Chapter 8: Solutions & Aqueous Reactions

Question 1

What is the formula for naming binary acids?

Answer 1

Binary acids are composed of hydrogen and a nonmetal. Names for binary acids have the form:
hydro + base name of nonmetal + ic acid.

Question 2

What is the formula for naming oxyacids?

Answer 2

Oxyacids contain hydrogen and an oxyanion (an anion containing a nonmetal and oxygen). For oxyanions ending with “ate,” the formula is base name of oxyanion + ic + acid.
For oxyanions ending with “ite” is base name of oxyanion + ous + acid.

Question 3

Define molecular equation.

Answer 3

A molecular equation is an equation that shows the complete neutral formulas for each compound in the reaction as if they existed as molecules. In actual solutions of soluble ionic compounds, dissolved substances are present as ions.

Question 4

Define complete ionic equations.

Answer 4

Complete ionic equations are equations that list all of the ions present as either reactants or products in a chemical reaction. It accounts for the fact that some ionic compounds are soluble and exist as individual ions in an aqueous solution.

Question 5

Define net ionic equations.

Answer 5

Net ionic equations are equations that show only the species that actually change during the reaction. To write these equations, the spectator ions must be removed.

Question 6

Give the Arrhenius definition of an acid.

Answer 6

An acid is a molecular compound that releases hydrogen ions (H+) when dissolved in water.

Question 7

Define polyprotic acids.

Answer 7

These are acids that contain more than one ionizable proton and release them sequentially.

Question 8

Give the Arrhenius definition of a base.

Answer 8

A base is a molecular compound that produces OH- in solution.

Question 9

What happens when an acid and a base mix?

Answer 9

The H+ from the acid combines with the OH- from the base to form H2O.

Question 10

Define oxidation-reduction (redox) reactions.

Answer 10

Redox reactions are reactions in which electrons transfer from one reactant to the other. These types of reactions occur both in and out of solution.

Question 11

What is the oxidation state/oxidation number?

Answer 11

The oxidation number of an atom in a compound is the “charge” it would have if all shared electrons were assigned to the more electronegative atom.

Question 12

How are oxidation and reduction defined in terms of oxidation states?

Answer 12

Oxidation: an increase in oxidation state
Reduction: a decrease in oxidation state

Question 13

Define oxidizing agent.

Answer 13

An oxidizing agent is a substance that causes the oxidation of another substance. In a redox reaction, the oxidizing agent is always reduced.

Question 14

Define reducing agent.

Answer 14

A reducing agent is a substance that causes the reduction of another substance. In a redox reaction, the reducing agent is always oxidized.

Question 15

What does the activity series of metals show?

Answer 15

This table lists metals in order of decreasing tendency to lose electrons. The metals at the top of the list have the greatest tendency to lose electrons–they are most easily oxidized and therefore the most reactive. The metals at the bottom of the list have the lowest tendency to lose electrons–they are the most difficult to oxidize and therefore the least reactive.

Question 16

When extra solvent is added to a concentration solution, what happens to the concentration of the solute and the moles of the solute?

Answer 16

The concentration of the solute decreases, but moles stay the same. When a dilution is made, initial moles must equal final moles.

Question 17

What two classes can solutes be separated into, and what makes them different from each other?

Answer 17

Electrolyte: solute breaks apart into constituent ions.
Nonelectrolyte: solute breaks apart into separate, uncharged molecules.

Question 18

Describe the process of dissolution for an ionic compound.

Answer 18

When dissolved, ionic compounds dissociate into constituent ions. Ions are kept from reforming a crystal lattice by the solvent forming an ion sphere around it.

Question 19

Define ion sphere.

Answer 19

An ion sphere is an octahedral arrangement of 6 solvent molecules oriented with opposing charge facing the ion.

Question 20

Describe the process of dissolution for molecular compounds.

Answer 20

When dissolved, molecular compounds do not dissociate (there are no intramolecular bonds broken).

Question 21

What is the exception to the molecular compound rule for dissolution?

Answer 21

Most molecular compounds, when dissolved, do not dissociate. However, the exception to this rule are the acids.

Question 22

Define acids.

Answer 22

Acids are molecular compounds that ionize when dissolved in water to form hydronium (H3O+) and a conjugate base, A-. Acids may be either strong (about 100% ionization) or weak (<100% ionization).

Question 23

What are the seven strong acids?

Answer 23

HCl, HBr, HI, HClO3, HClO4, HNO3, and H2SO4. (for the first ionization).

Question 24

In a titration, where does the endpoint occur in relation to the equivalence point?

Answer 24

The endpoint always occurs after the equivalence point.

Question 25

In general, O has an oxidation state of -2. What are the two exceptions to this?

Answer 25

In peroxide (O2 2-), the oxidation state is -1. In superoxide (O2 -), the oxidation state is -1/2.