Acids and Bases

Question 1

Acidic Solution

Answer 1

Contains more hydrogen ions than hydroxide ions.

Question 2

Basic Solution

Answer 2

Contains more hydroxide ions than hydrogen ions.

Question 3

Arrhenius model

Answer 3

A model of acids and bases; states that an acid is a substance that contains hydrogen and ionizes to produce hydrogen ions in aqueous solution and a base is a substance that contains a hydroxide group and dissociates to produce a hydroxide ion in aqueous solution.

Question 4

Bronsted-Lowry model

Answer 4

A model of acids and bases in which an acid is a hydrogen-ion donor and a base is a hydrogen-ion acceptor.

Question 5

Conjugated acid

Answer 5

The species produced when a base accepts a hydrogen ion from an acid

Question 6

Conjugated base

Answer 6

The species produced when an acid donates a hydrogen ion to a base

Question 7

Conjugated acid-base pair

Answer 7

Consists of two substances related to each other by the donating and accepting of a single hydrogen ion.

Question 8

Amphoteric

Answer 8

Describes water and other substances that can act as both acids and bases.

Question 9

Lewis model

Answer 9

A Lewis acid is an electron-pair acceptor and a Lewis base is an electron-pair donor.

Question 10

Electrolyte

Answer 10

An ionic compound whose aqueous solution conducts an electric current.

Question 11

Strong acid

Answer 11

an acid that ionizes completely in aqueous solution.

Question 12

Weak acid

Answer 12

An acid that ionizes only partially in dilute aqueous solution

Question 13

Acid ionization constant

Answer 13

The value of the equilibrium constant expression for the ionization of a weak acid.

Question 14

Strong base

Answer 14

A base that dissociates entirely into metal ions and hydroxide ions in aqueous solution

Question 15

Weak base

Answer 15

A base that ionizes only partially in dilute aqueous solution to form the conjugate acid of the base and hydroxide ion

Question 16

Base ionization constant

Answer 16

The value of the equilibrium constant expression for the ionization of a base.

Question 17

Le Chatelier’s principle

Answer 17

States that if a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress.

Question 18

pH

Answer 18

The negative logarithm of the hydrogen ion concentration of a solution ; acidic solutions have a pH values between 0-7, basic solutions have values between 7-14, and a solution with a pH of 7.0 is neutral.

Question 19

pOH

Answer 19

The negative logarithm of the hydroxide ion concentration of a solution; a solution with a pOH below 7.0 is basic and a solution with a pOH of 7.0 is neutral

Question 20

Ion product constant for water

Answer 20

The value of the equilibrium constant expression for the self-ionization of water.

Question 21

Neutralization reaction

Answer 21

A reaction in which an acid and a base react in aqueous solution to produce a salt and water.

Question 22

Salt

Answer 22

An ionic compound made up of a cation from a base and an anion from an acid

Question 23

Titration

Answer 23

The process in which an acid-base neutralization reaction is used to determine the concentration of a solution of unknown concentration

Question 24

Titrant

Answer 24

A solution of known concentration used to titrate a solution of unknown concentration; also called the standard solution.

Question 25

Equivalance point

Answer 25

The point at which the moles of H+ ions from the acid equals moles of OH- ions from the base.

Question 26

Acid-base indicator

Answer 26

A chemical dye whose color is affected by acidic and basic solutions.

Question 27

End point

Answer 27

The point at which the indicator that is used in a titration changes color.

Question 28

Salt hydrolysis

Answer 28

The process in which anions of the dissociated salt accept hydrogen ions from water, or the cations of the dissociated salt donate hydrogen ions to water.

Question 29

Buffer

Answer 29

A solution that resists changes in pH when limited amounts of acid or base are added

Question 30

Buffer capacity

Answer 30

The amount of acid or base a buffer solution can absorb without a significant change in pH.

Question 31

Who introduced the Arrhenius model

Answer 31

The one to introduce this model was Svante Arrhenius, in 1883 he proposed this model of acids and bases.

Question 32

Who made The Bronsted-Lowry model

Answer 32

Danish chemist Johannes Bronsted and English chemist Thomas Lowry proposed a more inclusive model of acids and bases - a model that focuses on the hydrogen ion (H+)

Question 33

What is the pH scale?

Answer 33

The pH scale is the negative logarithm of the hydrogen ion concentration of a solution ; acidic solutions have a pH values between 0-7, basic solutions have values between 7-14, and a solution with a pH of 7.0 is neutral.

Question 34

What is the formula for pH

Answer 34

pH = -log[H+]

Question 35

What is the formula for pOH

Answer 35

pOH = -log[OH-]

Question 36

How are pH and pOH related

Answer 36

pH + pOH = 14.00

Question 37

If they give you pH, how do you calculate the concentration?

Answer 37

[H+] = 10^-pH

Question 38

What is the formula for Ion product constant of water

Answer 38

Kw = [H+] [OH-]