LO 47 - 53

Question 1

The [H3O+] in a strong acid solution is ________ the concentration of the strong acid because it __________

Answer 1

equal
completely ionizes

Question 2

Strong acids solutions that are extremely diluted (10^-5 M or less) do NOT _______

Answer 2

completely ionize

Question 3

How can you find the [H3O+] of a weak acid solution?

Answer 3

set up a RICE table using the neutralization reaction, initial concentration of the weak acid, and the Ka value at equilibrium

Question 4

__________ is the ratio of the ionized acid concentration to the initial acid concentration times 100%

Answer 4

percent ionization

Question 5

% ionization = __________

Answer 5

( [H3O+] equil. / [HA] initial ) · 100%

Question 6

The equilibrium [H3O+] of a weak acid ___________ with increasing initial concentration

Answer 6

increases

Question 7

The % ionization of a weak acid _________ with increasing initial concentration

Answer 7

decreases

Question 8

In a mixture of a strong and weak acid, the formation of H3O+ by the strong acid will _________ of additional H3O+ by the weak acid

Answer 8

suppress the formation

Question 9

In mixtures of strong and weak acids, what sources of H3O+ are almost always negligible?

Answer 9

ionization of the weak acid
autoionization of the water

Question 10

In a mixture of two weak acids, how do you determine the pH?

Answer 10

use a RICE table and associated Ka values for each acid to determine the H3O+ ionized from each weak acid.
[H3O+] 1 + [H3O+] 2 = total [H3O+]
-log (total [H3O+]) = pH total

Question 11

Just like strong acids, strong bases ___________ in solution

Answer 11

fully ionize

Question 12

Unlike diprotic acids, bases containing 2 or more OH- ions ___________

Answer 12

dissociate in a single step, NOT one after another

Question 13

the ____________ constant (Kb) quantifies the extent ionization of a weak base

Answer 13

base ionization

Question 14

Kb = __________

Answer 14

[BH+] [OH-] / [B]

Question 15

The smaller the Kb value, the ________ the base

Answer 15

weaker, less basic

Question 16

Most weak bases are _______, which are an ammonia with one or more ______ groups

Answer 16

amines
hydrocarbon

Question 17

Anions in solution tend to form ______ or _______ solutions

Answer 17

basic
neutral

Question 18

Cations in solution tend to form _______ solutions

Answer 18

acidic

Question 19

You can think of dissociated anions as the _______ to their acids

Answer 19

conjugate bases
ex. Cl - as the conjugate base to HCl

Question 20

Anions that are the conjugate to weak acids are themselves _________

Answer 20

weak bases

Question 21

Anions that are the conjugate to strong acids are __________

Answer 21

pH neutral

Question 22

log(Ka) + log(Kb) =
pKa + pKb =
Ka · Kb =

Answer 22

log(Kw)
14
Kw

Question 23

What three categories do dissociated cations typically fall into?

Answer 23

1. counter anions to strong bases
2. conjugate acids to weak bases
3. small, high charged metals

Question 24

In solution, strong bases completely dissociate to form OH- and the solvated __________ which do NOT ionize in water and are this considered _______

Answer 24

counter anion
pH neutral

Question 25

Nonionic **weak** base + (H+) creates the ____________ cation which acts as a ________

Answer 25

conjugate acid weak acid

Question 26

Cations such as Al 3+ and Fe 3+ form _____________ solutions because the hydration of the ion means they act as a __________ acid

Answer 26

weak acid Bronsted-Lowry

Question 27

Summarize the properties of anions

Answer 27

Conjugate bases of acids that generally act as weak bases or are neutral

Question 28

Summarize the properties of cations

Answer 28

Counterions of strong bases, conjugate acids of weak bases, and small highly charged metals

Question 29

The stronger the acid, the ________ the conjugate base

Answer 29

weaker (thus weaker acids make more basic conjugate, and stronger acids a more neutral conjugate)