Deck 9: Introduction to Solutions and Aqueous Reactions

Question 1

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of H₂SO₄ and KOH are mixed.

A) H⁺(aq) + OH^-(aq) → H₂O(l)
B) 2 K⁺(aq) + SO₄^2-(aq) → K₂SO₄(s)
C) H⁺(aq) + OH^-(aq) + 2 K⁺(aq) + SO₄^2-(aq) → H₂O(l) + K₂SO₄(s)
D) H₂²⁺(aq) + OH^-(aq) → H₂(OH)₂(l)
E) No reaction occurs.

Answer 1

H⁺(aq) + OH^-(aq) → H₂O(l)

Question 2

Give the complete ionic equation for the reaction (if any)that occurs when aqueous solutions of MgSO₃ and HI are mixed.

A) 2 H⁺(aq) + SO₃^2-(aq) → H₂SO₃(s)
B) Mg²⁺(aq) + 2 I^-(aq) → MgI₂(s)
C) 2 H⁺(aq) + SO₃^2-(aq) + Mg²⁺(aq) + 2 I^-(aq)→ H₂SO₃(s) + MgI₂(aq)
D) 2 H⁺(aq) + SO₃^2-(aq) → H₂O(l) + SO₂(g)
E) No reaction occurs.

Answer 2

2 H⁺(aq) + SO₃^2-(aq) → H₂O(l) + SO₂(g)

Question 3

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution.

A) 1.50 M
B) 1.18 M
C) 0.130 M
D) 0.768 M
E) 2.30 M

Answer 3

1.50 M

Question 4

How many molecules of sucrose (C₁₂H₂₂O₁₁,molar mass = 342.30 g/mol)are contained in 14.3 mL of 0.140 M sucrose solution?

A) 8.29 × 10²² molecules C₁₂H₂₂O₁₁
B) 1.21 × 10²¹ molecules C₁₂H₂₂O₁₁
C) 6.15 × 10²² molecules C₁₂H₂₂O₁₁
D) 1.63 × 10²³ molecules C₁₂H₂₂O₁₁
E) 5.90 × 10²⁴ molecules C₁₂H₂₂O₁₁

Question 5

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of Al(C₂H₃O₂)₃ and LiNO₃ are mixed.

A) Al³⁺(aq) + 3 NO₃^-(aq) → Al(NO₃)₃(s)
B) Li⁺(aq) + C₂H₃O₂^-(aq) → LiC₂H₃O₂(s)
C) Al³⁺(aq) + 3 NO₃^-(aq) + Li⁺(aq) + C₂H₃O₂^-(aq) → Al(NO₃)₃(aq) + LiC₂H₃O₂(s)
D) 3 Li⁺(aq) + (C₂H₃O₂)₃^3-(aq) → Li₃(C₂H₃O₂)_3(s)
E) No reaction occurs.

Question 6

According to the following reaction,what mass of PbCl₂ can form from 235 mL of 0.110 M KCl solution? Assume that there is excess Pb(NO₃)₂.
2 KCl(aq)+ Pb(NO₃)₂(aq)→ PbCl₂(s)+ 2 KNO₃(aq)

A) 7.19 g
B) 3.59 g
C) 1.80 g
D) 5.94 g
E) 1.30 g

Question 7

Identify acetic acid.

A) strong electrolyte, weak acid
B) weak electrolyte, weak acid
C) strong electrolyte, strong acid
D) weak electrolyte, strong acid
E) nonelectrolyte

Question 8

What volume of 0.305 M AgNO₃ is required to react exactly with 155.0 mL of 0.274 M Na₂SO₄ solution? Hint: You will want to write a balanced reaction.

A) 581 mL
B) 173 mL
C) 345 mL
D) 139 mL
E) 278 mL

Question 9

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of Na₂CO₃ and HCl are mixed.

A) 2 H⁺(aq) + CO₃^2-(aq) → H₂CO₃(s)
B) 2 Na⁺(aq) + CO₃^2-(aq) + 2 H⁺(aq) + 2 Cl^-(aq) → H₂CO₃(s) + 2 NaCl(aq)
C) 2 H⁺(aq) + CO₃^2-(aq) → H₂O(l) + CO₂(g)
D) 2 Na⁺(aq) + CO₃^2-(aq) + 2 H⁺(aq) + 2 Cl^-(aq) → H₂CO₃(s) + 2 Na⁺(aq) + 2 Cl^-(aq)
E) No reaction occurs.

Question 10

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of K₂S and Fe(NO₃)₂ are mixed.

A) K⁺(aq) + NO₃^-(aq) → KNO₃(s)
B) Fe²⁺(aq) + S^2-(aq) + 2 K⁺(aq) + 2 NO₃^-(aq) → FeS(s) + 2 K⁺(aq) + 2 NO₃^-(aq)
C) Fe²⁺(aq) + S^2-(aq) + 2 K⁺(aq) + 2 NO₃^-(aq) → Fe²⁺(aq) + S^2-(aq) + 2 KNO₃(s)
D) Fe²⁺(aq) + S^2-(aq) → FeS(s)
E) No reaction occurs.

Question 11

Give the complete ionic equation for the reaction (if any)that occurs when aqueous solutions of lithium sulfide and copper (II)nitrate are mixed.

A) Li⁺(aq) + SO₄^2-(aq) + Cu⁺(aq) + NO₃^-(aq) → CuS(s) + Li⁺(aq) + NO₃^-(aq)
B) Li⁺(aq) + S^-(aq) + Cu⁺(aq) + NO₃^-(aq) → CuS(s) + LiNO₃(aq)
C) 2 Li⁺(aq) + S^2-(aq) + Cu²⁺(aq) + 2 NO₃^-(aq) → Cu²⁺(aq) + S^2-(aq) + 2 LiNO₃(s)
D) 2 Li⁺(aq) + S^2-(aq) + Cu²⁺(aq) + 2 NO₃^-(aq) → CuS(s) + 2 Li⁺(aq) + 2 NO₃^-(aq)
E) No reaction occurs.

Question 12

Determine the molarity of a solution formed by dissolving 468 mg of MgI₂ in enough water to yield 50.0 mL of solution.

A) 0.0297 M
B) 0.0337 M
C) 0.0936 M
D) 0.0107 M
E) 0.0651 M

Question 13

Identify HCl.

A) strong electrolyte, weak acid
B) weak electrolyte, weak acid
C) strong electrolyte, strong acid
D) weak electrolyte, strong acid
E) nonelectrolyte

Question 14

Which of the following is an acid-base reaction?

A) C(s) + O₂(g) → CO₂(g)
B) 2 HClO₄(aq) + Ca(OH)₂(aq) → 2 H₂O(l) + Ca(ClO₄)₂(aq)
C) Fe(s) + 2 AgNO₃(aq) → 2 Ag(s) + Fe(NO₃)₂(aq)
D) MgSO₄(aq) + Ba(NO₃)₂(aq) → Mg(NO₃)₂(aq) + BaSO₄(s)
E) None of the above are acid base reactions.

Question 15

Determine the number of grams H₂ formed when 250.0 mL of 0.743 M HCl solution reacts with 3.41 × 10²³ atoms of Fe according to the following reaction. 2 HCl(aq)+ Fe(s)→ H₂(g)+ FeCl₂(aq)

A) 0.374 g
B) 1.33 g
C) 1.14 g
D) 0.187 g
E) 1.51 g

Question 16

Which of the following is a gas-evolution reaction?

A) 2 C₂H₆(l) + 7 O₂(g) → 4 CO₂(g) + 6 H₂O(g)
B) 2 H₂(g) + O₂(g) → 2 H₂O(g)
C) LiCl(aq) + NaNO₃(aq) → LiNO₃(aq) + NaCl(g)
D) NH₄Cl(aq) + KOH(aq) → KCl(aq) + NH₃(g) + H₂O(l)
E) None of the above are gas-evolution reactions.

Question 17

What mass (in g)of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC₂H₃O₂ solution with 55.0 mL of 0.109 M MgCl₂ solution?
2 AgC₂H₃O₂(aq)+ MgCl₂(aq)→ 2 AgCl(s)+ Mg(C₂H₃O₂)₂(aq)

A) 0.838 g
B) 1.72 g
C) 0.859 g
D) 2.56 g
E) 1.70 g

Question 18

According to the following reaction,how many moles of Fe(OH)₂ can form from 175.0 mL of 0.227 M LiOH solution? Assume that there is excess FeCl₂.
FeCl₂(aq)+ 2 LiOH(aq)→ Fe(OH)₂(s)+ 2 LiCl(aq)

A) 3.97 × 10^-2 moles
B) 2.52 × 10^-2 moles
C) 1.99 × 10^-2 moles
D) 5.03 × 10^-2 moles
E) 6.49 × 10^-2 moles

Question 19

Choose the statement below that is TRUE.

A) A weak acid solution consists of mostly nonionized acid molecules.
B) The term "strong electrolyte" means that the substance is extremely reactive.
C) A strong acid solution consists of only partially ionized acid molecules.
D) The term "weak electrolyte" means that the substance is inert.
E) A molecular compound that does not ionize in solution is considered a strong electrolyte.

Question 20

According to the following reaction,what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO₃)₂ solution?
2 KCl(aq)+ Pb(NO₃)₂(aq)→ PbCl₂(s)+ 2 KNO₃(aq)

A) 97.4 mL
B) 116 mL
C) 43.0 mL
D) 86.1 mL
E) 58.1 mL

Question 21

Which of the following compounds will undergo a gas-evolving reaction in an aqueous solution?

A) CH₃COOH
B) HF
C) HCl
D) H₂SO₄
E) H₂CO₃

Question 22

A beaker contains 0.50 mol of potassium bromide in 600 mL of water.An additional 600 mL of water is added.The number of moles of potassium bromide in the beaker is

A) 0.50 mol.
B) 0.83 mol.
C) 0.25 mol.
D) 1.2 mol.
E) 0.42 mol.

Question 23

Which of the following is a strong electrolyte in solution?

A) CdS
B) FeCl₃
C) CH₃COOH
D) NiC₂O₄
E) PbMnO₄

Question 24

If 4.89 g of ZnCl₂ is dissolved in enough water to give a total volume of 500 mL,what is the molarity of the solution?

A) 0.217 M
B) 0.0179 M
C) 0.0717 M
D) 1.33 M
E) 0.849 M

Question 25

6.74 g of the monoprotic acid KHP (MW = 204.2 g/mol)is dissolved into water.The sample is titrated with a 0.703 M solution of calcium hydroxide to the equivalence point.What volume of base was used?

A) 8.64 mL
B) 11.8 mL
C) 23.5 mL
D) 47.0 mL
E) 93.9 mL

Question 26

Determine the oxidation state of P in PO₃^3-.

A) +3
B) +6
C) +2
D) 0
E) -3

Question 27

What element is undergoing reduction (if any)in the following reaction?
Zn(s)+ 2 AgNO₃(aq)→ Zn(NO₃)₂(aq)+ 2 Ag(s)

A) Zn
B) N
C) O
D) Ag
E) This is not an oxidation-reduction reaction.

Question 28

Determine the reducing agent in the following reaction. 2 Li(s)+ Fe(C₂H₃O₂)₂(aq)→ 2 LiC₂H₃O₂(aq)+ Fe(s)

A) O
B) H
C) C
D) Fe
E) Li

Question 29

Determine the oxidation state of nitrogen in NO.

A) +5
B) +3
C) 0
D) +2
E) +4

Question 30

The titration of 80.0 mL of an unknown concentration H₃PO₄ solution requires 126 mL of 0.218 M KOH solution.What is the concentration of the H₃PO₄ solution (in M)?

A) 1.03 M
B) 0.343 M
C) 0.114 M
D) 0.138 M
E) 0.0461 M

Question 31

Determine the oxidation state of nitrogen in NO₂.

A) +5
B) +3
C) 0
D) +2
E) +4

Question 32

What element is undergoing oxidation (if any)in the following reaction?
CH₄(g)+ 2 O₂(g)→ CO₂(g)+ 2 H₂O(g)

A) O
B) H
C) C
D) both C and H
E) None of the elements is undergoing oxidation.

Question 33

Determine the oxidizing agent in the following reaction. Ni(s)+ 2 AgClO₄(aq)→ Ni(ClO₄)₂(aq)+ 2 Ag(s)

A) Ag
B) Ni
C) Cl
D) O
E) This is not an oxidation-reduction reaction.

Question 34

When an aqueous solution of manganese (II)nitrate is combined with an aqueous solution of ammonium sulfide,what should precipitate out?

A) MnS
B) Mn(SO₃)₂
C) Mn(SO₄)₂
D) Mn₂SO₃
E) Mn₂SO₄

Question 35

What element is undergoing oxidation (if any)in the following reaction?
2 MnO₄^-(aq)+ 3 NO₂^-(aq)+ H₂O(l)→ 2 MnO₂(s)+ 3 NO₃^-(aq)+ 2 OH^-(aq)

A) Mn
B) O
C) N
D) H
E) This is not an oxidation-reduction reaction

Question 36

What is the name for an aqueous solution of HIO?

A) hydroiodic acid
B) hypoiodous acid
C) iodous acid
D) iodic acid
E) periodic acid

Question 37

Determine the oxidation state of C in CO₃^-2.

A) +4
B) +2
C) -2
D) -4
E) +6

Question 38

The titration of 25.0 mL of an unknown concentration H₂SO₄ solution requires 83.6 mL of 0.12 M LiOH solution.What is the concentration of the H₂SO₄ solution (in M)?

A) 0.20 M
B) 0.40 M
C) 0.10 M
D) 0.36 M
E) 0.25 M

Question 39

What element is undergoing oxidation (if any)in the following reaction?
Zn(s)+ 2 AgNO₃(aq)→ Zn(NO₃)₂(aq)+ 2 Ag(s)

A) Zn
B) N
C) O
D) Ag
E) This is not an oxidation-reduction reaction.

Question 40

All of the following compounds are soluble EXCEPT

A) Ba(OH)₂.
B) Pb(NO₃)₂.
C) ZnCl₂.
D) AgBr.
E) Cu(C₂H₃O₂)₂.

Question 41

What element is undergoing oxidation (if any)in the following reaction?
2 HCl(aq)+ Ca(OH)₂(aq)→ 2 H₂O(l)+ 2 CaCl₂(aq)

A) H
B) Cl
C) Ca
D) O
E) This is not an oxidation-reduction reaction

Question 42

How many liters of a 0.0550 M Li F solution contain 0.163 moles of Li F?

A) 3.37 L
B) 1.48 L
C) 8.97 L
D) 2.96 L
E) 1.12 L

Question 43

How many moles of Na I are required to make 250 mL of a 3.00 M solution?

A) 750 moles
B) 0.750 moles
C) 3 moles
D) 0.250 moles

Question 44

How many grams of AgNO₃ are needed to make 250.mL of a solution that is 0.155 M?

A) 0.105 g
B) 0.152 g
C) 6.58 g
D) 105 g

Question 45

Determine the oxidation state of Cl in ClO₃^-.

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

Question 46

What volume of 1.46 M CrBr₂ solution is required to react with 50.0 mL of 0.210 M Na₂CO₃ solution?
CrBr₂(aq)+ Na₂CO₃(aq)→ CrCO₃(s)+ 2NaBr(aq)

A) 139 mL
B) 45.3 mL
C) 7.19 mL
D) 1.68 mL
E) 34.6 mL

Question 47

Calculate the number of grams of solute in 250.0 mL of 0.179 M KOH.

A) 78.4
B) 0.798
C) 2.51 ×
D) 2.51
E) 7.98 × 10^-4

Question 48

How many milliliters of a 0.266 M CsNO₃ solution are required to make 150.0 mL of 0.075 M CsNO₃ solution?

A) 53.2 mL
B) 42.3 mL
C) 18.8 mL
D) 23.6 mL
E) 35.1 mL

Question 49

How many moles of Na F are contained in 258.6 mL of 0.0296 M Na F solution?

A) 1.31 × 10^-3 mol
B) 8.74 × 10^-3 mol
C) 1.14 × 10^-3 mol
D) 3.67 × 10^-3 mol
E) 7.65 × 10^-3 mol

Question 50

If 42.389 g of Fe₃Br₂ is dissolved in enough water to give a total volume of 750 mL,what is the molarity of the solution?

A) 0.327 M
B) 0.0971 M
C) 0.0327 M
D) 0.173M
E) 0.436 M

Question 51

How many grams of NaCl are required to make 300.0 mL of a 2.500 M solution?

A) 58.40 g
B) 175.3 g
C) 14.60 g
D) 43.83 g

Question 52

Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188 M Sr(NO₃)₂ solution to 150.0 mL.

A) 1.13 M
B) 0.0887 M
C) 0.0313 M
D) 0.0199 M
E) 0.0501 M

Question 53

How many milliliters of a 0.184 M RbNO₃ solution contain 0.113 moles of RbNO₃?

A) 543 mL
B) 163 mL
C) 614 mL
D) 885 mL
E) 326 mL

Question 54

Which of the following solutions will have the highest concentration of chloride ions?

A) 0.10 M NaCl
B) 0.10 M MgCl₂
C) 0.10 M AlCl₃
D) 0.05 M CaCl₂
E) All of these solutions have the same concentration of chloride ions.

Question 55

How many moles of CH₃CH₂Cl are contained in 548 mL of 0.0788 M CH₃CH₂Cl solution?

A) 4.32 × 10^-2 mol
B) 2.32 × 10^-2 mol
C) 6.95 × 10^-2 mol
D) 1.44 × 10^-2 mol
E) 5.26 × 10^-2 mol

Question 56

What is the concentration of nitrate ions in a 0.125 M Ba(NO₃)₂ solution?

A) 0.125 M
B) 0.0625 M
C) 0.375 M
D) 0.250 M
E) 0.160 M

Question 57

What volume (in mL)of 0.0887 M Mg Br₂ solution is needed to make 275.0 mL of 0.0224 M Mg Br₂ solution?

A) 72.3 mL
B) 91.8 mL
C) 10.9 mL
D) 69.4 mL
E) 14.4 mL

Question 58

Determine the concentration of a solution prepared by diluting 20.0 mL of a 0.200 M KCl to 250.0 mL.

A) 0.160 M
B) 0.0320 M
C) 2.50 M
D) 0.00800 M
E) 0.0160 M

Question 59

What is the concentration of magnesium ions in a 0.125 M Mg SO₄ solution?

A) 0.125 M
B) 0.0625 M
C) 0.375 M
D) 0.250 M
E) 0.160 M

Question 60

What is the concentration of FeCl₃ in a solution prepared by dissolving 30.0 g of FeCl₃ in enough water to make 275 mL of solution?

A) 6.73 × 10^-4 M
B) 0. 673 M
C) 1.49 M
D) 1.49 × 10³ M

Question 61

What volume of a 0.540 M NaOH solution contains 12.5 g of NaOH?

A) 0. 169 L
B) 0. 579 L
C) 1. 73 L
D) 5.92 L

Question 62

How many grams of C OH must be added to water to prepare 175mL of a solution that is 1.0 M CH₃OH?

Question 63

What is the concentration of NO₃^- ions in a solution prepared by dissolving 15.0 g of Ca(NO₃)₂ in enough water to produce 300.mL of solution?

A) 0. 152 M
B) 0. 305 M
C) 0. 403 M
D) 0.609 M

Question 64

What is the concentration of HCl in the final solution when 65 mL of a 9.0 M HCl solution is diluted with pure water to a total volume of 0.15 L?

A) 2.1 × 10^-2 M
B) 3.9 M
C) 21 M
D) 3.9 × 10³ M

Question 65

How many grams of NaOH (MW = 40.0)are there in 500.0 mL of a 0.175 M NaOH solution?

Question 66

How many aluminum ions are present in 65.5 mL of 0.210 M Al I₃ solution?

A) 4.02 × 10²³ aluminum ions
B) 5.79 × 10²⁴ aluminum ions
C) 2.48 × 10²² aluminum ions
D) 8.28 × 10²¹ aluminum ions
E) 1.21 × 10²² aluminum ions

Question 67

How many ions are present in 30.0 mL of 0.600 M H₂CO₃ solution?

A) 3.25 × 10²² ions
B) 2.17 × 10²² ions
C) 1.08 × 10²² ions
D) 5.42 × 10²² ions
E) 3.61 × 10²¹ ions

Question 68

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 7.00 g of K₃PO₄ in enough water to make 350.mL of solution?

A) 0.0 236 M
B) 0. 0943 M
C) 0. 377 M
D) 0. 754 M

Question 69

How many milliliters of a 9.0 M H₂SO₄ solution are needed to make 0.45 L of a 3.5 M solution?

A) 0. 18 mL
B) 1.2 mL
C) 180 mL
D) 1200 mL

Question 70

What is the concentration (M)of C OH in a solution prepared by dissolving 3.96 g of C OH in sufficient water to give exactly 230 mL of solution?

Question 71

What is the concentration (M)of a NaCl solution prepared by dissolving 5.3 g of NaCl in sufficient water to give 115 mL of solution?

Question 72

How many chloride ions are present in 65.5 mL of 0.210 M Al Cl₃ solution?

A) 4.02 × 10²³ chloride ions
B) 5.79 × 10²⁴ chloride ions
C) 2.48 × 10²² chloride ions
D) 8.28 × 10²¹ chloride ions
E) 1.21 × 10²² chloride ions

Question 73

How many milliliters of a stock solution of 12.1 M would be needed to prepare 0.500 L of 0.500 M ?

A) 0.0484
B) 20.7
C) 3.03
D) 48.4
E) 0.0207

Question 74

A FeCl₃ solution is 0.175 M.How many mL of a 0.175 M FeCl₃ solution are needed to make 650.mL of a solution that is 0.300 M in Cl^- ion?

A) 1.11 mL
B) 371 mL
C) 1110 mL
D) It is not possible to make a more concentrated solution from a less concentrated solution.

Question 75

A stock solution of is prepared and found to contain 12.1 M of .If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L,the concentration of the diluted solution is ________ M.

A) 0.242
B) 1.65
C) 0.605
D) 605
E) 242

Question 76

How many grams of P are in 325 mL of a 5.50 M solution of P ?

Question 77

What is the concentration (M)of sodium ions in 4.57 L of a .533 M P solution?

Question 78

Pure acetic acid ( )is a liquid and is known as glacial acetic acid.Calculate the molarity of a solution prepared by dissolving 15.00 mL of glacial acetic acid at 25°C in sufficient water to give 500.0 mL of solution.The density of glacial acetic acid at 25°C is 1.05 g/mL.

A) 1.89 × 10³ M
B) 31.5 M
C) 0.0315 M
D) 0.525 M
E) 5.25 × 10^-4 M

Question 79

What is the concentration of an AlCl₃ solution if 150.mL of the solution contains 550.mg of Cl^- ion?

A) 3.45 × 10^-2 M
B) 8.25 × 10^-2 M
C) 1.03 × 10^-1 M
D) 3.10 × 10^-1 M

Question 80

A student prepared a stock solution by dissolving 15.0 g of KOH in enough water to make 150.mL of solution.She then took 15.0 mL of the stock solution and diluted it with enough water to make water to make 65.0 mL of a final solution.What is the concentration of KOH for the final solution?

A) 0. 411 M
B) 0. 534 M
C) 1.87 M
D) 2.43 M