Deck 4: Reactions in Aqueous Solution

Question 1

Which of the following ionic compounds is not soluble in water?

A) K₂CO₃
B) AgNO₃
C) CaBr₂
D) CsI
E) PbI₂

Answer 1

PbI₂

Question 2

What reaction occurs when aqueous solutions of silver nitrate and potassium iodide are mixed?

A) Ag⁺(aq)+ K⁺(aq)→ AgK(s)
B) NO₃−(aq)+ I−(aq)→ NO₃I(s)
C) NO₃−(aq)+ K⁺(aq)→ KNO₃(s)
D) Ag⁺(aq)+ NO₃−(aq)+ K⁺(aq)+ I−(aq)→ AgI(s)+ 2KNO₃(s)
E) Ag⁺(aq)+ I−(aq)→ AgI(s)

Answer 2

Ag⁺(aq)+ I−(aq)→ AgI(s)

Question 3

Which of the following ionic compounds are likely to be soluble in water: Mg(OH)₂,Pb(NO₃)₂,AgI,Na₂CO₃,and Cu₃(PO₄)₃?

A) Na₂CO₃ only
B) Pb(NO₃)₂ and Na₂CO₃
C) Mg(OH)₂,Na₂CO₃,and Cu₃(PO₄)₃
D) Mg(OH)₂,AgI,and Cu₃(PO₄)₃
E) Pb(NO₃)₂,AgI,Na₂CO₃,and Cu₃(PO₄)₃

Answer 3

Pb(NO₃)₂ and Na₂CO₃

Question 4

Precipitation reactions occur

A) when group 1 cations are mixed with group 17 anions.
B) when insoluble reactants are mixed.
C) when ionic compounds react to form non-ionic products.
D) predominantly with halide salts.
E) when soluble ionic reactants combine to form insoluble products.

Question 5

Which of the following compounds is least soluble in water?

A) Fe(OH)₃.
B) Sr(OH)₂.
C) Al(NO₃)₃.
D) KI.
E) CuCl₂.

Question 6

Which of the following reagents can be added to silver nitrate to precipitate the silver ion?

A) Pb(NO₃)₂
B) NH₄ClO₄
C) KNO₃
D) NaI
E) KClO₄

Question 7

Which of the following reagents can be added to a solution of sodium carbonate to precipitate the carbonate ion?

A) FeCl₃
B) MgBr₂
C) Cu(ClO₄)₂
D) Pb(NO₃)₂
E) all of the above

Question 8

What mass of precipitate is formed when 25.00 mL of 0.200 M BaCl₂ and 35.00 mL of 0.125 M Na₂SO₄ are mixed?

A) 0.510 g
B) 1.17 g
C) 1.02 g
D) 2.04 g
E) 0.583 g

Question 9

What is the net ionic equation for the reaction of aqueous sodium hydroxide and aqueous iron(II)chloride?

A) Na⁺(aq)+ OH^-(aq)→ NaOH(s)
B) Na⁺(aq)+ Cl^-(aq)→ NaCl(s)
C) Fe²⁺(aq)+ 2OH^-(aq)→ Fe(OH)₂(s)
D) Fe²⁺(aq)+ OH^-(aq)→ FeOH⁺(s)
E) Fe²⁺(aq)+ 2Cl^-(aq)→ FeCl₂(s)

Question 10

What volume of 0.250 M KCl(aq)will completely react with 50.0 mL of 0.115 M Pb(NO₃)₂(aq)? Pb²⁺(aq)+ 2Cl−(aq)→ PbCl₂(s)

A) 23.0 mL
B) 46.0 mL
C) 11.5 mL
D) 109 mL
E) 218 mL

Question 11

Write a balanced net ionic equation for the reaction of aqueous solutions of lead(II)nitrate and potassium chloride.

A) Pb(NO₃)₂(aq)+ 2KCl(aq)→ PbCl₂(s)+ 2KNO₃(aq)
B) Pb²⁺(aq)+ 2K⁺(aq)→ PbK₂(s)
C) Pb²⁺(aq)+ 2Cl−(aq)→ PbCl₂(s)
D) NO₃−(aq)+ K⁺(aq)→ KNO₃(s)
E) no precipitation occurs.

Question 12

What reaction occurs when aqueous solutions of sodium hydroxide and copper(II)bromide are mixed?

A) Na⁺(aq)+ OH−(aq)+ Cu²⁺(aq)+ 2Br−(aq)→ NaCu(s)+ Br₂OH(aq)
B) Na⁺(aq)+ OH−(aq)+ CuBr₂(s)→ NaBr₂(aq)+ CuOH(s)
C) Na⁺(aq)+ Br−(aq)→ NaBr(s)
D) 2Na⁺(aq)+ Br₂(aq)→ 2NaBr(s)
E) 2OH−(aq)+ Cu²⁺(aq)→ Cu(OH)₂(s)

Question 13

Write a balanced net ionic equation for the reaction of manganese(II)hydroxide,Mn(OH)₂,with hydrochloric acid.

A) Mn(OH)₂(s)+ 2H⁺(aq)→ Mn²⁺(aq)+ 2H₂O(l)
B) Mn(OH)₂(s)+ 2H⁺(aq)→ MnH₂(s)+ 2OH−(aq)
C) (OH)₃(aq)+ 3H⁺(aq)→ 3H₂O(l)
D) 3OH−(aq)+ 3H⁺(aq)→ 3H₂O(l)
E) Mn²⁺(aq)+ 2Cl−(aq)→ MnCl₂(aq)

Question 14

If aqueous solutions of sodium sulfate and barium chloride are mixed,a white precipitate forms.What is the identity of the precipitate?

A) Na₂Ba
B) NaCl₂
C) NaCl
D) BaSO₄
E) Ba₂SO₄

Question 15

Identify all of the spectator ions in the precipitation reaction below. Ca²⁺(aq)+ 2Br−(aq)+ 2Li⁺(aq)+ CO₃²⁻(aq)→ CaCO₃(s)+ 2Li⁺(aq)+ 2Br−(aq)

A) Ca²⁺ and Li⁺
B) Br− and CO₃²⁻
C) Br− and Li⁺
D) CaCO₃
E) Ca²⁺,Br−,Li⁺,and CO₃²⁻

Question 16

Which of the following pairs of aqueous solutions will produce a precipitate when mixed?

A) NaCl(aq)and Ca(NO₃)₂(aq)
B) KCl(aq)and NaOH(aq)
C) Cu(NO₃)₂(aq)and AgNO₃(aq)
D) ZnSO₄(aq)and LiCl(aq)
E) K₂SO₄(aq)and Pb(ClO₄)₂(aq)

Question 17

If aqueous solutions of nickel(II)chloride and potassium phosphate are mixed,which insoluble compound will form?

A) Ni₃(PO₄)₂
B) NiCl₂
C) KCl
D) K₂Ni
E) K₃PO₄

Question 18

What net ionic reaction occurs when aqueous solutions of potassium carbonate and iron(III)bromide are mixed?

A) CO₃²⁻(aq)+ 2Fe⁺(aq)→ Fe₂CO₃(s)
B) 3CO₃²⁻(aq)+ 2Fe³⁺(aq)→ Fe₂(CO₃)₃(s)
C) 3CO₃²⁻(aq)+ 6Fe⁺(aq)→ 3Fe₂CO₃(s)
D) 3K₂CO₃(aq)+ 2Fe³⁺(aq)+ 6Br−(aq)→ Fe₂(CO₃)₃(s)+ 6KBr(s)
E) no reaction occurs

Question 19

If an aqueous solution of ____ is added to a mixture of Pb²⁺ and Ba²⁺,the lead ion will precipitate,but the barium ion will remain in solution.

A) NaOH
B) Na₂SO₄
C) K₃PO₄
D) KCO₃
E) Ca(CH₃CO₂)₂

Question 20

Identify all of the spectator ions in the reaction below. Zn(OH)₂(s)+ 2H⁺(aq)+ 2NO₃−(aq)→ Zn²⁺(aq)+ 2NO₃−(aq)+ 2H₂O(l)

A) Zn(OH)₂
B) NO₃−
C) Zn²⁺
D) H⁺
E) H⁺ and NO₃−

Question 21

The principal ingredient in Tums antacid tablets is calcium carbonate,CaCO₃.A single tablet contains 0.500 g CaCO₃.What volume of 0.2500 M HCl is required to titrate a tablet of Tums? 2H⁺(aq)+ CO₃²⁻(aq)→ H₂O(l)+ CO₂(g)

A) 0.0100 mL
B) 0.0200 mL
C) 10.0 mL
D) 20.0 mL
E) 40.0 mL

Question 22

A oxidizing agent is a species that

A) takes a proton from an Arrhenius acid.
B) is oxidized in a chemical reaction.
C) gains electrons in a chemical reaction.
D) loses electrons in a chemical reaction.
E) gives a proton to an Arrhenius base.

Question 23

According to the Arrhenius acid-base definition

A) acids produce H⁺ in aqueous solutions and bases produce OH− in aqueous solutions.
B) acids produce OH− in aqueous solutions and bases produce H⁺ in aqueous solutions.
C) acids only react with bases.
D) all hydrogen halides are strong acids.
E) acids and bases are strong electrolytes.

Question 24

Exactly 19.36 mL of 0.1481 M NaOH is used to titrate a 25.00 mL sample of HF.What is the concentration of the hydrofluoric acid?

A) 6.464 × 10−² M
B) 1.147 × 10−¹ M
C) 1.916 × 10−¹ M
D) 2.867 × 10−³ M
E) 6.570 × 10−³ M

Question 25

Which of the following compounds is a weak base?

A) NaOH
B) H₂CO₃
C) LiCl
D) NH₃
E) CH₃CO₂H

Question 26

Identify the oxidizing and reducing agents in the redox reaction below. 3Cu(s)+ 8H⁺(aq)+ 2NO₃−(aq)→ 3Cu²⁺(aq)+ 2NO(g)+ 4H₂O(l)

A) reducing agent: Cu;oxidizing agent: Cu²⁺
B) reducing agent: NO₃−;oxidizing agent: NO
C) reducing agent: Cu;oxidizing agent: NO₃−
D) reducing agent: NO₃−;oxidizing agent: Cu
E) reducing agent: H⁺;oxidizing agent: NO

Question 27

What is the balanced net ionic equation for the reaction between aqueous solutions of acetic acid and sodium hydroxide?

A) CH₃CO₂H(aq)+ OH−(aq)→ CH₃(aq)+ CO₃²⁻(aq)+ H₂(g)
B) CH₃CO₂H(aq)+ 3NaOH(aq)→ CCO₂H³⁻(aq)+ 3Na⁺(aq)+ H₂O(l)
C) CH₃CO₂H(aq)+ OH−(aq)→ CH₃−(aq)+ CO₂(g)+ H₂O(l)
D) CH₃CO₂H(aq)+ OH−(aq)→ CH₃CO₂−(aq)+ H₂O(l)
E) CH₃CO₂H(aq)+ 2Na⁺(aq)+ 2OH−(aq)→ CH₃CO₂²⁻(aq)+ 2Na⁺(aq)+ H₂O(l)

Question 28

Assign oxidation numbers to each atom in manganese(IV)oxide.

A) Mn = +4;O = 0
B) Mn = +4;O = −2
C) Mn = +2;O = 0
D) Mn = +2;O = −2
E) Mn = 0;O = 0

Question 29

In the laboratory,acid spills are often neutralized by adding sodium bicarbonate.What mass of sodium bicarbonate reacts with 225 mL of 6.00 M HCl? H⁺(aq)+ NaHCO₃(s)→ H₂O(l)+ CO₂(g)+ Na⁺(aq)

A) 1.35 g
B) 71.5 g
C) 113 g
D) 143 g
E) 2240 g

Question 30

What is the oxidation number of iodine in potassium iodate,KIO₃?

A) -1
B) 0
C) +3
D) +5
E) +7

Question 31

Assign oxidation numbers to each atom in sodium hydrogen carbonate,NaHCO₃?

A) Na = +1,H = -1,C = +6,O = -2
B) Na = +1,H = +1,C = +4,O = -2
C) Na = +1,H = -1,C = +2,O = -2
D) Na = -1,H = +1,C = 0,O = -2
E) Na = 0,H = 0,C = 0,O = 0

Question 32

When HCl(g)and NH₃(g)are mixed,a white solid forms.What is the balanced equation for this reaction?

A) HCl(g)+ NH₃(g)→ NH₄Cl(s)
B) HCl(g)+ NH₃(g)→ NH₂Cl(g)+ H₂(s)
C) HCl(g)+ NH₃(g)→ NH₄(s)+ Cl(g)
D) HCl(g)+ NH₃(g)→ NH₂Cl(s)+ H₂(g)
E) 3HCl(g)+ NH₃(g)→ NCl₃(s)+ 3H₂(g)

Question 33

Balance the reaction and identify which species is reduced and which is oxidized. Na(s)+ H₂O(l)→ Na⁺(aq)+ OH−(aq)+ H₂(g)

A) Na(s)+ H₂O(l)→ Na⁺(aq)+ OH−(aq)+ H₂(g);Na reduced,H₂O oxidized
B) 2Na(s)+ 2H₂O(l)→ 2Na⁺(aq)+ 2OH−(aq)+ H₂(g);Na reduced,H₂O oxidized
C) Na(s)+ H₂O(l)→ Na⁺(aq)+ OH−(aq)+ H₂(g);H₂O reduced,Na oxidized
D) 2Na(s)+ 2H₂O(l)→ 2Na⁺(aq)+ 2OH−(aq)+ H₂(g);H₂O reduced,Na oxidized
E) 2Na(s)+ 2H₂O(l)→ 2Na⁺(aq)+ 2OH−(aq)+ H₂(g);not a redox reaction

Question 34

Which list contains only strong acids?

A) HCl,HNO₃,HF,HClO₄
B) H₂SO₄,H₃PO₄,HClO₄,NH₃
C) HCl,HNO₃,H₃PO₄,HClO₄
D) HCl,H₂SO₄,HClO₄,HI
E) HNO₃,H₂SO₄,NaOH,H₃PO₄

Question 35

Which of the following are strong bases: NH₃,NaOH,Ba(OH)₂,and HF?

A) NH₃ and HF
B) NaOH and Ba(OH)₂
C) NH₃ and NaOH
D) NaOH,Ba(OH)₂,and HF
E) NH₃,NaOH,Ba(OH)₂,and HF

Question 36

What is the net ionic equation for the reaction of aqueous hydrochloric acid and aqueous potassium hydroxide?

A) HCl(aq)+ OH^-(aq)→ H₂O(l)+ Cl^-(aq)
B) Cl^-(aq)+ K⁺(aq)→ KCl(s)
C) HCl(aq)+ KOH(aq)→ KCl(aq)+ H₂O(l)
D) Cl^-(aq)+ K⁺(aq)→ KCl(aq)
E) H⁺(aq)+ OH^-(aq)→ H₂O(l)

Question 37

Which of the following compounds is a weak acid?

A) HCl
B) H₃PO₄
C) HNO₃
D) HClO₄
E) H₂SO₄

Question 38

What is the oxidation half-reaction for the reaction of zinc with hydrochloric acid? Zn(s)+ 2H⁺(aq)→ Zn²⁺(aq)+ H₂(g)

A) Zn(s)→ Zn²⁺(aq)+ 2e−
B) Zn(s)+ 2e− → Zn²⁺(aq)
C) 2H⁺(aq)→ H₂(g)+ 2e−
D) 2H⁺(aq)+ 2e− → H₂(g)
E) none of the above

Question 39

What are the spectator ions in the reaction between aqueous hydrobromic acid and aqueous sodium hydroxide?

A) Na⁺ only
B) H⁺ and OH^-
C) Na⁺ and Br^-
D) Br^- only
E) H⁺,Br^-,Na⁺,and OH^-

Question 40

A mass of 0.4113 g of an unknown acid,HA,is titrated with NaOH(aq).If the acid reacts with 28.10 mL of 0.1055 M NaOH(aq),what is the molar mass of the acid?

A) 2.965 × 10^-3 g/mol
B) 9.128 g/mol
C) 138.7 g/mol
D) 337.3 g/mol
E) 820.7 g/mol

Question 41

What volume of 0.2500 M cobalt(III)sulfate is required to react completely with 5.00 g of sodium carbonate?

A) 62.9 mL
B) 78.6 mL
C) 10.2 mL
D) 11.7 mL
E) 31.4 mL

Question 42

Identify the reaction type for the reaction between potassium metal and hydrochloric acid. 2K(s)+ 2H⁺(aq)→ 2K⁺(aq)+ H₂(g)

A) precipitation
B) acid-base
C) oxidation-reduction
D) both answers a and c
E) none of the above

Question 43

What is the reduction half-reaction for the equation below? 5Fe²⁺(aq)+ MnO₄−(aq)+ 8H⁺(aq)→ 5Fe³⁺(aq)+ Mn²⁺(aq)+ 4H₂O(l)

A) MnO₄−(aq)+ 5e− → Mn²⁺(aq)+ 2O₂(g)
B) MnO₄−(aq)+ 8H⁺(aq)+ 5e− → Mn²⁺(aq)+ 4H₂O(l)
C) Fe²⁺(aq)+ e− → Fe³⁺(aq)
D) 8H⁺(aq)+ 8e− → 8H₂O(l)
E) none of the above

Question 44

In the reaction given below,how many grams of sodium metal are consumed if 2.02 g of hydrogen gas are produced? 2Na(s)+ 2H₂O(l)→ 2NaOH(aq)+ H₂(g)

A) 92.0 g
B) 5.75 g
C) 11.5 g
D) 23.0 g
E) 46.0 g

Question 45

How many grams of KClO₃ are needed to produce of 2.56 grams of O₂? 2KClO₃(s)→ 2KCl(s)+ 3O₂(g)

A) 1.00 g
B) 1.71 g
C) 6.53 g
D) 9.80 g
E) 14.7 g

Question 46

Which of the pictorial representations best represents the precipitation reaction that occurs between aqueous solutions of Fe³⁺ and OH−? Assume that the circles represent cations and the squares represent anions.

A)
B)
C)
D)
E)

Question 47

Write a balanced half-reaction for the reduction of permanganate ion,MnO₇−,to Mn²⁺ in an acidic solution.

A) MnO₄−(aq)+ 4H₂O(l)→ Mn²⁺(aq)+ 8OH−(aq)
B) MnO₄−(aq)+ 8H⁺(aq)+ 5e− → Mn²⁺(aq)+ 4H₂O(l)
C) MnO₄−(aq)+ 5e− → Mn²⁺(aq)+ 4O^2-(aq)
D) MnO₄−(aq)→ Mn²⁺(aq)+ 4O²⁻(aq)
E) MnO₄−(aq)+ 4H⁺(aq)+ 5e− → Mn²⁺(aq)+ 4OH−(aq)