Chapter 9: Introduction to Solutions & Aqueous Reactions

Question 1

Aqueous Solutions

Answer 1

Solutions in which water acts as the solvent.

Question 2

Solution

Answer 2

A homogenous mixture of two substances.

Question 3

Solvent

Answer 3

The majority component of a solution.

Question 4

Solute

Answer 4

The minority component of a solution.

Question 5

Dilute Solution

Answer 5

A solution that contains a very small amount of solute relative to the amount of solvent.

Question 6

Concentrated Solution

Answer 6

A solution that contains a very large amount of solute relative to the amount of solvent.

Question 7

Molarity (M)

Answer 7

A means of expressing solution concentration as the number of moles of solute per liter of solution.
M = amount of solute (mol)/volume of solution (L)

Question 8

Stock Solution

Answer 8

A highly concentrated form of a solution used in laboratories to make less concentrated solution via dilution.

Question 9

Dilution Equation

Answer 9

M1V1=M2V2
M1 = initial molarity of concentrated solution
V1 = initial volume of concentrated solution
M2 = molarity of final diluted solution
V2 = volume of final diluted solution

Question 10

Solution Stoichiometry

Answer 10

The volume and concentration of a reactant or product can be used to calculate its amount in moles. Then the stoichiometric coefficients in the chemical equation to convert the amount in moles of another reactant or product.

Question 11

Conceptual Plan of Solution Stoichiometry

Answer 11

Volume A –> Amount A (moles) —> Amount B (moles) —> Volume B

Question 12

Electrolyte

Answer 12

A substance that dissolves in water to form solutions that conduct electricity.

Question 13

Strong Electrolyte

Answer 13

A substance that completely dissociates into ions when dissolved in water.

Question 14

Nonelectrolyte

Answer 14

A compound that does not dissociate into ions when dissolved in water. It creates solutions called nonelectrolyte solutions that do not conduct electricity. Most molecular compounds (except acids) dissolve in water as intact molecules.

Question 15

Nonelectrolyte Solutions

Answer 15

Solutions that do not conduct electricity.

Question 16

Acids

Answer 16

Molecular compounds that ionize to form H+ ions when they dissolve in water.

Question 17

Strong Acid

Answer 17

An acid that completely ionizes in a solution.

- They are also strong electrolytes since they completely ionize in a solution

Question 18

Chemical Equation of a Strong Acid

Answer 18

Represent the complete ionization of a strong acid with a reaction arrow between the acid and its ionized form:
HCl (aq) –> H+ (aq) + Cl- (aq)

Question 19

Weak Acid

Answer 19

An acid that does not completely ionize in water. Are classified as weak electrolytes.

Question 20

Chemical Equation of a Weak Acid

Answer 20

Represent the partial ionization of a weak acid with opposing half arrows between the reactant and product:
HC2H3O2 (aq) H+ (aq) + C2H3O2- (aq)

Question 21

Weak Electrolyte Solutions

Answer 21

The resulting solution of a weak acid.

Question 22

Weak Electrolyte

Answer 22

A substance that does not completely ionize in the water and only weakly conducts electricity in solution.

Question 23

Soluble

Answer 23

Describes a compound that is able to dissolve to a significant extent, usually in water.

Question 24

Insoluble

Answer 24

Describes a compound that is incapable of dissolving in water or extremely difficult to dissolve in water.

Question 25

Solubility of a Compound Containing L+

Answer 25

Soluble

Question 26

Solubility of a Compound Containing Na+

Answer 26

Soluble

Question 27

Solubility of a Compound Containing K+

Answer 27

Soluble

Question 28

Solubility of a Compound Containing NH4+

Answer 28

Soluble

Question 29

Solubility of a Compound Containing NO3-

Answer 29

Soluble

Question 30

Solubility of a Compound Containing C2H3O2-

Answer 30

Soluble

Question 31

Solubility of a Compound Containing Cl-

Answer 31

Soluble unless paired with Ag+, H2+2, or Pb2+.

Question 32

Solubility of a Compound Containing Br-

Answer 32

Soluble unless paired with Ag+, H2+2, or Pb2+.

Question 33

Solubility of a Compound Containing I-

Answer 33

Soluble unless paired with Ag+, H2+2, or Pb2+.

Question 34

Solubility of a Compound Containing SO42-

Answer 34

Soluble unless paired with Sr2+, Ba2+, Pb2+, Ag+, or Ca2+.

Question 35

Solubility of a Compound Containing OH-

Answer 35

Insoluble unless paired with Li+, Na+, K+, or NH4+. When paired with Ca2+, Sr2+, or Ba2+, the resulting compound is slightly soluble.

Question 36

Solubility of a Compound Containing S2-

Answer 36

Insoluble unless paired with Li+, Na+, K+, or NH4+, Ca2+, Sr2+, or Ba2+.

Question 37

Solubility of a Compound Containing CO32-

Answer 37

Insoluble unless paired with Li+, Na+, K+, or NH4+.

Question 38

Solubility of a Compound Containing PO43-

Answer 38

Insoluble unless paired with Li+, Na+, K+, or NH4+.

Question 39

Precipitation Reaction

Answer 39

A reaction in which a solid, insoluble product forms upon mixing two solutions.

Question 40

Precipitate

Answer 40

A solid, insoluble ionic compound that forms in, and separate from, a solution. - Only insoluble compounds form precipitates - If the possible products are both soluble, no reaction occurs and no precipitate forms - if one or both of the possible products are insoluble, a precipitation reaction occurs.

Question 41

Molecular Equation

Answer 41

A chemical equation showing the complete neutral formula for each compound in the reaction.

Question 42

Complete Ionic Equation

Answer 42

A chemical equation that lists individually all of the ions present as either reactants or products in a chemical reaction.

Question 43

Spectator Ion

Answer 43

An ion in a complete ionic equation that does not participate in the reaction and therefore remains in the solution. Spectator ions are emitted from the equation.

Question 44

Acid-Base Reactions (Neutralization Reactions)

Answer 44

An acid reacts with a base and the two neutralize each other, producing water or in some cases a weak electrolyte.