Question 1

Determine the concentration of a solution prepared by diluting 20.0 mL of 0.200 mol L-1 NaCl to 250.0 mL.

Accepted Answer

A) 0.160 mol L-1 
B) 0.0320 mol L-1 
C) 2.50 mol L-1 
D) 0.00800 mol L-1 
E) 0.0160 mol L-1 
A) 0.160 mol L-1 
B) 0.0320 mol L-1 
C) 2.50 mol L-1 
D) 0.00800 mol L-1 
E) 0.0160 mol L-1

Question 2

Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00 moles of O2. 2C8H18 + 25O2 → 16CO2 + 18H2O

Accepted Answer

A) 0.640 moles 
B) 64.0 moles 
C) 2.56 moles 
D) 16.0 moles 
A) 0.640 moles 
B) 64.0 moles 
C) 2.56 moles 
D) 16.0 moles

Question 3

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

Accepted Answer

A) K+(aq)+ NO3-(aq)→ KNO3(s) 
B) Fe2+(aq)+ S2-(aq)+ 2K+(aq)+ 2NO3-(aq)→ FeS(s)+ 2K+(aq)+ 2NO3-(aq) 
C) Fe2+(aq)+ S2-(aq)+ 2K+(aq)+ 2NO3-(aq)→ Fe2+(aq)+ S2-(aq)+ 2KNO3(s) 
D) Fe2+(aq)+ S2-(aq)→ FeS(s) 
E) No reaction occurs. 
A) K+(aq)+ NO3-(aq)→ KNO3(s) 
B) Fe2+(aq)+ S2-(aq)+ 2K+(aq)+ 2NO3-(aq)→ FeS(s)+ 2K+(aq)+ 2NO3-(aq) 
C) Fe2+(aq)+ S2-(aq)+ 2K+(aq)+ 2NO3-(aq)→ Fe2+(aq)+ S2-(aq)+ 2KNO3(s) 
D) Fe2+(aq)+ S2-(aq)→ FeS(s) 
E) No reaction occurs.

Question 4

Define a limiting reagent.

Accepted Answer

A limiting reagent is a reacta

Question 5

The mixing of which pair of reactants will result in a precipitation reaction?

Accepted Answer

A) Ba(NO3)2(aq)+ Na2CO3(aq) 
B) K2SO4(aq)+ Cu(NO3)2(aq) 
C) NaClO4(aq)+ (NH4)2S(aq) 
D) NH4Br(aq)+ NH4I(aq) 
A) Ba(NO3)2(aq)+ Na2CO3(aq) 
B) K2SO4(aq)+ Cu(NO3)2(aq) 
C) NaClO4(aq)+ (NH4)2S(aq) 
D) NH4Br(aq)+ NH4I(aq)

Question 6

The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of a 0.12 mol L-1 LiOH solution. What is the concentration of the H2SO4 solution (in mol L-1)?

Accepted Answer

A) 0.20 mol L-1 
B) 0.40 mol L-1 
C) 0.10 mol L-1 
D) 0.36 mol L-1 
E) 0.25 mol L-1 
A) 0.20 mol L-1 
B) 0.40 mol L-1 
C) 0.10 mol L-1 
D) 0.36 mol L-1 
E) 0.25 mol L-1

Question 7

Identify the oxidation state of Mg in 
MgCl2(aq). Mg(s)+ 2HCl(aq)→ MgCl2(aq)+ H2(g)

Accepted Answer

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

Question 8

Which of the following is an oxidation-reduction reaction?

Accepted Answer

A) HCl(aq)+ LiOH(aq)→ LiCl(aq)+ H2O(l) 
B) NaI(aq)+ AgNO3(aq)→ AgI(s)+ NaNO3(aq) 
C) Pb(C2H3O2)2(aq)+ 2NaCl(aq)→ PbCl2(s)+ 2NaC2H3O2(aq) 
D) Mg(s)+ 2HCl(aq)→ MgCl2(aq)+ H2(g) 
E) All of the above are oxidation-reduction reactions. 
A) HCl(aq)+ LiOH(aq)→ LiCl(aq)+ H2O(l) 
B) NaI(aq)+ AgNO3(aq)→ AgI(s)+ NaNO3(aq) 
C) Pb(C2H3O2)2(aq)+ 2NaCl(aq)→ PbCl2(s)+ 2NaC2H3O2(aq) 
D) Mg(s)+ 2HCl(aq)→ MgCl2(aq)+ H2(g) 
E) All of the above are oxidation-reduction reactions.

Question 9

What is the concentration of NO3- ions in a solution prepared by dissolving 25.0 g of Ca(NO3)2 in enough water to produce 300. mL of solution?

Accepted Answer

A) 0.254 mol L-1 
B) 0.508 mol L-1 
C) 0.672 mol L-1 
D) 1.02 mol L-1 
A) 0.254 mol L-1 
B) 0.508 mol L-1 
C) 0.672 mol L-1 
D) 1.02 mol L-1

Question 10

Identify the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 8.000 moles of O2. 2C8H18 + 25O2 → 16CO2 + 18H2O

Accepted Answer

A) 20.00% 
B) 25.00% 
C) 50.00% 
D) 12.50% 
A) 20.00% 
B) 25.00% 
C) 50.00% 
D) 12.50%

Question 11

How many ions are present in 30.0 mL of a 0.600 mol L-1 Na2CO3 solution?

Accepted Answer

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 
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 12

Which of the following is a weak electrolyte?

Accepted Answer

A) LiOH 
B) CaCl2 
C) MgCO3 
D) NaC2H3O2 
E) Li2SO4 
A) LiOH 
B) CaCl2 
C) MgCO3 
D) NaC2H3O2 
E) Li2SO4

Question 13

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

Accepted Answer

A) 0.10 mol L-1 NaCl 
B) 0.10 mol L-1 MgCl2 
C) 0.10 mol L-1 AlCl3 
D) 0.05 mol L-1 CaCl2 
E) All of these solutions have the same concentration of chloride ions. 
A) 0.10 mol L-1 NaCl 
B) 0.10 mol L-1 MgCl2 
C) 0.10 mol L-1 AlCl3 
D) 0.05 mol L-1 CaCl2 
E) All of these solutions have the same concentration of chloride ions.

Question 14

Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas. How many grams of oxygen are formed when 10.0 g of dinitrogen monoxide decomposes?

Accepted Answer

A) 0.275 g 
B) 3.64 g 
C) 7.27 g 
D) 14.5 g 
A) 0.275 g 
B) 3.64 g 
C) 7.27 g 
D) 14.5 g

Question 15

Calculate the number of grams of solute in 500.0 mL of 0.189 mol L-1 KOH.

Accepted Answer

A) 148 
B) 1.68 
C) 5.30 × 103 
D) 5.30 
E) 1.68 × 10-3 
A) 148 
B) 1.68 
C) 5.30 × 103 
D) 5.30 
E) 1.68 × 10-3

Question 16

A student prepared a stock solution by dissolving 10.0 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 65.0 mL of a final solution. What is the concentration of KOH for the final solution?

Accepted Answer

A) 0.274 mol L-1 
B) 0.356 mol L-1 
C) 2.81 mol L-1 
D) 3.65 mol L-1 
A) 0.274 mol L-1 
B) 0.356 mol L-1 
C) 2.81 mol L-1 
D) 3.65 mol L-1

Question 17

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+ O2(g)→ 2MgO(s)
When 4.00 g of magnesium burns, what is the theoretical yield of magnesium oxide?

Accepted Answer

A) 4.00 g 
B) 6.63 g 
C) 0.165 g 
D) 3.32 g 
E) 13.3 g 
A) 4.00 g 
B) 6.63 g 
C) 0.165 g 
D) 3.32 g 
E) 13.3 g

Question 18

Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide: Pb2+(aq)+ 2I-(aq)→ PbI2(s)
Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many millilitres of 3.550 mol L-1 HI(aq)must be added to a solution containing 0.700 mol of Pb(NO3)2(aq)completely precipitate the lead?

Accepted Answer

A) 2.54 × 10-3 mL 
B) 394 mL 
C) 197 mL 
D) 0.197 mL 
E) 0.394 mL 
A) 2.54 × 10-3 mL 
B) 394 mL 
C) 197 mL 
D) 0.197 mL 
E) 0.394 mL

Question 19

How many millilitres of 0.260 mol L-1 Na2S are needed to react with 40.00 mL of 0.315 mol L-1 AgNO3? Na2S(aq)+ 2AgNO3(aq)→ 2NaNO3(aq)+ Ag2S(s)

Accepted Answer

A) 24.2 mL 
B) 48.5 mL 
C) 66.0 mL 
D) 96.9 mL 
A) 24.2 mL 
B) 48.5 mL 
C) 66.0 mL 
D) 96.9 mL

Question 20

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

Accepted Answer

A) 2H+(aq)+ SO32-(aq)→ H2SO3(s) 
B) Mg2+(aq)+ 2I-(aq)→ MgI2(s) 
C) 2H+(aq)+ SO32-(aq)+ Mg2+(aq)+ 2I-(aq)→ H2SO3(s)+ MgI2(aq) 
D) 2H+(aq)+ SO32-(aq)→ H2O(l)+ SO2(g) 
E) No reaction occurs. 
A) 2H+(aq)+ SO32-(aq)→ H2SO3(s) 
B) Mg2+(aq)+ 2I-(aq)→ MgI2(s) 
C) 2H+(aq)+ SO32-(aq)+ Mg2+(aq)+ 2I-(aq)→ H2SO3(s)+ MgI2(aq) 
D) 2H+(aq)+ SO32-(aq)→ H2O(l)+ SO2(g) 
E) No reaction occurs.

Exam 4: Chemical Reactions and Stoichiometry

Determine the concentration of a solution prepared by diluting 20.0 mL of 0.200 mol L-1 NaCl to 250.0 mL.

Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00 moles of O2. 2C8H18 + 25O2 → 16CO2 + 18H2O

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

Define a limiting reagent.

The mixing of which pair of reactants will result in a precipitation reaction?

The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of a 0.12 mol L-1 LiOH solution. What is the concentration of the H2SO4 solution (in mol L-1)?

Identify the oxidation state of Mg in MgCl2(aq). Mg(s)+ 2HCl(aq)→ MgCl2(aq)+ H2(g)

Which of the following is an oxidation-reduction reaction?

What is the concentration of NO3- ions in a solution prepared by dissolving 25.0 g of Ca(NO3)2 in enough water to produce 300. mL of solution?

Identify the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 8.000 moles of O2. 2C8H18 + 25O2 → 16CO2 + 18H2O

How many ions are present in 30.0 mL of a 0.600 mol L-1 Na2CO3 solution?

Which of the following is a weak electrolyte?

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

Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas. How many grams of oxygen are formed when 10.0 g of dinitrogen monoxide decomposes?

Calculate the number of grams of solute in 500.0 mL of 0.189 mol L-1 KOH.

A student prepared a stock solution by dissolving 10.0 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 65.0 mL of a final solution. What is the concentration of KOH for the final solution?

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+ O2(g)→ 2MgO(s) When 4.00 g of magnesium burns, what is the theoretical yield of magnesium oxide?

How many millilitres of 0.260 mol L-1 Na2S are needed to react with 40.00 mL of 0.315 mol L-1 AgNO3? Na2S(aq)+ 2AgNO3(aq)→ 2NaNO3(aq)+ Ag2S(s)

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

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Determine the concentration of a solution prepared by diluting 20.0 mL of 0.200 mol L^-1 NaCl to 250.0 mL.

Give the theoretical yield, in moles, of CO₂from the reaction of 4.00 moles of C₈H₁₈ with 4.00 moles of O₂. 2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O

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

The titration of 25.0 mL of an unknown concentration H₂SO₄ solution requires 83.6 mL of a 0.12 mol L^-1 LiOH solution. What is the concentration of the H₂SO₄ solution (in mol L^-1)?

Identify the oxidation state of Mg in MgCl₂(aq). Mg(s)+ 2HCl(aq)→ MgCl₂(aq)+ H₂(g)

What is the concentration of NO₃^- ions in a solution prepared by dissolving 25.0 g of Ca(NO₃)₂ in enough water to produce 300. mL of solution?

Identify the percent yield when 28.16 g of CO₂ are formed from the reaction of 4.000 moles of C₈H₁₈ with 8.000 moles of O₂. 2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O

How many ions are present in 30.0 mL of a 0.600 mol L^-1 Na₂CO₃ solution?

Calculate the number of grams of solute in 500.0 mL of 0.189 mol L^-1 KOH.

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+ O₂(g)→ 2MgO(s) When 4.00 g of magnesium burns, what is the theoretical yield of magnesium oxide?

How many millilitres of 0.260 mol L^-1 Na₂S are needed to react with 40.00 mL of 0.315 mol L^-1 AgNO₃? Na₂S(aq)+ 2AgNO₃(aq)→ 2NaNO₃(aq)+ Ag₂S(s)

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