Acid-Base Equilibrium

Question 1

arrhenius acid theory

Answer 1

acids are substances that yield H+ ions (or H3O+ ions) as the only positive ions in solution

Question 2

arrhenius bases definition

Answer 2

substances that yeild OH- ions as the only negative ion in solution

Question 3

what is the bronsted-lowry definition acids

Answer 3

acids are proton H+ donors

Question 4

what is the bronsted-lowry bases theory?

Answer 4

bases are proton H+ acceptors

Question 5

what is the lewis acid definition

Answer 5

acids are electron pai acceptors

Question 6

what is the lewis bases theory

Answer 6

are electron pair donors

Question 7

conjugate acid

Answer 7

compound formed when a base gains a hydrogen ion

Question 8

conjugate base

Answer 8

compound formed when an acid loses a hydrogen ion

Question 9

strong acid

Answer 9

ionizes 100% in water to form hydronium ions and the anion of the acid

Question 10

weak acid

Answer 10

ionizes less than 50% in water to form hydronium ions and the anion of the acids

Question 11

strong base

Answer 11

metal hydroxides that DISSOCIATE completely in water to form hydroxide and metal ions

Question 12

weak base

Answer 12

substances that react with water to form hydroxide ions and a cation

Question 13

percent ionization

Answer 13

the degree to which a weak acid or base ionizes in water

Question 14

autoionization of water

Answer 14

when water reacts with itself to form H3O+ and OH- ions

Question 15

amphoteric/amphiprotic

Answer 15

substances that can act as an acid in one reaction but as a base in another

Question 16

polyprotic acids

Answer 16

have more than 1 acidic hydrogen

Question 17

neutralization

Answer 17

combining an acid and a base to create a salt and water

Question 18

describe a salt

Answer 18

solid at room temperature composed of cations and anions and arranged in a crystal lattice

Question 19

what happens when a salt dissolves in water

Answer 19

they dissociate into aqueous solutions of ions that may or may not affect the pH of a solution

Question 20

what type of salt form neutral solutions?

Answer 20

cation of a strong base and anion of a strong acid

Question 21

what type of salts form acidic solutions?

Answer 21

• salts where the cation is the conjugate acid of a weak base and the anion of a strong acid
• salts where the cation is a highly charged metal ion and the anion is from a strong acid
• non-metal oxides

Question 22

what type of salts form basic solutions

Answer 22

• salts with the cation of a strong base and the anion of a weak acid
• metal oxides

Question 23

what happens to pH when the cation is the conjugate acid of a weak base and anion is the conjugate base of the weak acid

Answer 23

the pH depends on the Ka of the conjugate acid and the Kb value of the conjugate base

Question 24

describe an acid base titration

Answer 24

a reaction between an acid and base resulting in the production of water and a salt (netutralization)

Question 25

indicator

Answer 25

something that changes colour at the end point

Question 26

end point

Answer 26

the point at which the indicator changes colour

Question 27

equivalence point or stochiometric point

Answer 27

when equal moles of H3O+ and OH- ions have reacted to produce water - neutralization is complete

Question 28

equivalence point pH of stron acid and base

Answer 28

at a pH of 7

Question 29

inflection point

Answer 29

where the equivalence point is on a titration curve - where the curve directoion changes

Question 30

what type of pH and salt is produced with a weak acid and a strong base - where is the equivalence point

Answer 30

produces a basic salt and equivalence point above pH of 7

Question 31

what type of salt does a strong acid and weak base produce and what is the pH of the equivalence point?

Answer 31

produces and acidic salta nd an equivalence point at a pH below 7

Question 32

midpoint of titration

Answer 32

the point at which half of the acid or base has been converted into its conjugate

Question 33

buffers

Answer 33

mixtures of conjugate acid-base pairs that allow a solution to resist changes in pH