Question 1

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

Accepted Answer

A)  2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2O(l) + CO2(g) + 2 Na+(aq) + 2 Cl-(aq) 
B)  2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 NaCl(s) 
C)  2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g) 
D)  2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 Na+(aq) + 2 Cl-(aq) 
E)  No reaction occurs. 
A)  2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2O(l) + CO2(g) + 2 Na+(aq) + 2 Cl-(aq) 
B)  2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 NaCl(s) 
C)  2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g) 
D)  2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 Na+(aq) + 2 Cl-(aq) 
E)  No reaction occurs.

Question 2

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

Question 3

How many grams of NaCl are required to make 250.00 mL of a 3.000 M solution?

Accepted Answer

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

Question 4

Balance the chemical equation given below,and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 35.00 mL of 0.00150 M calcium hydroxide. _____ Ca(OH)2(aq)+ _____ H3PO4(aq)→ _____ Ca3(PO4)2(aq)+ _____ H2O(l)

Accepted Answer

A)  2.36 mL 
B)  11.7 mL 
C)  17.5 mL 
D)  26.2 mL 
A)  2.36 mL 
B)  11.7 mL 
C)  17.5 mL 
D)  26.2 mL

Question 5

What is the molar concentration of phosphate ions in a 0.350 M Li3PO4 solution?

Accepted Answer

A)  0.117 M 
B)  0.350 M 
C)  1.05 M 
D)  1.40 M 
E)  4.40 M 
A)  0.117 M 
B)  0.350 M 
C)  1.05 M 
D)  1.40 M 
E)  4.40 M

Question 6

Identify ammonia.

Accepted Answer

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

Question 7

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2 Mg(s)+   (g)→ 2 MgO(s)
When 3.50 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

Accepted Answer

A)  3.50 
B)  5.80 
C)  0.144 
D)  2.90 
E)  11.6 
A)  3.50 
B)  5.80 
C)  0.144 
D)  2.90 
E)  11.6

Question 8

Identify the oxidation state of Mg in Mg(s). Mg(s)+ 2 HCl(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 9

How many grams of C   OH must be added to water to prepare 325 mL of a solution that is 4.50 M CH3OH?

Accepted Answer

A)  47.0 g 
B)  144 g 
C)  11.2 g 
D)  0.325 g 
E)  18.0 g 
A)  47.0 g 
B)  144 g 
C)  11.2 g 
D)  0.325 g 
E)  18.0 g

Question 10

What is the concentration of NO3- ions in a solution prepared by dissolving 30.0 g of Ca(NO3)2 in enough water to produce 300.mL of solution?

Accepted Answer

A)  0.305 M 
B)  0.609 M 
C)  0.806 M 
D)  1.22 M 
A)  0.305 M 
B)  0.609 M 
C)  0.806 M 
D)  1.22 M

Question 11

Which of the following compounds is an Arrhenius base?

Accepted Answer

A)  CH3OH 
B)  CH3CO2H 
C)  HOI 
D)  KOH 
A)  CH3OH 
B)  CH3CO2H 
C)  HOI 
D)  KOH

Question 12

Give the spectator ions for the reaction that occurs when aqueous solutions of H2SO4 and KOH are mixed.

Accepted Answer

A)  H+ and OH- 
B)  K+ and SO42- 
C)  H+ and SO42- 
D)  OH- and K+ 
E)  No spectator ions are present. 
A)  H+ and OH- 
B)  K+ and SO42- 
C)  H+ and SO42- 
D)  OH- and K+ 
E)  No spectator ions are present.

Question 13

Calculate the number of grams of solute in 500.0 mL of 0.169 M KOH.

Accepted Answer

A)  166 g 
B)  1.51 g 
C)  4.74 × 103 g 
D)  4.74 g 
E)  1.51 × 10-3 g 
A)  166 g 
B)  1.51 g 
C)  4.74 × 103 g 
D)  4.74 g 
E)  1.51 × 10-3 g

Question 14

Determine the molarity of a solution formed by dissolving 4.00 moles of KBr in enough water to yield 3.00 L of solution.

Accepted Answer

A)  1.33 M 
B)  2.00 M 
C)  0.750 M 
D)  3.00 M 
E)  12.00 M 
A)  1.33 M 
B)  2.00 M 
C)  0.750 M 
D)  3.00 M 
E)  12.00 M

Question 15

Consider the following reaction.How many moles of oxygen are required to produce 2.00 moles of carbon dioxide? Assume that there is excess C3H7SH present. C3H7SH(l)+ 6 O2(g)→ 3 CO2(g)+ SO2(g)+ 4 H2O(g)

Accepted Answer

A)  1.00 moles O2 
B)  3.00 moles O2 
C)  2.00 moles O2 
D)  4.00 moles O2 
E)  2.50 moles O2 
A)  1.00 moles O2 
B)  3.00 moles O2 
C)  2.00 moles O2 
D)  4.00 moles O2 
E)  2.50 moles O2

Question 16

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

Accepted Answer

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

Question 17

What is the concentration (M)of CH3OH in a solution prepared by dissolving 12.5 g of CH3OH in sufficient water to give exactly 230 mL of solution?

Accepted Answer

A)  1.70 M 
B)  0.391 M 
C)  0.0543 M 
D)  0.700 M 
E)  6.20 M 
A)  1.70 M 
B)  0.391 M 
C)  0.0543 M 
D)  0.700 M 
E)  6.20 M

Question 18

What is the oxidation number of the sulfur atom in SO42-?

Accepted Answer

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

Question 19

How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 0.690 g of Fe2S3 if the percent yield for the reaction is 65.0%? 3 Na2S(aq)+ 2 FeCl3(aq)→ Fe2S3(s)+ 6 NaCl(aq)

Accepted Answer

A)  12.8 mL 
B)  21.6 mL 
C)  25.5 mL 
D)  51.1 mL 
A)  12.8 mL 
B)  21.6 mL 
C)  25.5 mL 
D)  51.1 mL

Question 20

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

Accepted Answer

A)  NH4NO3 + Li2CO3 
B)  Hg2(NO3)2 + KBr 
C)  KI + Li3PO4 
D)  AgC2H3O2 + Cu(NO3)2 
E)  None of the above solution pairs will produce a precipitate. 
A)  NH4NO3 + Li2CO3 
B)  Hg2(NO3)2 + KBr 
C)  KI + Li3PO4 
D)  AgC2H3O2 + Cu(NO3)2 
E)  None of the above solution pairs will produce a precipitate.

Exam 4: Chemical Quantities and Aqueous Reactions

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

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

How many grams of NaCl are required to make 250.00 mL of a 3.000 M solution?

Balance the chemical equation given below,and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 35.00 mL of 0.00150 M calcium hydroxide. _____ Ca(OH)2(aq)+ _____ H3PO4(aq)→ _____ Ca3(PO4)2(aq)+ _____ H2O(l)

What is the molar concentration of phosphate ions in a 0.350 M Li3PO4 solution?

Identify ammonia.

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2 Mg(s)+ (g)→ 2 MgO(s) When 3.50 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

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

How many grams of C OH must be added to water to prepare 325 mL of a solution that is 4.50 M CH3OH?

What is the concentration of NO3- ions in a solution prepared by dissolving 30.0 g of Ca(NO3)2 in enough water to produce 300.mL of solution?

Which of the following compounds is an Arrhenius base?

Give the spectator ions for the reaction that occurs when aqueous solutions of H2SO4 and KOH are mixed.

Calculate the number of grams of solute in 500.0 mL of 0.169 M KOH.

Determine the molarity of a solution formed by dissolving 4.00 moles of KBr in enough water to yield 3.00 L of solution.

Consider the following reaction.How many moles of oxygen are required to produce 2.00 moles of carbon dioxide? Assume that there is excess C3H7SH present. C3H7SH(l)+ 6 O2(g)→ 3 CO2(g)+ SO2(g)+ 4 H2O(g)

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

What is the concentration (M)of CH3OH in a solution prepared by dissolving 12.5 g of CH3OH in sufficient water to give exactly 230 mL of solution?

What is the oxidation number of the sulfur atom in SO42-?

How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 0.690 g of Fe2S3 if the percent yield for the reaction is 65.0%? 3 Na2S(aq)+ 2 FeCl3(aq)→ Fe2S3(s)+ 6 NaCl(aq)

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

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Chemical Bonding I: Lewis Theory

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

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

Balance the chemical equation given below,and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 35.00 mL of 0.00150 M calcium hydroxide. ___ Ca(OH)₂(aq)+ _ H₃PO₄(aq)→ _ Ca₃(PO₄)₂(aq)+ ___ H₂O(l)

What is the molar concentration of phosphate ions in a 0.350 M Li₃PO₄ solution?

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

How many grams of C OH must be added to water to prepare 325 mL of a solution that is 4.50 M CH₃OH?

What is the concentration of NO₃^- ions in a solution prepared by dissolving 30.0 g of Ca(NO₃)₂ in enough water to produce 300.mL of solution?

Give the spectator ions for the reaction that occurs when aqueous solutions of H₂SO₄ and KOH are mixed.

Consider the following reaction.How many moles of oxygen are required to produce 2.00 moles of carbon dioxide? Assume that there is excess C₃H₇SH present. C₃H₇SH(l)+ 6 O₂(g)→ 3 CO₂(g)+ SO₂(g)+ 4 H₂O(g)

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

What is the concentration (M)of CH₃OH in a solution prepared by dissolving 12.5 g of CH₃OH in sufficient water to give exactly 230 mL of solution?

What is the oxidation number of the sulfur atom in SO₄^2-?

How many milliliters of 0.200 M FeCl₃ are needed to react with an excess of Na₂S to produce 0.690 g of Fe₂S₃ if the percent yield for the reaction is 65.0%? 3 Na₂S(aq)+ 2 FeCl₃(aq)→ Fe₂S₃(s)+ 6 NaCl(aq)