Assignment 9: Acids and Bases

Question 1

arrhenius acid

Answer 1

a substance that when added to water gives/produces H⁺ ion(s)

• increases [H⁺] in an aqueous solution

Question 2

arrhenius base

Answer 2

a substance that when added to water gives/produces OH^- ion(s)

• increases [OH^-] in an aqueous solution

Question 3

definition

strong acid/base

Answer 3

a substance that dissociates completely (all HCl turns into H⁺ and Cl^-)

Question 4

definition

weak acid/base

Answer 4

a substance that doesn’t dissociate completely (there is a reverse reacton at equilibrium, so the ions are turned back into an acid/base)

Question 5

k_eq for water = k_w

Answer 5

k_w = [H⁺][OH^-] = 10^-14

k_w = (k_a)(k_b)

Question 6

pH

Answer 6

-log[H⁺]

Question 7

pOH

Answer 7

-log[OH^-]

Question 8

pk_w

Answer 8

= -logk_w

= -log([H⁺][OH^-]} = -log[H⁺] + -log[OH^-]

= pH + pOH

= 14

Question 9

examples

strong acid

Answer 9

HCl, H₂SO₄, HNO₃

Question 10

Brønsted-Lowry Definition

Answer 10

acid: gives a proton (H⁺)
base: accepts/receives/takes a proton (H⁺)

Question 11

neutralization reaction

Answer 11

reaction between an acid and a base

Question 12

examples

strong bases

Answer 12

IA, KOH, NaOH

Question 13

examples

weak acids

Answer 13

HAc(HC₂H₃O₂), NH₄⁺

Question 14

examples

weak bases

Answer 14

NH₃, Ac^-

Question 15

buffer

Answer 15

a combination of a weak acid and it’s conjugate base in roughly equal proportions, so that any added strong acid or base can be neutralized by the available weak acid or base without the pH changing very much ([H⁺] is very close to K_a)

Question 16

k_sp = [A][B]

Answer 16

equilibrium

Question 17

k_sp < [A][B]

Answer 17

precipitate forms

Question 18

k_sp > [A][B]

Answer 18

no precipitate forms (just ions)

Question 19

k_sp

Answer 19

= [prod]

• the k_eq of a saturated solution at equilibrium where the reactants are solids

Question 20

saturated solution

Answer 20

solution with maxium amount of solute, such that if any more solute was added, it wouldn’t dissolve

Question 21

conjugate acid/base pair

Answer 21

a pair of an acid and a base that differ only by an H⁺ and OH^-

Question 22

relative strength/size of conjugate acid/base pairs

Answer 22

strong/very large acid —> very weak/very small base

weak/large acid —> weak/small base

weak/small acid —> weak/large base

very weak/very small —> strong/very large base

Question 23

[H⁺] = k_a

Answer 23

pH = pk_a

[HIn] = [In^-]

mixed color

Question 24

[H⁺] > k_a

Answer 24

pH < pk_a

[HIn] > [In^-]

color of acid (HIn)

(if [HIn]:[In^-] is 10:1, then pH = pk_a - 1)

Question 25

[H⁺] < k_a

Answer 25

pH > pk_a

[HIn] < [In^-]

color of base (In^-)

(if [HIn]:[In-] is 1:10, then pH = pka + 1)

Question 26

equilibrium

Answer 26

k_sp = [A][B]

Question 27

precipitate forms

Answer 27

k_sp < [A][B]

Question 28

no precipitate forms (just ions)

Answer 28

k_sp > [A][B]

Question 29

NH₄⁺¹

Answer 29

ammonium

Question 30

OH^-1

Answer 30

hydroxide

Question 31

CO₃^-2

Answer 31

carbonate

Question 32

PO₄^-3

Answer 32

phosphate

Question 33

SO₄^-2

Answer 33

sulfate

Question 34

NO₃^-1

Answer 34

nitrate

Question 35

C₂H₃O₂^-1

Answer 35

acetate

Question 36

ammonium

Answer 36

NH₄⁺¹

Question 37

hydroxide

Answer 37

OH^-1

Question 38

carbonate

Answer 38

CO₃^-2

Question 39

phosphate

Answer 39

PO₄^-3

Question 40

sulfate

Answer 40

SO₄^-2

Question 41

nitrate

Answer 41

NO₃^-1

Question 42

acetate

Answer 42

C₂H₃O₂^-1