Deck 4: Reactions in Aqueous Solution

Question 1

The relationship between volume and concentration of stock and dilute solutions is $\frac { V _ { s } } { M _ { s } } = \frac { V _ { a } } { M _ { d } }$ .

Answer 1

False

Question 2

When electricity, in the form of an electrical potential, is applied to a solution, ions in solution migrate toward a similarly charged rod or plate to complete an electrical circuit.

Answer 2

False

Question 3

Given: 2C₆H₅COOH + Na₂CO₃ $\rightarrow$ 2C₆H₅COONa + H₂O + CO₂
In the above reaction, the volume of 0.3250 M Na₂CO₃ needed for the complete reaction of 54.0 g C₆H₅COOH is17.6 L.

Answer 3

False

Question 4

What volume of a 2.00 M sucrose stock solution is necessary to prepare 2,750 mL of a sucrose solution with molarity 5.34 M?

A) 3.01 L
B) 2.10 L
C) 2.00 L
D) 7.34 L
E) 0.750 L

Question 5

Write a short note on parts per million and parts per billion that are used as units to represent concentrations of solutions.
The concentrations of very dilute solutions are often expressed in parts per million (ppm), which is grams of solute per 10⁶ g of solution, or in parts per billion (ppb), which is grams of solute per 10⁹ g of solution. For aqueous solutions at 20°C, 1 ppm corresponds to 1 μg per milliliter, and 1 ppb corresponds to 1 ng per milliliter.

Question 6

Which of the following is a nonelectrolyte?

A) Acetic acid
B) Methyl ketone
C) Formic acid
D) Sodium chloride
E) Ammonia

Question 7

Which of the following are the two classes of organic compounds that act as nonelectrolytes?

A) Carboxylic acids and esters
B) Alkanes and carboxylic acids
C) Ketones and aldehydes
D) Alkenes and esters
E) Carboxylic acids and ethers

Question 8

A(n) _____ is a commercially prepared solution of known concentration.

Question 9

What is the concentration of OH ^- in 0.0345 M Ba(OH)₂?

A) 0.0251 M
B) 0.0543 M
C) 0.0345 M
D) 0.0960 M
E) 0.0690 M

Question 10

Calcium sulfate is a nonelectrolyte.

Question 11

What is the concentration of Ca²⁺ in 0.0152 M Ca₃(NO₃)₂?

A) 0.0152 M
B) 0.0304 M
C) 0.0456 M
D) 0.456 M
E) 0.304 M

Question 12

Differentiate between strong electrolytes and weak electrolytes.

Question 13

Which of the following is an example of a compound that is very soluble in water but that is essentially nonconductive?

A) Sucrose
B) Calcium chloride
C) Barium hydroxide
D) Sulfuric acid
E) Sodium bromide

Question 14

Why is water described as a polar substance?

Question 15

_____ are compounds that dissolve in water and have essentially no effect on conductivity.

Question 16

Which of the following is a strong electrolyte?

A) 2-propanol
B) Formaldehyde
C) Ferrous sulfate
D) Ethanol
E) Acetone

Question 17

In chemistry, the _____ of a solution describes the quantity of a solute that is contained in a particular quantity of solvent or solution.

Question 18

Polar liquids are good solvents for ionic compounds.

Question 19

What is an electrolyte?

A) It is the term used to describe acids that do not dissolve in water.
B) It is the term used to describe bases that do not dissolve in water.
C) It is any compound that can form carbon dioxide when it reacts with water.
D) It is any compound that can form ions when it dissolves in water.
E) It is any compound that can act as a solvent for water.

Question 20

Individual cations and anions that are each surrounded by their own shell of water molecules are called _____.

Question 21

Given: CH₃COOH + NaOH $\rightarrow$ CH₃COO⁻Na⁺ + H₂O
If 663 mL of 0.150 M CH₃COOH is mixed with 444 mL of 0.326 M NaOH, the limiting agent in the reaction is ____.

Question 22

The _____ in the balanced chemical equation tell how many moles of reactants are needed and how many moles of products can be produced.

Question 23

Given complete ionic equation: 2Ag⁺(aq) + 2NO₃⁻(aq) + 2K⁺(aq) + Cr₂O₇²⁻(aq) $\rightarrow$ Ag₂Cr₂O₇(s) + 2K⁺(aq) + 2NO₃⁻(aq) Convert the given equation into an overall chemical equation.

A) 2AgNO₃ (aq) + K₂Cr₂O₇ (aq) $\rightarrow$ Ag₂Cr₂O₇(s) + 2KNO₃(aq)
B) Ag₂Cr₂O₇(s) + K₂Cr₂O₇ (aq) $\rightarrow$ 2AgNO₃ (aq) + 2KNO₃(aq)
C) 2AgNO₃ (aq) + 2KNO₃(aq) $\rightarrow$ Ag₂Cr₂O₇(s) + K₂Cr₂O₇(aq)
D) 2Ag⁺(aq) + 2NO₃⁻(aq) + 2K⁺(aq) + Cr₂O₇²⁻(aq) $\rightarrow$ 2K⁺(aq) + 2NO₃⁻(aq)
E) 2Ag⁺(aq) + Cr₂O₇²⁻(aq) $\rightarrow$ Ag₂Cr₂O₇(s)

Question 24

The full molecular chemical equation shows all the substances present in the form in which they actually exist in the solution.

Question 25

Differentiate between an overall chemical equation and a complete ionic equation.

Question 26

Given an outline of the steps involved in the calculation of moles from volume for a given equation.

Question 27

Given complete ionic equation: 3Ag⁺(aq) + 3F⁻(aq) + 3Na⁺(aq) + PO₄³⁻(aq) → Ag₃PO₄(s) + 3Na⁺(aq) + 3F⁻(aq) In the above complete ionic equation, the spectator ions are:

A) 3Ag⁺(aq) and 3F⁻(aq).
B) 3Na⁺(aq) and 3Ag⁺(aq).
C) 3F⁻(aq) and 3Na⁺(aq).
D) 3Ag⁺(aq) and (PO₄)³⁻(aq).
E) (PO₄)³⁻(aq) and 3F⁻(aq).

Question 28

When table salt is added to an aqueous solution of silver nitrate, the exchange reaction yields a precipitate of silver chloride.

Question 29

Given: 2C₆H₅COOH + Na₂CO₃ $\rightarrow$ 2C₆H₅COONa + H₂O + CO₂ What mass of CO₂ is formed when 275 mL of 0.150 M Na₂CO₃ is mixed with 775 mL of 0.254 M C₆H₅COOH?

A) 2.54 g
B) 3.63 g
C) 1.82 g
D) 6.36 g
E) 4.52 g

Question 30

Which of the following is the net ionic equation for the reaction between the aqueous solutions of magnesium sulfate and sodium carbonate?

A) MgSO₄(aq) + Na₂CO₃(aq) → MgCO₃(s) + Na₂SO₄(s)
B) MgSO₄(aq) + Na₂CO₃(aq) → MgCO₃(s) + Na⁺(aq) + SO₄^2-(aq)
C) Na⁺(aq) + SO₄^2-(aq) → Na₂SO₄(s)
D) Mg²⁺(aq) + CO₃^2-(aq)→ MgCO₃(s)
E) Mg²⁺(aq) + SO₄^2-(aq) + Na⁺(aq) + CO₃^2-(aq) → MgCO₃(s) + Na⁺(aq) + SO₄^2- (aq)

Question 31

The ions that do not participate in the actual reaction are called _____.

Question 32

Given: If 885 mL of 0.250 M pentanoic acid(molar mass = 102 g/mol) is mixed with 885 mL of 0.524 M cyclopentanol(molar mass = 86.1 g/mol), the 0.524 M cyclopentanol acts as the limiting agent.

Question 33

Calcium hydroxide is insoluble in water.

Question 34

_____ is a chemical equation that shows which ions and molecules are hydrated and which are present in other forms and phases.

Question 35

Given: HCOOH+ KOH $\rightarrow$ HCOO⁻K⁺ + H₂O What volume of 0.105 M KOH must be added to 125 mL of a solution containing 6.20 × 10⁻⁵ g of HCOOH to ensure that formation of the HCOO⁻K⁺ is complete?

A) 18.3 $\mu$ L
B) 6.28 $\mu$ L
C) 125 $\mu$ L
D) 12.8 $\mu$ L
E) 10.5 $\mu$ L

Question 36

In the equation given below, cyclopentanol (molar mass = 86.1 g/mol) reacts with pentanoic acid (molar mass = 102 g/mol) to produce cyclopentanoate(molar mass = 170.2 g/mol) and water. The volume of 0.297 M pentanoic acid needed for the complete reaction of 40.0 g cyclopentanol is _____ mL.

A) 0.86 × 10³
B) 5.78 × 10³
C) 7.58 × 10³
D) 1.56 × 10³
E) 0.76 × 10³

Question 37

The net ionic equation shows only those species that participate in the chemical reaction.

Question 38

Given: CH₃CH₂COOH + H₂O $\rightarrow$ CH₃CH₂COO⁻ + H₃O⁺ What volume of 0.500 M CH₃CH₂COOH is reacting with water to form 2.86 g of CH₃CH₂COO⁻?

A) 0.487 L
B) 0.0118 L
C) 0.0487 L
D) 0.0784 L
E) 0.784 L

Question 39

In the reaction of barium chloride with sodium sulfate, SO₄^2- acts as a spectator ion.

Question 40

Given: HCOOH + KOH $\rightarrow$ HCOO⁻K⁺ + H₂O What mass of HCOO⁻K⁺ is formed when 383 mL of 0.250 M HCOOH is mixed with 885 mL of 0.524 M KOH?

A) 885 g
B) 48.5 g
C) 8.05 g
D) 1.06 g
E) 32.0 g

Question 41

The precipitate formed when an aqueous solution of lithium bromide is reacted with an aqueous solution of silver nitrate is _____.

A) LiBr
B) AgBr
C) LiNO₃
D) AgNO₃
E) LiAg

Question 42

The insoluble product that forms in a precipitation reaction is called a(n) _____.

Question 43

HCl is the conjugate acid of the chloride ion.

Question 44

Why are precipitation reactions called double displacement reactions?

Question 45

_____ is a monoprotic acid.

A) Sulfuric acid
B) Phosphoric acid
C) Citric acid
D) Benzoic acid
E) Carbonic acid

Question 46

What is the pH of a 3.0 × 10⁻⁵ M aqueous solution of H₂SO₄?

A) 4.2
B) 2.4
C) 3.0
D) 0.3
E) -0.3

Question 47

According to the Arrhenius definition of acids and bases, an acid is a substance:

A) that dissolves in water to produce OH^- ions.
B) that accept a proton.
C) that dissolves in water to produce H⁺ ions.
D) produced by the reaction of two bases.
E) that has a greater OH^- ion concentration than H⁺ ion.

Question 48

Which of the following is an example of a neutralization reaction?

A) MgCl₂+2NaNO₃ $\rightarrow$ Mg(NO₃)₂+2NaCl
B) HI(aq) + KOH(aq) $\rightarrow$ I(s) + H₂O(l)
C) 2C₆H₆COOH + Na₂CO₃(aq) $\rightarrow$ 2C₆H₆COO⁻Na⁺(aq) + H₂O + CO₂(g)
D) 2Na⁺ + S^2- → Na₂S(s)
E) BaCl₂(aq) + Na₂SO₄(aq) → BaSO₄(s) + 2Na⁺(aq) + 2Cl^-(aq)

Question 49

The net ionic equation for the reaction that occurs when an aqueous solution of lead nitrate is mixed with a solution containing potassium iodide is:

A) K⁺(aq) + NO₃^-(aq) → KNO₃(s).
B) Pb(NO₃)₂(aq) + 2KI(aq) → PbI₂(s) + 2KNO₃(s).
C) Pb²⁺(aq) + NO₃^-(aq) + K⁺(aq) + 2I^-(aq) → KNO₃(s) + PbI₂(s).
D) Pb²⁺(aq) + 2I^-(aq) → PbI₂(s).
E) K⁺(aq) + I^- (aq) → KI(s).

Question 50

_____ is the crystalline solid formed when an aqueous solution of barium chloride is reacted with an aqueous solution of sodium sulfate.

A) NaCl
B) BaCl₂
C) Na(OH)₂
D) NaSO₄
E) BaSO₄

Question 51

Which of the following is an example of a strong base?

A) Acetylacetone
B) Methylamine
C) Ammonia
D) Potassium hydroxide
E) Methylethyl ketone

Question 52

Define Arrhenius acids and bases.

Question 53

Explain with an example, how precipitation reactions can be used to recover precious metals for recycling.
Student examples may vary.
Precipitation reactions can be used to recover silver from solutions that are used to develop conventional photographic films. Silver bromide turns black when exposed to light and this reaction is used by the photographers to capture images in shades of grey. The washing of unexposed silver bromide using sodium thiosulfate solution generates a dilute silver waste solution. Instant photo operations can generate more than a hundred gallons of dilute silver waste solution per day. The silver from these solutions can be recovered by first removing the thiosulfate by oxidation and then precipitating Ag⁺ ions with excess chloride ions.

Question 54

CH₃CO₂H is an example of a polyprotic acid.

Question 55

Which of the following reactions will not result in the formation of a precipitate?

A) Aqueous silver nitrate added to a solution containing potassium chloride
B) Aqueous solution of barium chloride added to a solution containing sodium sulfate
C) Aqueous solution of strontium chloride added to a solution containing potassium carbonate
D) Aqueous solution of sodium sulfate added to a solution containing ammonium iodide
E) Aqueous solution of rubidium hydroxide is added to a solution containing cobalt chloride

Question 56

The pH of a solution decreases with the increase in hydrogen ion concentration.

Question 57

Which of the following salts is insoluble in water?

A) (NH₄)₂SO₄
B) (NH₄)₃PO₄
C) LiCl
D) MgSO₄
E) Ba(OH)₂

Question 58

Which of the following is a strong acid?

A) HClO
B) HCN
C) HF
D) HNO₂
E) HClO₄

Question 59

The white precipitate formed when lead acetate is reacted with an aqueous solution of ammonium iodide is _____.

Question 60

Which of the following is a triprotic acid?

A) Benzoic acid
B) Phosphoric acid
C) Formic acid
D) Nitric acid
E) Acetic acid

Question 61

What are the biological effects of acid rain?

Question 62

The _____ ions are responsible for the increased acidity in rain and snow.

A) bromide
B) chloride
C) oxide
D) sulfate
E) phosphate

Question 63

Which of the following is an inert metal?

A) Lead
B) Nickel
C) Tin
D) Silver
E) Zinc

Question 64

A substance that can behave both as an acid and a base is called a(n) _____ substance.

Question 65

Consider the reaction: Cu(s) + 2 Ag⁺(aq) → Cu²⁺(aq) + 2 Ag(s).
In this reaction, silver is reduced from +1 to 0 oxidation state.

Question 66

The compound responsible for the brown color of smog is _____.

Question 67

Compounds containing elements in low oxidation states become reduced in chemical reactions.

Question 68

Based on the activity series, cobalt can reduce the salts of _____.

A) chromium
B) cadmium
C) calcium
D) copper
E) iron

Question 69

H₃O⁺ is called the _____ ion.

Question 70

Metal objects suffer damage from acid rain through oxidation-reduction reactions.

Question 71

Based on the activity series, there will be no reaction when:

A) lithium metal is dropped into aqueous silver nitrate.
B) a strip of zinc is placed in a solution containing lead iodide.
C) a strip of chromium is placed in a solution containing magnesium sulfate.
D) an iron rod is dipped into a solution of copper sulfate.
E) a chunk of silver is dropped into a solution containing mercuric chloride.

Question 72

Differentiate between strong acids and weak acids.

Question 73

The balanced chemical equation for the reaction when molten iron reacts with water to form ferrous ions and hydrogen gas is:

A) 2Fe(l) + 2H₂O(l) → Fe²⁺(aq) + 3OH^-(aq) + 2H₂(g)
B) Fe(l) + 2H₂O(l) → Fe²⁺(aq) + H₂(g)
C) 2Fe(l) + H₂O(l) → Fe²⁺(aq) + 2H₂(g)
D) Fe(l) + 2H₂O(l) → Fe²⁺(aq) + 2OH^- (aq) + 2H₂(g)
E) Fe(l) + 2H₂O(l) → Fe²⁺(aq) + 2OH^- (aq) + H₂(g)

Question 74

Lead has a greater tendency to be oxidized than chromium.

Question 75

Which of the following elements has the greatest tendency to lose electrons?

A) Magnesium
B) Copper
C) Potassium
D) Manganese
E) Cadmium

Question 76

The _____ is a precipitation that is dramatically more acidic because of human activities and has significant consequences for all the living organisms.

Question 77

Acid rain results in the increase of _____ ions in groundwater, which when present in high concentrations, is toxic to plants and affects plant growth.

A) OH^-
B) Al³⁺
C) SO₄^2-
D) NO₃⁻
E) CO₃^2-

Question 78

The scrubbers in coal-burning power plants use _____ to trap SO₂.

A) NO₂
B) ZnO
C) CaCO₃
D) CaSO₄
E) CaO

Question 79

Which of the following reactions shows the formation of a compound that is responsible for the damage of marble buildings and sculptures by acid rain?

A) H₂SO₃(aq) + Ca(OH)₂(s) → CaSO₃.2H₂O(s)
B) CaO(s) + H₂O(l) → Ca(OH)₂(s)
C) CaCO₃(s) + H₂SO₄(aq) → CaSO₄(s) + H₂O(l) + CO₂(g)
D) 2N₂(g) + 5O₂(g) + 2H₂O(l) → 4HNO₃(aq)
E) 2H₂SO₃(aq) + O₂(g) → 2H₂SO₄(aq)

Question 80

Acid rain results in the increase in pH of natural waters.