Chapter 4: Types of Chemical Reactions and Solution Stoichiometry

Question 1

Solvent

Answer 1

Dissolving medium

Question 2

Aqueous solution

Answer 2

A solution in which water is the dissolving medium or solvent

Question 3

Polar molecule

Answer 3

A molecule that has a permanent dipole moment

Question 4

Hydration

Answer 4

The interaction between solute particles and water molecules

Question 5

Solubility

Answer 5

The amount of a substance that dissolves in a given volume of solvent at a given temperature

Question 6

Solute

Answer 6

A substance dissolved in a liquid to form a solution

Question 7

Electrical conductivity

Answer 7

The ability to conduct an electric current

Question 8

Strong electrolyte

Answer 8

A material that, when dissolved in water, gives a solution that conducts an electric current very efficiently (completely ionized)

Question 9

Weak electrolyte

Answer 9

A material that, when dissolved in water, gives a solution that conducts only a small electric current (produces relatively few ions)

Question 10

Nonelectrolyte

Answer 10

A substance that, when dissolved in water, gives a nonconducting solution (produces no ions)

Question 11

Classes of strong electrolytes

Answer 11

1. Soluble salts
2. Strong acids
3. Strong bases

Question 12

Acid

Answer 12

A substance that produce H+ ions (protons) when it is dissolved in water (PROTON DONOR)

Question 13

Strong acid

Answer 13

An acid that completely dissociates to produces an H+ ion and the conjugate base (HCl, HF, HBr, HNO3, H2SO4, HClO4) (PROTON ACCEPTOR)

Question 14

Strong base

Answer 14

A metal hydroxide salt that completely dissociates into its ions in water (LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2)

Question 15

Weak acid

Answer 15

An acid that dissociates only slightly in aqueous solution

Question 16

Weak base

Answer 16

A base that reacts with water to produce hydroxide ions to only a slight extent in aqueous solution

Question 17

Molarity

Answer 17

Moles of solute per volume of solution in liters

Question 18

Standard solution

Answer 18

A solution whose concentration is accurately known

Question 19

Dilution

Answer 19

The process of adding solvent to lower the concentration of solute in a solution (M1V1 = M2V2)

Question 20

Three main types of solution reactions

Answer 20

1. Precipitation reactions
2. Acid-base reactions
3. Oxidation-reduction reactions

Question 21

Precipitation reaction

Answer 21

A reaction in which an insoluble substance forms and separates from the solution

Question 22

Precipitate

Answer 22

The solid that forms from a precipitation reaction

Question 23

Formula equation

Answer 23

An equation representing a reaction in solution showing the reactants and products in undissociated form ,whether they are strong or weak electrolytes

Question 24

Complete ionic equation

Answer 24

An equation that shows al substances that are strong electrolytes as ions

Question 25

Net ionic equation

Answer 25

An equation for a reaction in solution, where strong electrolytes are written as ions, showing only those components that are directly involved in the chemical change

Question 26

Steps for solving stoichiometry problems for reactions in solution

Answer 26

1. Identify the species present in the combined solution, and determine what reaction occurs
2. Write the balanced net ionic equation for the reaction
3. Calculate the moles of reactants
4. Determine which reactant is limiting
5. Calculate the moles of product or products, as required
6. Convert to grams or other units, as required

Question 27

Neutralization reaction

Answer 27

An acid-base reaction

Question 28

Steps for performing calculations for acid-base reactions

Answer 28

1. List the species present in the combined solution before any reaction occurs, and decide what reaction will occur
2. Write the balanced net ionic equation for this reaction
3. Calculate the moles of reactants. For reactions in solution, use the volumes of the original solutions and their molarities
4. Determine the limiting reactant where appropriate
5. Calculate the moles of the required reactant or product
6. Convert to grams or volume (of solution), as required

Question 29

Volumetric analysis

Answer 29

A technique for determining the amount of a certain substance by doing a titration

Question 30

Titration

Answer 30

A technique in which one solution is used to analyze another, involving delivery (from a buret) of a measured volume of a solution of known concentration (the titrant) into a solution containing the substance being analyzed (the analyte)

Question 31

Equivalence point/stoichiometric point

Answer 31

The point in the titration where enought titrant has been added to react exactly with the analyte

Question 32

Indicator

Answer 32

A substance added at the beginning of the titration that changes color at (or very near) the equivalence point

Question 33

Endpoint

Answer 33

The point where the indicator actually changes color =

Question 34

Oxidation-reduction reactions

Answer 34

Reactions in which one or more electrons are transferred

Question 35

Oxidation states

Answer 35

A concept that provides a way to keep track of electrons in oxidation-reduction reactions according to certain rules

Question 36

Oxidation

Answer 36

An increase in oxidation state (a loss of electrons)

Question 37

Reduction

Answer 37

A decrease in oxidation state (a gain of electrons)

Question 38

Oxidizing agent

Answer 38

Electron acceptor

Question 39

Reducing agent

Answer 39

Electron donor

Question 40

Steps for balancing oxidation-reduction reactions by oxidation states

Answer 40

1. Write the unbalanced equation
2. Determine the oxidation states of all atoms in the reactants and products
3. Show electrons gained and lost using “tie lines.”
4. Use coefficients to equalize the electrons gained and lost
5. Balance the rest of the equation by inspection
6. Add appropriate states