Deck 6: Aqueous Solutions: Part I

Question 1

How did Marie Curie approach her cooking?

A)Through random guess work
B)By changing variables one by one
C)By getting advice from older cooks
D)Marie Curie didn't cook.

Answer 1

B

Question 2

What ingredients do muffins contain that brownies do not?

A)Butter
B)Flour
C)Eggs and milk
D)Buttermilk and baking soda

Answer 2

D

Question 3

What is the more scientific name for baking soda?

A)Sodium chloride
B)Sodium carbonate
C)Sodium bicarbonate
D)Baking bicarbonate

Answer 3

C

Question 4

What is the chemical difference between buttermilk and milk?

A)Buttermilk contains less fat.
B)Buttermilk contains more fat.
C)Buttermilk has been mixed with butter.
D)None of the above.

Question 5

If the major difference between a brownie recipe and a muffin recipe is buttermilk and baking soda, what must these two do to the muffin mixture?

A)Prevent it from rising.
B)Make it dense.
C)Make it lighter and airier.
D)Cause it to be chewier.

Question 6

What is the common solvent in all aqueous solutions?

A)oil
B)water
C)alcohol
D)None of the above.

Question 7

In a mixture of two materials in aqueous phase, the one that is present in the largest amount is called _____________.

A)the solvated ion
B)the solute
C)the solution
D)the solvent

Question 8

How can the alcohol be defined in an alcoholic beverage with 10% alcohol content by volume?

A)as a solvent
B)as a solute
C)as a solution
D)as a fluid

Question 9

Blood plasma is considered what component of a solution?

A)the solvent
B)the protein
C)the solute
D)the lipid

Question 10

How are molecules described when they contain both a positive and negative end?

A)planar
B)apolar
C)nonpolar
D)polar

Question 11

What causes an ionic compound to dissolve in water?

A)the ionic nature of the solute
B)the nonpolar nature of water
C)the polar nature of water
D)the ionic nature of the solvent

Question 12

How does water overcome the attractive forces holding a solute particle in a solid?

A)by surrounding the solute particles
B)by isolating the solvent particles
C)by interspersing with the solvent molecules
D)by surrounding the solvent particles

Question 13

Molecular compounds form ions when they dissolve in water.

Question 14

What does the expression "like dissolves like" mean?

A)In general, polar compounds will dissolve in a polar solvent.
B)In general, polar solutes will not dissolve in a polar solvent.
C)In general, nonpolar compounds will dissolve in a polar solvent.
D)In general, polar compounds will dissolve in a nonpolar solvent like water.

Question 15

Why is a molecular compound like ethylene glycol soluble in water?

A)Both are nonpolar molecules.
B)Both are polar molecules.
C)Both are small molecules.
D)Both are liquid-state molecules.

Question 16

In general, when an aqueous solution is heated, what happens to the solubility of ionic compounds within it?

A)Solubility decreases.
B)Solubility increases.
C)Kinetic energy is added by the solute.
D)Kinetic energy is removed by the solute.

Question 17

What affects the rate at which solutes dissolve?

A)temperature of the solution
B)surface area of the solute
C)concentration of the solute
D)All of the above.

Question 18

Why does powdered sugar dissolve in water more rapidly than a sugar cube?

A)greater surface area of the powder
B)more kinetic energy in the powdered sample
C)greater concentration in the sugar cube
D)greater density of the sugar cube

Question 19

What is an electrolyte?

A)a compound that dissolves in water
B)a compound that dissociates into ions in water
C)a compound that dissociates into molecules in water
D)an ionic compound that doesn't dissolve in water

Question 20

When electrodes are placed in a solution of electrolytes, how does the current flow?

A)Positively charged cations are attracted to the negatively charged cathode.
B)Negatively charged cations are attracted to the negatively charged anode.
C)Positively charge anions are attracted to the negatively charged cathode.
D)Negatively charged cations are attracted to the positively charged cathode.

Question 21

What is a weak electrolyte?

A)a compound that completely forms ions in solution
B)a compound that only partially forms molecules in solution
C)a compound that completely forms molecules in solution
D)a compound that only partially forms ions in solution

Question 22

Which compounds could be electrolytes?

A)SO₃
B)NO₂
C)CH₄
D)MgCl₂

Question 23

Of the following, which could be electrolytes?

A)PCl₃
B)CaCl₂
C)Both of the above.
D)None of the above.

Question 24

Which of these are electrolytes?

A)ICl
B)CO₂
C)NaCl
D)CO

Question 25

Which of the following are electrolytes: SO₃, MgBr₂, and CO₂?

A)SO₂ and MgBr₂
B)SO₂ and CO₂
C)only SO₂
D)only MgBr₂

Question 26

Which of the following are not electrolytes?

A)NaI
B)CaCl₂
C)KBr
D)NO₂

Question 27

Of the group, SO₂, SO₃, and CO, which are non-electrolytes?

A)SO₂ and SO₃ are non-electrolytes.
B)SO₂ and CO are non-electrolytes.
C)All are non-electrolytes.
D)All are electrolytes.

Question 28

What is a compound that does not dissociate into ions in aqueous solution?

A)a crystalline compound
B)a salt
C)an electrolyte
D)a non-electrolyte

Question 29

LiI is not an electrolyte.

Question 30

Which of the following is an electrolyte?

A)Li₂SO₄
B)SO₃
C)CO
D)H₂O

Question 31

Assuming the cations and anions switch in the reaction with reactants AgNO₃ + NaI →, the solid product will be NaNO₃.

Question 32

What is the solid product when the following two reactants are mixed in aqueous solution, AgNO₃ + KBr →?

A)AgBr
B)AgNO₃
C)KNO₃
D)None of the above.

Question 33

When the following two salts-AgC₂H₃O₂ + NaNO₃ →-are mixed in aqueous solution, what is the solid product?

A)AgNO₃
B)NaC₂H₃O₂
C)NaNO₃
D)There is no solid product.

Question 34

When lead(II) nitrate is mixed with sodium chloride in aqueous solution, what is the solid product?

A)sodium nitrate
B)lead(II) chloride
C)lead chloride
D)None of the above.

Question 35

What is a saturated solution?

A)one that contains the maximum amount of solute that can be dissolved
B)one that contains the maximum amount of solvent that can be dissolved
C)one that contains the maximum amount of solution that can be dissolved
D)one that contains the maximum amount of a salt that can be dissolved

Question 36

What kind of salt is NaCN?

A)insoluble
B)soluble
C)sparingly soluble
D)an insoluble solid

Question 37

According to the solubility table, KBr should be _________.

A)soluble
B)insoluble
C)molecular
D)sparingly soluble

Question 38

According to the solubility table, CaCO₃ should be __________.

A)supersaturatable
B)soluble
C)insoluble
D)molecular

Question 39

What kind of compound is KOH?

A)insoluble in water
B)soluble in non-aqueous solution
C)soluble in water
D)a molecular solid

Question 40

What kind of compound is AgCl in water?

A)insoluble
B)soluble
C)dissolvable
D)not enough information to tell

Question 41

How should Na₂S behave in water?

A)It should be insoluble.
B)It should be a molecular solid.
C)It should be supersaturatable.
D)It should be soluble.

Question 42

Which cation can make an insoluble product with Cl^- in water?

A)Na⁺
B)Ag⁺
C)Ca²⁺
D)K⁺

Question 43

Which cation will make an insoluble precipitate with Br^- in water?

A)Li⁺
B)K⁺
C)Both of the above.
D)None of the above.

Question 44

How does the compound PbCl₂ behave in water?

A)It is soluble.
B)It is insoluble.
C)It is acidic.
D)It is basic.

Question 45

Silver acetate is insoluble in water.

Question 46

If the reaction AgNO₃ + NaCl → NaNO₃ + AgCl were written out as a total ionic reaction, which ions would be the spectator ions?

A)Ag⁺ and NO₃^-
B)Na⁺ and Ag⁺
C)Na⁺ and NO₃^-
D)Cl^- and NO₃^-

Question 47

What are spectator ions?

A)ions that are soluble in aqueous solution after a reaction has taken place
B)ions that are insoluble in solution after a reaction has taken place
C)ions that precipitate from solution when a reaction takes place
D)ions that escape from solution after a reaction takes place

Question 48

What type of compound is potassium iodide?

A)insoluble
B)soluble
C)a precipitate
D)a reactant

Question 49

A total ionic equation shows all the ions in an aqueous reaction that form a precipitate only, and no others.

Question 50

In the reaction of lead (II) nitrate and potassium bromide, what will be the net ionic equation?

A)NO₃^- + K⁺ → KNO₃
B)NO₃^- + 2 K⁺ → K₂NO₃
C)Pb²⁺ + 2 Br^- → PbBr₂
D)Pb⁺ + Br^- → PbBr

Question 51

What happens to a saturated salt solution in water when the solution is cooled?

A)A precipitate forms.
B)More salt can be added to the solution.
C)The solution contracts.
D)Nothing.

Question 52

What is the molarity of a solution made by diluting 100 mL of a 2.5 M solution to 200 mL?

A)200 M
B)2.5 M
C)5.0 M
D)1.25 M

Question 53

What is the molarity of a solution made from 54.9 g of NaCl in 0.75 L of water?

A)73.2 M
B)1.25 M
C)1.42 M
D)0.01 M

Question 54

What is the molarity of a solution made from 0.25 mol of KBr and 0.80 L of water?

A)0.31 M
B)3.20 M
C)0.20 M
D)1.05 M

Question 55

A solution made from 19.0 g of NaBr and 500 mL of water has what molarity?

A)38.0 M
B)0.37 M
C)0.038 M
D)481.0 M

Question 56

What is the molarity of a solution made from 65.0 g of Na₂SO₄ and 2.30 L of water?

A)6.50 M
B)1.05 M
C)0.46 M
D)0.20 M

Question 57

When a solution is made from 1.0 g of KI and 0.090 L of water, what is its molarity?

A)0.001 M
B)0.09 M
C)0.07 M
D)11.1 M

Question 58

If 300 mL of a solution with a 1.5 M is diluted to 750 mL, what is its new molarity?

A)0.60 M
B)0.34 M
C)6.67 M
D)0.30 M

Question 59

A solution, 200 mL, with a 2.3 M is diluted to 650 mL, what is its new molarity?

A)0.69 M
B)17.7 M
C)0.71 M
D)7.48 M

Question 60

If 250 mL of a solution with a 0.5 M is diluted to 850 mL, what is its new molarity?

A)0.50 M
B)0.43 M
C)0.15 M
D)6.25 M

Question 61

If 10 mL of a solution with a 2.5 M is diluted to 950 mL, what is its new molarity?

A)26.3 M
B)0.26 M
C)23.8 M
D)0.03 M

Question 62

What do all weak acids have in common?

A)They are weak electrolytes.
B)They are non-electrolytes.
C)They are strongly acidic.
D)They are strong electrolytes.

Question 63

Which of the following are strong acids?

A)HF, KOH, and HCl
B)HBr, HI, and HCl
C)HCl, HOH, and HI
D)HBr, HSe, and HI

Question 64

Which of the following is a strong acid?

A)HCHO, formic acid
B)H₂CO₃
C)acetic acid
D)None of these are strong acids.

Question 65

Why might a weak acid like HF still be able to dissolve glass?

A)Because it is concentrated.
B)Because it is really a strong acid.
C)Because it does not contain oxygen.
D)None of the above.

Question 66

What is the old, common name for NaOH?

A)base
B)fat
C)lye
D)acid

Question 67

When sodium hydroxide is combined with animal fat, what type of reaction occurs?

A)a neutralization
B)a saponification
C)a double displacement
D)a redox reaction

Question 68

What elements form bases when they react with water?

A)the coinage metals
B)the halogens
C)the transition metals
D)the alkali metals and alkaline earths

Question 69

NaOH is classified as what kind of compound?

A)weak base
B)strong acid
C)strong base
D)weak acid

Question 70

How is a base defined?

A)as a compound that produces hydroxide ions
B)as a compound that produces H⁺ ions
C)as a compound with a pH below 7
D)as a compound with pH = 7

Question 71

Of the following acids, which is/are strong?

A)HCl
B)HNO₃
C)Both of the above.
D)None of the above.

Question 72

In the reaction Cu + 2 HCl → CuCl₂ + H₂, what happened to the acid?

A)The Cu has been reduced.
B)The Cl^- has been oxidized.
C)The H⁺ has been reduced.
D)Nothing.

Question 73

In the reaction 2 HBr + Fe → H₂ + FeBr₂, what happened to the Br^-?

A)It was oxidized.
B)It was reduced.
C)It was zeroed.
D)Nothing.

Question 74

In the reaction 2 HCl + Zn → H₂ + ZnCl₂, what chemical change occurred with the zinc metal?

A)Nothing.
B)It neutralized.
C)It reduced.
D)It oxidized.

Question 75

According to the reaction Sn + 2 HI → SnI₂ + H₂, what happened to the I^-?

A)It oxidized.
B)No oxidation or reduction.
C)It reduced.
D)Not enough information to tell.

Question 76

What kind of reaction is the addition of KOH to HCl?

A)a reduction-oxidation that does not make a precipitate
B)a reduction-oxidation that makes a precipitate
C)a neutralization that makes a salt and water
D)an addition that makes salt and water

Question 77

What is lithium hydroxide?

A)LiOH, a strong base
B)LiOH, a weak base
C)Li(OH)₂, a strong base
D)Li(OH)₂, a weak base

Question 78

What is the formula for calcium hydroxide and how is it classified?

A)CaOH, a weak base
B)Ca(OH)₂, a weak base
C)CaOH, a strong base
D)Ca(OH)₂, a strong base

Question 79

A solution with a pH = 3.5 is said to be ___________.

A)acidic
B)basic
C)neutral
D)Can't tell from the information given.

Question 80

What is the pH of a solution with a [H⁺] = 1.0 × 10^-8?

A)4
B)8
C)12
D)Can't be determined.