Deck 5: Chemical Reactions

Question 1

Which statement about the reaction below is true, given large amounts of reactants?

A) Ba(NO₃)₂ is insoluble in water and will precipitate.
B) K₂CO₃ is insoluble in water and will precipitate.
C) BaCO₃ is insoluble in water and will precipitate.
D) Both BaCO₃ and KNO₃ are insoluble in water and will precipitate.
E) All compounds in the reaction are soluble in water and no reaction occurs.

Answer 1

BaCO₃ is insoluble in water and will precipitate.

Question 2

All of the following are strong electrolytes except:

A) CH₃COOH.
B) H₂SO₄.
C) HNO_3.
D) HBr.
E) NaOH.

Answer 2

CH₃COOH.

Question 3

Which compound will dissolve in water in large amounts?

A) AgCl
B) Al(OH)₃
C) Na₂SO₄
D) BaSO₄
E) MgS

Answer 3

Na₂SO₄

Question 4

Which statement about bases is true?

A) Bases increase the hydroxide ion concentration of water when dissolved in it.
B) Bases increase the hydronium ion concentration of water when dissolved in it.
C) Bases turn phenolphthlalein colorless.
D) Bases react with limestone to produce gas bubbles.
E) Bases react with many metals to produce a flammable gas.

Question 5

Which of the following is a nonelectrolyte?

A) Mg(OH)₂
B) NaCl
C) KI
D) HBr
E) C₆H₁₂O₆

Question 6

Which of the following is a reducing agent?

A) I₂
B) Na
C) O₂
D) F₂
E) Br₂

Question 7

Which statement about the reaction below is true, given large amounts of reactants?

A) NaNO₃ is insoluble in water and will precipitate.
B) AgCl is insoluble in water and will precipitate.
C) Both NaNO₃ and AgCl are insoluble in water and will precipitate.
D) AgNO₃ is insoluble in water and no reaction will occur.
E) All compounds in the reaction are soluble in water and no reaction occurs.

Question 8

What is the reducing agent in the reaction below?

A) Zn
B) Cu²⁺
C) CuSO₄
D) Zn²⁺
E) SO₄^2-

Question 9

What is the correct formula for the hydroxide ion?

A) H₃O⁺
B) OH^-
C) NH₄⁺
D) H⁺
E) H^-

Question 10

What is the net ionic equation for the reaction of AlCl₃ and NaOH?

A) Na⁺ + Cl^- NaCl
B) Al⁺ + OH^- AlOH
C) Al³⁺ + 3OH^- Al(OH)₃
D) Al³⁺ + OH^3- AlOH
E) Na³⁺ + 3Cl^- NaCl₃

Question 11

Which of the following best describes an acid?

A) Acids react with many metals to produce a flammable gas.
B) Acids react with many metals to produce precipitates.
C) Acids increase the hydrogen ion concentration of water when dissolved in it.
D) Both a and c.
E) All of these.

Question 12

Which one or two substances are reduced in the reaction below?

A) Al
B) Al and Cl₂
C) Al and AlCl₃
D) Cl₂ and AlCl₃
E) Cl₂

Question 13

Which statement about strong acids is true?

A) Strong acids are weak electrolytes.
B) Strong acids are very concentrated.
C) Strong acids are mostly converted to ions when dissolved in water.
D) Citric acid is a strong acid.
E) Strong acids react only with strong bases.

Question 14

Which statement about neutralization reactions is true?

A) A weak acid cannot neutralize a strong base.
B) The net ionic equation for a neutralization reaction shows the formation of hydrogen gas
C) The net ionic equation for a neutralization reaction shows the formation of soluble salts.
D) The net ionic equation for a neutralization reaction shows the formation of water.
E) Organic acids neutralize bases by forming hydrogen gas.

Question 15

Which statement about the reaction below is true, given large amounts of reactants?

A) SrSO₄ is soluble in water and will not precipitate.
B) NaCl is a spectator ion and will not precipitate.
C) SO₄^2- is a spectator ion and will not precipitate.
D) Na⁺ is a spectator ion and will not precipitate.
E) All compounds in the reaction are soluble in water and no reaction occurs.

Question 16

What is the net ionic equation for the reaction of Ca(NO₃)₂ and Na₂SO₄?

A) 2Ca⁺ + SO₄^2- Ca₂SO₄
B) Na⁺ + NO₃^- NaNO₃
C) Ca²⁺ + SO₄^2- CaSO₄
D) Na²⁺ + 2NO₃^- Na(NO₃)₂
E) Ca⁺ + SO₄^- CaSO₄

Question 17

What is the correct formula for the hydronium ion?

A) OH^-
B) H₃O⁺
C) H⁺
D) H^-
E) NH₄⁺

Question 18

Which compounds will not dissolve in water in large amounts at 20 ^$\circ$ C?

A) I & II
B) I & IV
C) II & III
D) III & IV

Question 19

Which of the following factors cause exchange reactions to occur?

A) formation of a gas, precipitate or water
B) formation of a gas or a precipitate
C) formation of a gas only
D) formation of a precipitate only
E) formation of water only

Question 20

Which compound will not dissolve in water in large amounts?

A) KNO₃
B) NH₄Cl
C) Ca(OH)₂
D) AgCl
E) Ag₂SO₄

Question 21

What is the oxidation number of O in H₂O₂?

A) -2
B) -1
C) 0
D) +1
E) +2

Question 22

What is reduced in the reaction below?

A) CH₄
B) CO₂
C) O₂
D) H₂O
E) O₂ and CO₂

Question 23

What is the oxidation number of O in Fe₂O₃?

A) +2
B) -2
C) -3
D) -5
E) +5

Question 24

Determine the volume of solution that contains 15.0 g of AgNO₃ if the solution is 0.375 M.

A) 31.5 mL
B) 33.1 mL
C) 235 mL
D) 247 mL
E) 956 mL

Question 25

How many moles of NaOH are present in 25.0 mL of a 0.1000 M NaOH solution?

A) 100 mol
B) 2.50 × 10^-3 mol
C) 0.100 mol
D) 2.50 mol
E) 25.0 mol

Question 26

A 50.0 mL sample of 0.108 M H₂SO₄ is diluted to 250.0 mL. What is its new molarity?

A) 0.0216 M
B) 0.108 M
C) 0.184 M
D) 0.461 M
E) 0.542 M

Question 27

Which reaction will not occur?

A) Al(s) + SnCl₂(aq) AlCl₃(aq) + Sn(s)
B) H₂(g) + AgNO₃(aq) HNO₃(aq) + Ag(s)
C) Mg(s) + CuSO₄(aq) Cu(s) + MgSO₄(aq)
D) Mg(s) + CaSO₄(aq) MgSO₄(aq) + Ca(s)
E) Ba(s) + HCl(aq) BaCl₂(aq) + H₂(g)

Question 28

Which element is most reactive?

A) Cu
B) Fe
C) K
D) Mg
E) Pb

Question 29

Which of the following represents oxidation?

A) 2 H⁺ + 2 e^- H₂
B) F₂ + 2 e^- 2 F^-
C) Mg²⁺ + 2 e^- Mg
D) Na Na⁺ + e^-
E) Ni²⁺ + 2 e^- Ni

Question 30

What is the oxidation number of N in NO?

A) -2
B) -1
C) 0
D) +1
E) +2

Question 31

Which substance is reduced in the reaction below?

A) CO
B) S
C) Na₂S
D) Na₂SO₄
E) none of these

Question 32

Which of the following represents reduction?

A) Al Al³⁺ + 3 e^-
B) O₂ + 4 e^- 2 O^2-
C) Fe Fe²⁺ + 2 e^-
D) Na Na⁺ + e^-
E) H₂ 2 H⁺ + 2 e^-

Question 33

What is the molarity of a solution that results when 21.3 g of (NH₄)₃PO₄ is dissolved in water and diluted to exactly 250.0 mL?

A) 1.61 × 10^-4 M
B) 0.357 M
C) 0.572 M
D) 2.28 M
E) 85.2 M

Question 34

What is oxidized in the reaction below?

A) CO
B) CO₂
C) I₂
D) I₂O₅
E) CO and CO₂

Question 35

What is the oxidation number of P in PO₄^3-?

A) +5
B) +3
C) -2
D) -3
E) -5

Question 36

If a 45.0 mL sample of 2.20 M Na₂SO₄ is diluted to yield a final solution that is 0.110 M in sodium ions, what is the volume of the final solution?

A) 110 mL
B) 450 mL
C) 900 mL
D) 1800 mL
E) 4500 mL

Question 37

What is the oxidation number of N in NH₄⁺?

A) -3
B) -1
C) 0
D) +1
E) +3

Question 38

Which substance is oxidized in the reaction below?

A) Na⁺
B) PbO
C) NaNO₃
D) NaNO₂
E) none of these

Question 39

Determine the ammonium ion concentration of a solution that results when 4.53 g of (NH₄)₂SO₄ is dissolved in water and diluted to exactly 100.0 mL.

A) 0.343 M
B) 0.686 M
C) 1.03 M
D) 1.37 M
E) 2.51 M

Question 40

Which element is least reactive?

A) Al
B) Cu
C) Zn
D) Pb
E) Fe

Question 41

Oxalic acid, H₂C₂O₄, reacts with Y(NO₃)₃ as shown by the equation below. What weight of yttrium oxalate is produced from 50.0 mL of 0.265 M Y(NO₃)₃ and excess oxalic acid? Assume that all of the yttrium oxalate is insoluble.

A) 1.46 g
B) 1.82 g
C) 2.93 g
D) 3.64 g
E) 5.85 g

Question 42

Give an example of a strong base.

Question 43

When an element is _____________, it loses electrons.

Question 44

How many grams of PbI₂ will precipitate from the reaction of 14.0 mL of 0.190 M Pb(NO₃)₂ with excess KI solution? Assume that all of the PbI₂ is insoluble.

A) 1.23 g
B) 1.33 g
C) 2.66 g
D) 3.69 g
E) 6260 g

Question 45

Which of the methods described below will yield 500 mL of a 0.100 M KMnO₄ solution?

A) Add exactly 500 mL of water to 7.90 g of KMnO₄.
B) Add exactly 500 mL of water to KMnO₄.
C) Dissolve 7.90 g of KMnO₄ in water and dilute to exactly 500 mL.
D) Dissolve 15.8 g KMnO₄ in water and dilute to exactly 500 mL.
E) Dilute 220 mL of 1.00 M KMnO₄ to exactly 500 mL.

Question 46

Determine the mass of BaSO₄ that is produced by the reaction of 45.0 mL of 0.155 M H₂SO₄ and 60.0 mL of 0.125 M BaCl₂. Assume that BaSO₄ is totally insoluble.

A) 1.45 g
B) 1.62 g
C) 1.79 g
D) 3.24 g
E) 0.775 g

Question 47

A 25.00 mL sample of HCl solution is neutralized by exactly 41.63 mL of 0.1363 M NaOH. What is the molarity of the HCl solution?

A) 0.2270 M
B) 0.2726 M
C) 0.06815 M
D) 0.1135 M
E) 0.05675 M

Question 48

A 64.05 mL sample of 0.250 M CH₃COOH is to be exactly neutralized with 0.500 M KOH. How many milliliters of KOH will be required?

A) 64.1 mL
B) 32.0 mL
C) 128 mL
D) 16.0 mL
E) 8.01 mL

Question 49

Molarity is a unit of solution concentration expressed in moles per _____________.

Question 50

A 25.00 mL sample of H₃PO₄ solution is neutralized by exactly 54.93 mL of 0.04345 M Ca(OH)₂. What is the molarity of the H₃PO₄ solution?

A) 0.0636 M
B) 0.09546 M
C) 0.1432 M
D) 0.2148 M
E) 0.2897 M

Question 51

A 65.00 mL sample of HNO₃ solution is neutralized by exactly 34.16 mL of 0.5841 M Ba(OH)₂. What is the molarity of the HNO₃ solution?

A) 0.1535 M
B) 0.2880 M
C) 0.3110 M
D) 0.6139 M
E) 2.594 M

Question 52

How many moles of ions are in 285 mL of 0.0150 M MgCl₂?

A) 4.128 × 10^-3 mol
B) 5.26 × 10^-2 mol
C) 1.28 × 10^-2 mol
D) 1.05 × 10^-1 mol
E) 5.26 × 10^-1 mol

Question 53

Ammonia and sulfuric acid react according to the equation given below. How many milliliters of 0.110 M sulfuric acid are required to exactly neutralize 25.0 mL of 0.0840 M NH₃ solution?

A) 1.46 mL
B) 1.82 mL
C) 3.64 mL
D) 5.85 mL
E) 9.55 mL

Question 54

Hydrochloric acid solutions are often standardized by the reaction below. How many grams of CaCO₃ are required to exactly react with 50.0 mL of 0.155 M HCl?

A) 0.194 g
B) 0.283 g
C) 0.341 g
D) 0.387 g
E) 0.566 g

Question 55

A solution is prepared by dissolving 20.0 g of NaI in enough water to make 300.0 mL of solution. How many moles of ions are in 25.0 mL of this solution?

A) 0.0111 mol
B) 0.0222 mol
C) 0.0445 mol
D) 0.111 mol
E) 0.445 mol

Question 56

How many grams of KCl are in 125.0 mL of 0.375 M KCl?

A) 3.49 g
B) 0.0469 g
C) 3.49 × 10^-3 g
D) 46.9 g
E) 0.938 g

Question 57

A 25.00 mL sample of HCl solution is neutralized by exactly 31.22 mL of 0.08152 M Ca(OH)₂. What is the molarity of the HCl solution?

A) 0.08152 M
B) 0.1018 M
C) 0.2036 M
D) 0.1021 M
E) 0.09453 M

Question 58

A solution is made by dissolving 60.0 g of AlCl₃ in enough water to make 250.0 mL of solution. How many moles of ions are in 5.00 mL of solution?

A) 3.60 × 10^-2 mol
B) 1.01 × 10^-3 mol
C) 1.25 × 10^-3 mol
D) 5.00 × 10^-3 mol
E) 9.00 × 10^-3 mol

Question 59

A neutralization reaction involves the reaction of a(n) _____________ with a(n) _____________.

Question 60

How many moles of ions are in a 250.0 mL sample of 0.150 M NaCl?

Question 61

Write the net ionic equation for the reaction given.

Question 63

A 25.0 mL solution of HNO₃ is reacted with 0.1125 M NaOH. The endpoint is reached when 57.8 mL of NaOH has been added. What is the molarity of HNO₃?

Question 64

A solution is made by dissolving 15.0 g of CaCl₂ in enough water to make exactly 500.0 mL of solution. What is the molarity of the solution?

Question 65

A chemical reaction for which spectator ions are deleted is called a(n) _____________ ionic equation.

Question 66

Match the following:

Question 67

Which substance is an oxidizing agent in the reaction below?