The oxidation number of Mn in KMnO4 is

A) +8. B) +7. C) +5. D) -7. E) -8. A) +8. B) +7. C) +5. D) -7. E) -8.

The oxidation number of Cl in ClO4- is

A) -1. B) +1. C) +3. D) +5. E) None of the above. A) -1. B) +1. C) +3. D) +5. E) None of the above.

In the following chemical reaction the oxidizing agent is: 5S + 6KNO3 + 2CaCO3 $\rarr$3K2SO4 + 2CaSO4 + CO2 + 3N2

A) S B) N2 C) KNO3 D) CaSO4 E) CaCO3 A) S B) N2 C) KNO3 D) CaSO4 E) CaCO3

Exam 4: Reactions in Aqueous Solution

Based on the solubility rules, which of the following will occur when a solution containing about 0.1 g of Pb(NO₃)₂(aq)is mixed with a solution containing 0.1 g of KI(aq)/100 mL?

Free

(Multiple Choice)

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Question 1

Correct Answer:

Verified

What mass of Li₃PO₄ is needed to prepare 500. mL of a solution having a lithium ion concentration of 0.175 M?

Free

(Multiple Choice)

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Question 2

Correct Answer:

Verified

Determine the oxidation number of each of the elements in K₂TaF₇?

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(Essay)

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Question 3

Correct Answer:

Verified

the oxidation number of K is +1; the oxidation number of Ta is +5; the oxidation number of F is -1

If 145 grams of potassium nitrate were added to water to make 1,500 mL of solution, what would be the molarity of the resulting solution?

(Short Answer)

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Question 4

The following equation is an example of a net ionic equation. Na⁺(aq)+ Br^-(aq)+ Ag⁺(aq)+ NO₃^-(aq) $\rarr$ AgBr(s)+ Na⁺(aq)+ NO₃^-(aq)

(True/False)

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Question 5

A 4.691 g sample of MgCl₂ is dissolved in enough water to give 750. mL of solution. What is the magnesium ion concentration in this solution?

(Multiple Choice)

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Question 6

The following experiments were carried out and observations recorded. Expt. #1: copper metal was added to an aqueous solution of silver nitrate Observation: The copper become coated with a substance. Expt. #2: lead metal was added to an aqueous solution of copper(II)nitrate Observation: The lead turned black and crumbled. Expt. #3: zinc metal was added to an aqueous solution of lead(II)nitrate Observation: The zinc appeared to fall apart. Rank the metals from most active to least active.

(Essay)

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Question 7

Which of the following compounds is a strong electrolyte?

(Multiple Choice)

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Question 8

The oxidation number of Mn in KMnO₄ is

(Multiple Choice)

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Question 9

Give an example of a diprotic acid.

(Short Answer)

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Question 10

Identify the following as either a good or poor conductor of electricity: an aqueous solution of Na₂SO₄.

(Short Answer)

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Question 11

The oxidation number of Cl in ClO₄^- is

(Multiple Choice)

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Question 12

What mass of Na₂SO₄ is needed to prepare 350. mL of a solution having a sodium ion concentration of 0.125 M?

(Multiple Choice)

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Question 13

In the following chemical reaction the oxidizing agent is: 5S + 6KNO₃ + 2CaCO₃ $\rarr$ 3K₂SO₄ + 2CaSO₄ + CO₂ + 3N₂

(Multiple Choice)

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Question 14

Name and give the formulas for six strong acids.

(Essay)

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Question 15

The distinguishing characteristic of all electrolyte solutions is that they

(Multiple Choice)

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Question 16

What is the molar concentration of chloride ions in a solution prepared by mixing 100. mL of 2.0 M KCl with 50. mL of a 1.5 M CaCl₂ solution?

(Short Answer)

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Question 17

Which of the following is an example of a disproportionation reaction?

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Question 18

Define and illustrate with an example the difference between an electrolyte and a nonelectrolyte.

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Question 19

Which of the following represents a precipitation reaction?

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Question 20

Showing 1 - 20 of 156

Exam 4: Reactions in Aqueous Solution

Based on the solubility rules, which of the following will occur when a solution containing about 0.1 g of Pb(NO3)2(aq)is mixed with a solution containing 0.1 g of KI(aq)/100 mL?

What mass of Li3PO4 is needed to prepare 500. mL of a solution having a lithium ion concentration of 0.175 M?

Determine the oxidation number of each of the elements in K2TaF7?

If 145 grams of potassium nitrate were added to water to make 1,500 mL of solution, what would be the molarity of the resulting solution?

The following equation is an example of a net ionic equation. Na+(aq)+ Br-(aq)+ Ag+(aq)+ NO3-(aq) →\rarr→ AgBr(s)+ Na+(aq)+ NO3-(aq)

A 4.691 g sample of MgCl2 is dissolved in enough water to give 750. mL of solution. What is the magnesium ion concentration in this solution?

Which of the following compounds is a strong electrolyte?

The oxidation number of Mn in KMnO4 is

Give an example of a diprotic acid.

Identify the following as either a good or poor conductor of electricity: an aqueous solution of Na2SO4.

The oxidation number of Cl in ClO4- is

What mass of Na2SO4 is needed to prepare 350. mL of a solution having a sodium ion concentration of 0.125 M?

In the following chemical reaction the oxidizing agent is: 5S + 6KNO3 + 2CaCO3 →\rarr→ 3K2SO4 + 2CaSO4 + CO2 + 3N2

Name and give the formulas for six strong acids.

The distinguishing characteristic of all electrolyte solutions is that they

What is the molar concentration of chloride ions in a solution prepared by mixing 100. mL of 2.0 M KCl with 50. mL of a 1.5 M CaCl2 solution?

Which of the following is an example of a disproportionation reaction?

Define and illustrate with an example the difference between an electrolyte and a nonelectrolyte.

Which of the following represents a precipitation reaction?

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Based on the solubility rules, which of the following will occur when a solution containing about 0.1 g of Pb(NO₃)₂(aq)is mixed with a solution containing 0.1 g of KI(aq)/100 mL?

What mass of Li₃PO₄ is needed to prepare 500. mL of a solution having a lithium ion concentration of 0.175 M?

Determine the oxidation number of each of the elements in K₂TaF₇?

The following equation is an example of a net ionic equation. Na⁺(aq)+ Br^-(aq)+ Ag⁺(aq)+ NO₃^-(aq) $\rarr$ AgBr(s)+ Na⁺(aq)+ NO₃^-(aq)

A 4.691 g sample of MgCl₂ is dissolved in enough water to give 750. mL of solution. What is the magnesium ion concentration in this solution?

The oxidation number of Mn in KMnO₄ is

Identify the following as either a good or poor conductor of electricity: an aqueous solution of Na₂SO₄.

The oxidation number of Cl in ClO₄^- is

What mass of Na₂SO₄ is needed to prepare 350. mL of a solution having a sodium ion concentration of 0.125 M?

In the following chemical reaction the oxidizing agent is: 5S + 6KNO₃ + 2CaCO₃ $\rarr$ 3K₂SO₄ + 2CaSO₄ + CO₂ + 3N₂

What is the molar concentration of chloride ions in a solution prepared by mixing 100. mL of 2.0 M KCl with 50. mL of a 1.5 M CaCl₂ solution?