Deck 7: Reactions in Aqueous Solutions

Question 1

Write and balance molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and phases of the products in each of the cases.

-An aqueous solution of calcium nitrate is mixed with an aqueous solution of sodium phosphate.

Answer 1

3Ca(NO₃)₂(aq) + 2Na₃PO₄(aq) $\rightarrow$ Ca₃(PO₄)₂(s) + 6NaNO₃(aq)

Question 2

An aqueous solution of sodium sulfate is allowed to react with an aqueous solution of calcium nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)?.

A) 2Na⁺(aq)
B) 2SO₄^2-(aq)
C) 3Ca²⁺(aq)
D) NO₃^-(aq)
E) K⁺(aq)

Answer 2

2Na⁺(aq)

Question 3

Write and balance molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and phases of the products in each of the cases.

-An aqueous solution of silver nitrate is mixed with an aqueous solution of potassium chromate.

Answer 3

2AgNO₃(aq) + K₂CrO₄(aq) $\rightarrow$ Ag₂CrO₄(s) + 2KNO₃(aq)

Question 4

A substance that, when dissolved in water, produces a solution that conducts electric current very efficiently is called

A) a strong electrolyte
B) a weak electrolyte
C) a strong ion
D) an electrical solute
E) none of these

Question 5

Write and balance molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and phases of the products in each of the cases.

-An aqueous solution of lead(II) nitrate is mixed with an aqueous solution of potassium chloride.

Question 6

Write and balance molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and phases of the products in each of the cases.

-An aqueous solution of lead(II) nitrate is mixed with an aqueous solution of sodium iodide.

Question 7

Write and balance molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and phases of the products in each of the cases.

-An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium sulfate.

Question 8

An aqueous solution of potassium sulfate is allowed to react with an aqueous solution of lead(II) nitrate. The net ionic equation contains which of the following species (when balanced in standard form)?.

A) Pb²⁺(aq)
B) 2SO₄^2-(aq)
C) 2K⁺(aq)
D) NO₃^-(aq)
E) 2NO₃^-(aq)

Question 9

Write the balanced molecular equation for the reaction between aqueous solutions of lithium phosphate and sodium hydroxide.

Question 10

When a precipitation reaction occurs, the ions that do not form the precipitate

A) evaporate
B) are cations only
C) form a second insoluble compound in the solution
D) are left dissolved in the solution
E) none of these

Question 11

Write and balance molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and phases of the products in each of the cases.

-An aqueous solution of copper(II) nitrate is mixed with an aqueous solution of sodium hydroxide.

Question 12

An aqueous solution of potassium sulfate is allowed to react with an aqueous solution of barium nitrate. What is the coefficient of the solid in the balanced equation (in standard form)?

A) 1
B) 2
C) 3
D) 4
E) 6

Question 13

Which drawing best represents the mixing of aqueous calcium chloride with aqueous potassium sulfate when they are mixed in stoichiometric amounts (neither reactant is limiting)?

A)
B)
C)
D)
E)

Question 14

Write and balance molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and phases of the products in each of the cases.

-An aqueous solution of barium hydroxide is mixed with an aqueous solution of sulfuric acid.

Question 15

Write and balance molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and phases of the products in each of the cases.

-An aqueous solution of barium nitrate is mixed with an aqueous solution of potassium phosphate.

Question 16

The factors that most commonly cause chemical reactions to occur are all the following except

A) formation of a solid
B) formation of a gas
C) formation of water
D) transfer of electrons
E) a decrease in temperature

Question 17

Complete and write the balanced molecular equation for the following: An aqueous solution of magnesium chloride is added to an aqueous solution of silver nitrate.

Question 18

When solutions of barium hydroxide and sulfuric acid are mixed, the net ionic equation is
Ba²⁺(aq) + SO₄^2-(aq) $\rightarrow$ BaSO₄(s) because only the species involved in making the precipitate are included.

Question 19

An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of barium nitrate. Identify the solid in the balanced equation.

A) BaSO₄
B) (NH₄)₂SO₄
C) Ba(NO₃)₂
D) NH₄NO₃
E) There is no solid formed when the two solutions are mixed.

Question 20

Write and balance molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and phases of the products in each of the cases.

-An aqueous solution of silver nitrate is mixed with an aqueous solution of potassium carbonate.

Question 21

Electrons are transferred in combustion reactions.

Question 22

An aqueous solution of sodium sulfide is allowed to react with an aqueous solution of barium chloride. The complete ionic equation contains which of the following species (when balanced in standard form)?

A) 2Na⁺(aq)
B) Na⁺(aq)
C) 3Ba²⁺(aq)
D) 2S^2-(aq)
E) Cl^-(aq)

Question 23

An aqueous solution of sodium carbonate is allowed to react with an aqueous solution of magnesium chloride. The complete ionic equation contains which of the following species (when balanced in standard form)?

A) CO₃^2-(aq)
B) 2Na⁺(aq)
C) 2Mg²⁺(aq)
D) Cl^-(aq)
E) 2Cl^-(aq)

Question 24

An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)?

A)
B)
C)
D)
E)

Question 25

The reaction HNO₃(aq) + NaOH(aq) H₂O(l) + NaNO₃(aq) is a(n) ________ reaction.

A) acid-base
B) precipitation
C) oxidation-reduction
D) single replacement
E) none of these

Question 26

An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The net ionic equation contains which of the following species (when balanced in standard form)?

A)
B)
C)
D)
E) No net ionic equation exists for this reaction.

Question 27

How many of the following are oxidation-reduction reactions?
(I) reaction of a metal with a nonmetal
(II) synthesis
(III) combustion
(IV) precipitation
(V) decomposition

A) 1
B) 2
C) 3
D) 4
E) 5

Question 28

The reaction 2K(s) + Br₂(l) $\rightarrow$ 2KBr(s) is a(n) ______________ reaction.

A) precipitation
B) acid-base
C) oxidation-reduction
D) double-displacement
E) single-replacement

Question 29

The equation 2C₂H₆ + 7O₂ $\rightarrow$ 4CO₂ + 6H₂O is an oxidation-reduction reaction. and why?

A) True; the carbon is oxidized, and the oxygen is reduced.
B) True; the carbon is reduced, and the oxygen is oxidized.
C) True; the carbon is oxidized, and the hydrogen is reduced.
D) True; the oxygen is reduced, and the hydrogen is oxidized.
E) False

Question 30

An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The molecular equation contains which one of the following terms (when balanced in standard form)?

A) KCl(s)
B) KNO₃(aq)
C) KNa(aq)
D) ClNO₃(aq)
E) NaCl(s)

Question 31

An aqueous solution of ammonium sulfide is allowed to react with an aqueous solution of barium chloride. What is the coefficient of the solid in the balanced equation (in standard form)?

A) 1
B) 2
C) 3
D) 4
E) 5

Question 32

The reaction AgNO₃(aq) + NaCl(aq) $\rightarrow$ AgCl(s) + NaNO₃(aq) is a(n) ______________ reaction.

A) precipitation
B) acid-base
C) oxidation-reduction
D) single-replacement
E) none of these

Question 33

Balance the complete ionic equation when aqueous barium hydroxide reacts with aqueous hydrochloric acid.

Question 34

When the following equation is balanced, what is the coefficient for H₂O? Ca(OH)₂(aq) + H₃PO₄(aq) $\rightarrow$ Ca₃(PO₄)₂(s) + H₂O(l)

A) 2
B) 3
C) 4
D) 6
E) 8

Question 35

The scientist who discovered the essential nature of acids through solution conductivity studies is

A) Priestley
B) Boyle
C) Einstein
D) Mendeleev
E) Arrhenius

Question 36

An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. Identify the solid in the balanced equation.

A) KCl
B) NaNO₃
C) KNO₃
D) NaCl
E) There is no solid formed when the two solutions are mixed.

Question 37

The complete ionic equation contains only those substances directly involved in reactions in aqueous solutions.

Question 38

How many electrons are transferred in the following oxidation-reduction reaction? Zn(s) + 2AgNO₃(aq) $\rightarrow$ Zn(NO₃)₂(aq) + 2Ag(s)

A) 1
B) 2
C) 3
D) 4
E) 5

Question 39

Write the molecular equation, the complete ionic equation, and the net ionic equation for the following reaction: Aqueous solutions of copper(II) nitrate and sodium hydroxide are mixed to form solid copper(II) hydroxide and aqueous sodium nitrate.

Question 40

An aqueous solution of ammonium carbonate is allowed to react with an aqueous solution of nickel(II) chloride. Identify the solid in the balanced equation.

A) NiCO₃
B) NH₄Cl
C) NiCl₂
D) (NH₄)₂CO₃
E) There is no solid formed when the two solutions are mixed.

Question 41

Classify the following reaction: 2Mg(s) + O₂(g) $\rightarrow$ 2MgO(s)

A) oxidation-reduction
B) combustion
C) synthesis
D) two of the above
E) a-c are all correct.

Question 42

When a metal and a nonmetal react, the metal ______________ electrons and the nonmetal ______________ electrons.

Question 43

Use the following choices to classify each reaction given below (more than one choice may apply).


-The equation 2Al(s) + 2Br₂(l) $\rightarrow$ 2AlBr₃(s) is a(n) ______________ reaction.

A)oxidation-reduction and synthesis
B)oxidation-reduction only
C)synthesis only
D)decomposition
E)combustion

Question 44

Use the following choices to classify each reaction given below (more than one choice may apply).


-H₂SO₄(aq) + Ba(OH)₂(aq) $\rightarrow$ 2H₂O(l) + BaSO₄(s)

A) oxidation-reduction
B) acid-base
C) precipitation

Question 45

Use the following choices to classify each reaction given below (more than one choice may apply).


-The equation 2Ag₂O(s) $\rightarrow$ 4Ag(s) + O₂(g) is a(n) ______________ reaction.

A)oxidation-reduction
B)synthesis
C)decomposition
D)combustion
E)two of these

Question 46

Use the following choices to classify each reaction given below (more than one choice may apply).


-Ca(s) + H₂(g) $\rightarrow$ CaH₂(s)

A) oxidation-reduction
B) acid-base
C) precipitation

Question 47

Use the following choices to classify each reaction given below (more than one choice may apply).


-Na₂SO₄(aq) + Pb(NO₃)₂(aq) $\rightarrow$ PbSO₄(s) + 2NaNO₃(aq)

A) oxidation-reduction
B) acid-base
C) precipitation

Question 48

In what type of reaction is water always a product?

A) precipitation
B) acid-base
C) oxidation
D) decomposition
E) synthesis

Question 49

A reaction that involves a transfer of electrons is called a(n) ______________ reaction.

A) precipitation
B) acid-base
C) oxidation-reduction
D) double-displacement
E) none of these

Question 50

Use the following choices to classify each reaction given below (more than one choice may apply).


-KBr(aq) + AgNO₃(aq) $\rightarrow$ AgBr(s) + KNO₃(aq)

A) oxidation-reduction
B) acid-base
C) precipitation

Question 51

Classify the following reaction: HNO₃(aq) + KOH(aq) $\rightarrow$ KNO₃(aq) +H₂O(l)

A) oxidation-reduction
B) combustion
C) precipitation
D) acid-base
E) two of the above

Question 52

Use the following choices to classify each reaction given below (more than one choice may apply).


-HNO₃(aq) + NaOH(aq) $\rightarrow$ H₂O(l) + NaNO₃(aq)

A) oxidation-reduction
B) acid-base
C) precipitation

Question 53

Use the following choices to classify each reaction given below (more than one choice may apply).


-ZnBr₂(aq) + 2AgNO₃(aq) $\rightarrow$ Zn(NO₃)₂(aq) + 2AgBr(s)

A) oxidation-reduction
B) acid-base
C) precipitation

Question 54

Use the following choices to classify each reaction given below (more than one choice may apply).


-Zn(s) + 2HCl(aq) $\rightarrow$ H₂(g) + ZnCl₂(aq)

A) oxidation-reduction
B) acid-base
C) precipitation

Question 55

Use the following choices to classify each reaction given below (more than one choice may apply).


-CH₄(g) + 2O₂(g) $\rightarrow$ CO₂(g) + 2H₂O(g)

A)oxidation-reduction
B)synthesis
C)decomposition
D)combustion
E)two of these

Question 56

Use the following choices to classify each reaction given below (more than one choice may apply).


-Zr(s) + O₂(g) $\rightarrow$ ZrO₂(s)

A) oxidation-reduction
B) acid-base
C) precipitation

Question 57

Use the following choices to classify each reaction given below (more than one choice may apply).


-HC₂H₃O₂(aq) + CsOH(aq) $\rightarrow$ H₂O(l) + CsC₂H₃O₂(aq)

A) oxidation-reduction
B) acid-base
C) precipitation

Question 58

Oxidation and reduction must occur simultaneously.

Question 59

When the following equation is balanced in standard form, what is the coefficient in front of the H₂O? C₂H₆(g) + O₂(g) CO₂(g) + H₂O(g)

A) 6
B) 2
C) 4
D) 1
E) 7

Question 60

Which of the following statements is not true?

A) When a metal reacts with a nonmetal, an ionic compound is formed.
B) A metal-nonmetal reaction can always be assumed to be an oxidation-reduction reaction.
C) Two nonmetals can undergo an oxidation-reduction reaction.
D) When two nonmetals react, the compound formed is ionic.
E) A metal-nonmetal reaction involves electron transfer.

Question 61

Use the following choices to classify each reaction given below (more than one choice may apply).


-P₄(s) + 5O₂(g) $\rightarrow$ P₄O₁₀(s)

A) oxidation-reduction
B) acid-base
C) precipitation

Question 62

Use the following choices to classify each reaction given below (more than one choice may apply).


-S₈(s) + 12O₂(g) $\rightarrow$ 8SO₃(g)

A) oxidation-reduction
B) acid-base
C) precipitation

Question 63

Use the following choices to classify each reaction given below (more than one choice may apply).


-C₃H₈(g) + 5O₂(g) $\rightarrow$ 3CO₂(g) + 4H₂O(g)

A) oxidation-reduction
B) acid-base
C) precipitation

Question 64

Use the following choices to classify each reaction given below (more than one choice may apply).


-C(s) + O₂(g) $\rightarrow$ CO₂(g)

A) oxidation-reduction
B) acid-base
C) precipitation