A)CH₃NH₂
B)CH₃CH₂OH
C)CH₃COOH
D)CH₃OCH₃
E)CH₃CH₂CH₂CH₂CH₃

Question 8

In a mixture of 5 mL water,10 mL alcohol,and 50 mL acetone the solvent(s)is(are)

A)acetone.
B)alcohol.
C)water.
D)acetone and alcohol.
E)alcohol and water.

Question 9

The number of components in a solution is

A)at least 2.
B)3.
C)4.
D)5.
E)6.

Question 10

Which statement about solubility is not true?

A)No additional solute will dissolve in a saturated solution.
B)A supersaturated solution is unstable.
C)Solubility of ionic solids increases greatly with temperature.
D)In a solution containing excess solute,an equilibrium exists between dissolved and undissolved solute.
E)The solubility of substances is measured as g solute/100 mL solvent.

Question 11

Which of the following can serve as the solvent in a solution?

A)a gas
B)a liquid
C)a solid
D)a mixture of commingled liquids
E)all of the above

Question 12

Water can be used to dissolve which type of compounds?

A)nonpolar compounds
B)polar compounds
C)ionic compounds
D)both A and B
E)both B and C

Question 13

All of the following statements describing solutions are true except

A)making a solution involves a physical change.
B)solutions are homogeneous.
C)the particles in a solution are atomic or molecular in size.
D)solutions are colorless.
E)solutions are transparent.

Question 14

The exothermic step in the dissolution of NaCl in water is

A)the separation of the ions in the salt.
B)the separation of the water molecules.
C)solvation (hydration)of the ions from the salt.
D)separation of the ions in the salt and the separation of the water molecules.

Question 15

Consider the following four liquids:
Water: highly polar;H-bonding
Hexanol: slightly polar;some H-bonding
Chloroform: slightly polar;no H-bonding
Octane: non-polar;no H-bonding
Which pair of liquids is immiscible?

A)water and octane
B)water and hexanol
C)hexanol and chloroform
D)chloroform and octane
E)none of the above

Question 16

The term miscible is used to describe which type of solution?

A)liquid/liquid
B)liquid/solid
C)gas/liquid
D)gas/gas
E)all of the above

Question 17

Which of the following statements about the solubility of gases in liquids is not correct?

A)A warm can of soda fizzes more than a cold can of soda when opened because gases are less soluble at higher temperature.
B)An opened can of soda goes "flat" because the partial pressure of carbon dioxide is lower in the atmosphere than in the unopened can.
C)A solution stored under an atmosphere of pure nitrogen will contain more dissolved nitrogen than the same solution stored under air because air is only 80% nitrogen.
D)Fish kills may occur in the summertime because an inadequate amount of oxygen is dissolved in the water.
E)none of the above

Question 18

Which of the following is miscible with CH₃CH₂OH?

A)CH₃CH₂CH₃
B)CH₃OH
C)CCl₄
D)CH₃CH₃
E)CBr₄

Question 19

Which statement best explains the meaning of the phrase "like dissolves like"?

A)A solvent will easily dissolve a solute of similar mass.
B)A solvent and solute with similar intermolecular forces will readily form a solution.
C)The only true solutions are formed when water dissolves a non-polar solute.
D)The only true solutions are formed when water dissolves a polar solute.
E)None of these statements is correct.

Question 20

Which of the following would be immiscible with carbon tetrachloride,CCl₄?

A)C₆H₁₂
B)CH₃CH₂OH
C)Br₂
D)C₃H₈
E)C₄H₁₀

Question 21

What is the molarity of a solution prepared by dissolving 48.0 g of NaOH in enough water to make 1.50 L of solution?

A)0.0313 M
B)0.556 M
C)0.800 M
D)1.28 M
E)32.0 M

Question 22

What is the molarity of a solution prepared by dissolving 3.50 mol NaCl in enough water to make 1.50 L of solution?

A)0.429 M
B)2.33 M
C)5.25 M
D)87.8 M
E)137 M

Question 23

Calculate the concentration of nitrogen gas in water with a nitrogen gas at a partial pressure of 0.826 atm above it.Henry's law constant for nitrogen in water is 6.8 × 10^-4 mol/L-atm.

A)5.6 × 10^-4 M
B)8.2 × 10^-3 M
C)1.2 × 10³ M
D)0.43 M

Question 24

Pressure has a large effect only on the solubility of ________ in liquids.

A)liquid
B)solid
C)gas
D)all of the above
E)none of the above

Question 25

What is the % (w/v)concentration of a solution containing 8.0 grams of alcohol in 50.0 mL of solution?

A)2.0%
B)4.0%
C)8.0%
D)16%
E)50%

Question 26

The solubility of gases in liquids

A)increases as temperature increases and increases as pressure increases.
B)decreases as temperature increases and increases as pressure increases.
C)decreases as temperature increases and decreases as pressure increases.
D)increases as temperature increases and decreases as pressure increases.
E)is independent of temperature and increases as pressure increases.

Question 27

In general,the solubility of ________ in water decreases as temperature increases.

A)gases
B)solids
C)liquids
D)none of these
E)all of these

Question 28

How much NaOH is present in a 250.mL sample of a 5.00% (w/v)solution?

A)5.00 g
B)10.0 g
C)12.5 g
D)25.0 g
E)250 g

Question 29

What is the molarity of a solution prepared by dissolving 0.750 mol CaCl₂ in enough water to make 0.500 L of solution?

A)0.375 M
B)0.667 M
C)1.50 M
D)83.2 M
E)166.5 M

Question 30

What is the molarity of a solution prepared by dissolving 1.25 mol of AgNO₃ in enough water to make 625 mL of solution?

A)2.00 M
B)0.00200 M
C)0.500 M
D)0.0118 M
E)0.340 M

Question 31

How many moles of HCl are present in 75.0 mL of a 0.200 M solution?

A)15.0 mol
B)2.67 mol
C)0.375 mol
D)0.275 mol
E)0.0150 mol

Question 32

Which solution is the most concentrated? Each choice refers to the same solute and solvent.

A)2.4 g solute in 2 mL solution
B)2.4 g solute in 5 mL solution
C)20 g solute in 50 mL solution
D)30 g solute in 150 mL solution
E)50 g solute in 175 mL solution

Question 33

The solubility of nitrogen in water exposed to the atmosphere,where the partial pressure of nitrogen is 593 mm,is 5.3 × 10^-4 M.At the same temperature,what would be the solubility of pure nitrogen,at a pressure of 760 mm?

A)4.1 × 10^-4 M
B)6.8 × 10^-4 M
C)1500 M
D)2400 M
E)none of the above

Question 34

Which solution is the least concentrated? Each choice refers to the same solute and solvent.

A)2.4 g solute in 2 mL solution
B)2.4 g solute in 5 mL solution
C)20 g solute in 50 mL solution
D)30 g solute in 150 mL solution
E)50 g solute in 175 mL solution

Question 35

What is the molarity of a solution prepared by dissolving 10.0 g of acetone,C₃H₆O,in enough water to make 125 mL of solution?

A)4.65 M
B)1.38 M
C)0.0465 M
D)0.0214 M
E)0.0125 M

Question 36

How many grams of NaOH are needed to make 750 mL of a 2.5% (w/v)solution?

A)3.9 g
B)7.5 g
C)19 g
D)20 g
E)50 g

Question 37

Which information is necessary to determine the molarity of a solution if the chemical formula of the solute is known?

A)only the mass of solute dissolved
B)only the volume of solvent used
C)the molar mass of both the solute and the solvent used
D)the mass of solute dissolved and the volume of solvent added
E)the mass of solute dissolved and the final volume of the solution

Question 38

All of the statements about molarity are correct except

A)the abbreviation is M.
B)the interpretation of the symbol is "moles of solute per mole of solvent."
C)moles = molarity × volume.
D)volume = moles/molarity.
E)the molarity of a diluted solution is less than the molarity of the original solution.

Question 39

What is the % (w/v)concentration of a solution containing 25.0 g of solute in 400.mL of solution?

A)2.50%
B)5.00%
C)6.25%
D)12.5%
E)25.0%

Question 40

How much NaCl is needed to make 50.0 mL of a 16% (w/v)solution?

A)2.0 g
B)4.0 g
C)8.0 g
D)12 g
E)16 g

Question 41

How many grams of Fe(NO₃)₃ are present in a 20.0 mL sample of a 0.500 M solution?

A)2.14 g
B)9.68 g
C)4.84 g
D)2.42 g
E)1.21 g

Question 42

How many grams of C₆H₁₂O₆ are needed to prepare 2.50 L of a 5.00% (w/v)solution?

A)1.25 g
B)0.200 g
C)12.5 g
D)125 g
E)200.g

Question 43

How many grams of CaCl₂ are needed to prepare 125 mL of a 1.50 M solution?

A)0.188 g
B)1.69 g
C)3.00 g
D)20.8 g
E)37.0 g

Question 44

A 50.0 mL sample of a 6.0 M solution of HCl is diluted to 200.mL.What is the new concentration?

A)24.0 M
B)6.0 M
C)2.10 M
D)2.00 M
E)1.50 M

Question 45

Calculate the concentration in ppm of a pollutant that has been measured at 450 mg per 150 kg of sample.

A)3.0 ppm
B)6.0 ppm
C)3000 ppm
D)330 ppm
E)none of the above

Question 46

All of the water in a 0.200 M solution of NaCl was evaporated and 0.150 mole of NaCl was obtained.What was the original volume of the sample?

A)30.0 mL
B)333 mL
C)750.mL
D)1000 mL (1.00 × 10³ mL)
E)1330 mL

Question 47

How many grams of water are needed to prepare 250.g of a solution that is 5.00% by mass NaCl?

A)5.00 g
B)12.5 g
C)238 g
D)245 g
E)1250 g

Question 48

Which list includes all the pieces of lab equipment needed to prepare a 0.500 M solution of NaCl from the pure salt and water?

A)buret;volumetric flask
B)buret;electronic balance
C)electronic balance;volumetric flask
D)electronic balance;graduated cylinder
E)volumetric pipet and bulb;volumetric flask

Question 49

Which procedure will produce 250 mL of a solution that is 4% by volume alcohol in water?

A)4 mL of alcohol is mixed with enough water to make 250 mL of solution.
B)10 mL of alcohol is mixed with enough water to make 250 mL of solution.
C)4 mL of alcohol is mixed with 250 mL of water.
D)10 mL of alcohol is mixed with 250 mL of water.
E)none of the above

Question 50

How many mL of 0.105 M AgNO₃ are needed for an experiment that requires 0.00510 mol of AgNO₃?

A)0.536 mL
B)17.8 mL
C)18.70 mL
D)20.6 mL
E)48.6 mL

Question 51

How many mL of a 5.00% (w/v)glucose solution are needed to provide 20.0 g of glucose?

A)5.00 mL
B)20.0 mL
C)4.00 mL
D)200.mL
E)400.mL

Question 52

What is the final concentration of a solution prepared by adding water to 50.0 mL of 1.5 M NaOH to make 1.00 L of solution?

A)0.075 M
B)0.030 M
C)1.5 M
D)7.5 M
E)30 M

Question 53

Normal saline is 0.920% (w/v)NaCl in water.How many grams of NaCl are needed to prepare 15.0 L of normal saline?

A)1.38 g
B)16.3 g
C)53.8 g
D)138 g
E)807 g

Question 54

How many mL of a 0.200 M HNO₃ solution contains 10.0 g of HNO₃?

A)2.00 mL
B)31.7 mL
C)159 mL
D)315 mL
E)793 mL

Question 55

How many grams of FeSO₄ are present in a 20.0 mL sample of a 0.500 M solution?

A)65.8 g
B)6.08 g
C)3.04 g
D)1.52 g
E)0.760 g

Question 56

A 50.0 mL sample of a 12.0 M solution of HCl is diluted to 250.mL.What is the new concentration?

A)60.0 M
B)12.0 M
C)10.4 M
D)3.00 M
E)2.40 M

Question 57

How many moles of solute are present in 12.0 L of 3.00 M HCl?

A)36.0 mol
B)4.00 mol
C)0.250 mol
D)3.00 mol
E)0.750 mol

Question 58

A 20.0 mL sample of CuSO₄ was evaporated to dryness,leaving 0.967 g of residue.What was the molarity of the original solution?

A)48.4 M
B)0.0207 M
C)0.0484 M
D)0.303 M
E)0.433 M

Question 59

Which list includes all the pieces of lab equipment needed to prepare 0.100 M H₃PO₄ from a 5.00 M solution of H₃PO₄?

A)buret;volumetric flask
B)buret;electronic balance
C)electronic balance;volumetric flask
D)electronic balance;graduated cylinder
E)volumetric pipet and bulb;volumetric flask

Question 60

How many mL of a 0.200 M KOH solution contains 10.0 g of KOH?

A)11.2 mL
B)50.0 mL
C)178 mL
D)281 mL
E)891 mL

Question 61

Which solution will have the highest boiling point?

A)0.050 M KNO₃
B)0.075 M CaCl₂
C)0.025 M NH₄NO₃
D)0.020 M Na₃PO₄
E)0.10 M C₆H₁₂O₆

Question 62

How many mL of 16 M NH₃ are needed to prepare 2.00 L of a 2.00 M solution?

A)250 mL
B)125 mL
C)16 mL
D)8.0 mL
E)4.0 mL

Question 63

Which aqueous solution will have the lowest freezing point?

A)0.60 molal sucrose
B)0.50 molal KF
C)0.60 molal glucose
D)0.24 molal FeI₃

Question 64

Considering 1.0 M solutions of each substance,which contains the largest concentration of ions?

A)K₂SO₄
B)FeCl₃
C)NaOH
D)NH₃
E)KCl

Question 65

A water solution of sodium chloride is a good conductor of electricity.Due to this property,table salt is classified as a(n)

A)weak electrolyte.
B)strong electrolyte.
C)non-electrolyte.
D)semi-electrolyte.
E)none of these.

Question 66

How many mL of 14.5 M NH₃ are needed to prepare 2.00 L of a 1.00 M solution?

A)138 mL
B)69.0 mL
C)276 mL
D)29.0 mL
E)7.25 mL

Question 67

Considering 0.10 M solutions of each substance,which contains the smallest concentration of ions?

A)(NH₄)₃PO₄
B)Ca(NO₃)₂
C)FeSO₄
D)K₂CO₃
E)Na₂SO₄

Question 68

Which has the lowest boiling point?

A)0.1 M Na₂SO₄
B)0.1 M glucose,C₆H₁₂O₆
C)0.1 M MgCl₂
D)0.1 M Al(NO₃)₃
E)pure water

Question 69

Which has the highest boiling point?

A)0.1 M Na₂SO₄
B)0.1 M glucose,C₆H₁₂O₆
C)0.1 M MgCl₂
D)0.1 M Al(NO₃)₃
E)pure water

Question 70

Which statement comparing solutions with pure solvents is not correct?

A)A solution containing a non-volatile solute has a lower vapor pressure than pure solvent.
B)A solution containing a non-volatile solute has a lower boiling point than pure solvent.
C)A solution containing a non-volatile solute has a lower freezing point than pure solvent.
D)A solution will have a greater mass than an equal volume of pure solvent if the solute has a molar mass greater than the solvent.
E)none of the above

Question 71

How many grams are contained in one equivalent of iron (III)ion,Fe^+3?

A)168 g
B)55.9g
C)18.6g
D)0.0537 g
E)6.02 × 10²³ g

Question 72

What is the final concentration of a solution prepared by using 75.0 mL of 18.0 M H₂SO₄ to prepare 500.mL of solution?

A)8.33 × 10^-3 M
B)1.20 M
C)2.70 M
D)2.35 M
E)15.7 M

Question 73

Which one of the following would act like a strong electrolyte in an aqueous solution?

A)KNO₃
B)CH₃OH
C)CCl₄
D)NH₃

Question 74

Which solution will have the lowest boiling point?

A)0.050 M KNO₃
B)0.075 M CaCl₂
C)0.025 M NH₄NO₃
D)0.020 M Na₃PO₄
E)0.10 M C₆H₁₂O₆

Question 75

How many grams are in 10.0 mEq of Ca²⁺?

A)0.201 g
B)40.1 g
C)20.1 g
D)0.802 g
E)0.401 g

Question 76

Which substance is not an electrolyte?

A)NaCl
B)HCl
C)NH₄NO₃
D)KOH
E)CH₄

Question 77

How many mL of water should be added to 50.0 mL of a 15.0 M H₂SO₄ solution to give a final concentration of 0.300 M?

A)950 mL
B)1000 mL
C)2450 mL
D)2500 mL
E)2550 mL

Question 78

What is the final concentration if 100 mL of water is added to 25.0 mL of 6.0 M NaCl?

A)1.2 M
B)1.5 M
C)6.0 M
D)24 M
E)30 M

Question 79

If a normal blood sample contains 4.5 mEq/L of calcium ion,how many mg of calcium are contained in a
Blood sample?

A)9.0 mg
B)5.6 mg
C)2.8 mg
D)2.3 mg
E)1.4 mg

Question 80

How many milliequivalents of chloride ion are contained in a sample that is determined to contain
Of chloride ion?

A)48.9 mEq
B)41.0 mEq
C)25.7 mEq
D)20.5 mEq
E)10.3 mEq