Deck 9: Solutions

Question 1

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

Answer 1

both B and C

Question 2

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.

Answer 2

solutions are colorless.

Question 3

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.

Answer 3

decreases as temperature increases and increases as pressure increases.

Question 4

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 5

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 6

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 7

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 8

The dissolving process is exothermic when

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

Question 9

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 10

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 11

An ionic compounded that attracts atmospheric water strongly is said to be

A)diluted.
B)hygroscopic.
C)immiscible.
D)miscible.
E)soluble.

Question 12

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 13

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

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

Question 14

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 15

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

Question 16

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

Question 17

The number of components in a solution is ________.

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

Question 18

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 19

A substance represented by a formula written as M_x

A)colloid.
B)solid hydrate.
C)solute.
D)solvent.
E)suspension.

Question 20

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 21

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 22

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 23

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 24

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 25

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 26

How much NaCl is needed to make 75 mL of a 12% (w/v)solution?

A)30 g
B)6.0 g
C)7.5 g
D)9.0 g
E)12 g

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 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 29

What is the % (w/v)concentration of a solution containing 12 grams of solute in 400 mL of solution?

A)1.2%
B)3.0%
C)4.0%
D)6.0%
E)12%

Question 30

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 31

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 32

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 33

How much NaCl is present in 25.0 mL of a 12.0% (w/v)solution?

A)3.00 g
B)4.00 g
C)6.00 g
D)12.0 g
E)48.0 g

Question 34

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 35

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 36

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 37

How much NaCl is present in a 15.0 mL sample of a 12.0% (w/v)solution?

A)1.80 g
B)12.0 g
C)15.0 g
D)0.800 g
E)1.25 g

Question 38

How much NaOH is present in a 75.0 mL sample of a 5.00% (w/v)solution?

A)3.75 g
B)5.00 g
C)6.67 g
D)15.0 g
E)75.0 g

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 many g of NaOH is needed to make 350.mL of a 2.50% (w/v)solution?

A)8.75 g
B)6.25 g
C)35.0 g
D)21.9 g
E)100.g

Question 41

How many g 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 42

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 43

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 44

How many moles of solute are present in 5.00 L of 6.00 M HCl?

A)0.833 mol
B)1.20 mol
C)6.00 mol
D)5.00 mol
E)30.0 mol

Question 45

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 46

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 47

How many moles of HCl are present in 35.5 mL of a 0.200 M solution?

A)0.236 mol
B)0.178 mol
C)0.974 mol
D)0.00710 mol
E)0.195 mol

Question 48

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 49

What is the molarity of a solution prepared by dissolving 36.0 g of NaOH in enough water to make 1.50 L of solution?

A)0.600 M
B)0.0240 M
C)0.900 M
D)1.35 M
E)0.0428 M

Question 50

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 51

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 52

How many g 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 53

What is the molarity of a solution prepared by dissolving 10.0 g of acetone,C₃H₆O,in enough water to make 250.mL of solution?

A)0.172 M
B)0.689 M
C)0.250 M
D)0.0430 M
E)0.0160 M

Question 54

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 55

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 56

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 57

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 58

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 59

What is the molarity of a solution prepared by dissolving 1.25 mol AgNO₃ in enough water to make 2.00 × 10³ mL of solution?

A)1.25 M
B)2.50 M
C)0.625 M
D)0.00250 M
E)0.106 M

Question 60

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 61

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 62

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 63

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 64

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 65

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 66

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 67

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 68

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 69

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 70

Which substance is not an electrolyte?

A)NaCl
B)HCl
C)NH₄NO₃
D)KOH
E)CH₄

Question 71

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 72

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

A)KNO₃
B)CH₃OH
C)CCl₄
D)NH₃

Question 73

How many grams are contained in one equivalent of iron (III)ion,Fe³⁺?

A)167.6 g
B)55.85 g
C)18.62 g
D)0.0537 g
E)6.02 × 10²³ g

Question 74

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 75

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 76

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 77

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 78

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 79

How many g of CaCl₂ are needed to prepare 500.mL of a 0.375 M solution?

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

Question 80

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