Question 1

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

Accepted Answer

A)  2 H+(aq) + CO32-(aq) → H2CO3(s) 
B)  2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 NaCl(aq) 
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 H+(aq) + CO32-(aq) → H2CO3(s) 
B)  2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 NaCl(aq) 
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

Balance the chemical equation given below,and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 40.00 mL of 0.00150 M calcium hydroxide. ________ Ca(OH)2(aq)+ ________ H3PO4(aq)→ ________ Ca3(PO4)2(aq)+ ________ H2O(l)

Accepted Answer

A)  2.70 mL 
B)  13.3 mL 
C)  20.0 mL 
D)  30.0 mL 
A)  2.70 mL 
B)  13.3 mL 
C)  20.0 mL 
D)  30.0 mL

Question 3

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

Accepted Answer

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

Question 4

Explain the difference between a strong and weak electrolyte.Give an example of each.

Accepted Answer

A strong electrolyte is either an ionic

Question 5

A solution is prepared by adding 1.50 g of solid NaCl to 50.0 mL of 0.100 M   .What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.

Accepted Answer

A)  0.713 
B)  0.613 
C)  0.130 
D)  0.230 
E)  0.513 
A)  0.713 
B)  0.613 
C)  0.130 
D)  0.230 
E)  0.513

Question 6

Which one of the following compounds is insoluble in water?

Accepted Answer

A)  K2SO4 
B)  NaNO3 
C)  Pb SO4 
D)  Rb2CO3 
A)  K2SO4 
B)  NaNO3 
C)  Pb SO4 
D)  Rb2CO3

Question 7

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

Accepted Answer

A)  K2CO3 + Na Br 
B)  Na2 SO4 + LiOH 
C)  CaS + Na2SO4 
D)  None of these solution pairs will produce a precipitate. 
E)  All of these solution pairs will produce a precipitate. 
A)  K2CO3 + Na Br 
B)  Na2 SO4 + LiOH 
C)  CaS + Na2SO4 
D)  None of these solution pairs will produce a precipitate. 
E)  All of these solution pairs will produce a precipitate.

Question 8

What reagent could be used to separate Br- from N O3- when added to an aqueous solution containing both?

Accepted Answer

A)  AgNO3(aq) 
B)  Ba(OH)2(aq) 
C)  CuSO4(aq) 
D)  NaI(aq) 
A)  AgNO3(aq) 
B)  Ba(OH)2(aq) 
C)  CuSO4(aq) 
D)  NaI(aq)

Question 9

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

Accepted Answer

A)  H F+ LiOH 
B)  Li2S + H F 
C)  K2CO3 + HNO3 
D)  MgCl2 + KOH 
E)  All of these solution pairs will produce a precipitate. 
A)  H F+ LiOH 
B)  Li2S + H F 
C)  K2CO3 + HNO3 
D)  MgCl2 + KOH 
E)  All of these solution pairs will produce a precipitate.

Question 10

Identify acetic acid.

Accepted Answer

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

Question 11

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

Accepted Answer

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

Question 12

Determine the oxidation state of Ti in Ti(SO4)2.

Accepted Answer

A)  +2 
B)  +4 
C)  +6 
D)  0 
E)  -2 
A)  +2 
B)  +4 
C)  +6 
D)  0 
E)  -2

Question 13

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

Accepted Answer

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

Question 14

H2SO4,H Br ,H ClO4,Li2CO3,and KI are all classified as

Accepted Answer

A)  acids. 
B)  nonelectrolytes. 
C)  strong electrolytes. 
D)  weak electrolytes. 
A)  acids. 
B)  nonelectrolytes. 
C)  strong electrolytes. 
D)  weak electrolytes.

Question 15

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

Accepted Answer

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

Question 16

Which of the following compounds is NOT an Arrhenius acid?

Accepted Answer

A)  CH3CO2H 
B)  N H3     
C)  HNO2 
D)  H2SO4 
A)  CH3CO2H 
B)  N H3     
C)  HNO2 
D)  H2SO4

Question 17

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)

Accepted Answer

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

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

Balance the chemical equation given below,and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 40.00 mL of 0.00150 M calcium hydroxide. Ca(OH)₂(aq)+ H₃PO₄(aq)→ Ca₃(PO₄)₂(aq)+ H₂O(l)

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

Explain the difference between a strong and weak electrolyte.Give an example of each.

A solution is prepared by adding 1.50 g of solid NaCl to 50.0 mL of 0.100 M .What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.

Which one of the following compounds is insoluble in water?

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

What reagent could be used to separate Br^- from NO₃^-when added to an aqueous solution containing both?

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

Identify acetic acid.

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

Determine the oxidation state of Ti in Ti(SO₄)₂.

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

H₂SO₄,H Br,HClO₄,Li₂CO₃,and KIare all classified as

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

Which of the following compounds is NOT an Arrhenius acid?

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)

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Thermochemistry

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

Filters

Exam 9: Introduction to Solutions and Aqueous Reactions

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

Balance the chemical equation given below,and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 40.00 mL of 0.00150 M calcium hydroxide. ________ Ca(OH)2(aq)+ ________ H3PO4(aq)→ ________ Ca3(PO4)2(aq)+ ________ H2O(l)

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

Explain the difference between a strong and weak electrolyte.Give an example of each.

A solution is prepared by adding 1.50 g of solid NaCl to 50.0 mL of 0.100 M .What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.

Which one of the following compounds is insoluble in water?

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

What reagent could be used to separate Br- from N O3- when added to an aqueous solution containing both?

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

Identify acetic acid.

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

Determine the oxidation state of Ti in Ti(SO4)2.

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

H2SO4,H Br ,H ClO4,Li2CO3,and KI are all classified as

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

Which of the following compounds is NOT an Arrhenius acid?

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)

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Thermochemistry

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

Filters

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

Balance the chemical equation given below,and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 40.00 mL of 0.00150 M calcium hydroxide. Ca(OH)₂(aq)+ H₃PO₄(aq)→ Ca₃(PO₄)₂(aq)+ H₂O(l)

What reagent could be used to separate Br^- from NO₃^-when added to an aqueous solution containing both?

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

Determine the oxidation state of Ti in Ti(SO₄)₂.

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

H₂SO₄,H Br,HClO₄,Li₂CO₃,and KIare all classified as

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

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)