Chapter 10

Question 1

Arrhenius definitions

Answer 1

dissociate

acid has excess H
Base has excess OH in solution

Question 2

Bronsted Lowry

Answer 2

Acid donates H- includes water
base accepts H

not limited to aq

Question 3

Lewis

Answer 3

most inclusive

acid is electron pair acceptor, base is donator

Question 4

amphoteric

Answer 4

acid or base depending on environment

common in polyvalent, amino acids, and water

Question 5

amphiprotic

Answer 5

can gain or lose protons

Question 6

acid anion

Answer 6

-ide to hydro-ic acid

Question 7

acid oxyanion

Answer 7

-ite to -ous acid
-ate to -ic acid

Question 8

autoionization

Answer 8

water reacts with self and is reversible

forms H3O+ and OH-

Question 9

Kw

Answer 9

[H3O+] [OH-] = 10^-14 at 25C

concentrations are 10^-7 when neutral

Question 10

pH

Answer 10

-log [H+]= log 1/H+

Question 11

pOH

Answer 11

-log [OH-]

pH+pOH= 14

Question 12

how to calculate log with
-log (n x10^-m)

Answer 12

= m-log n

n is between 0 and 10, so log is between 0 and 1

= m=0.n

Question 13

Ka and Kb

Answer 13

Smaller ka is weaker acid

ka= [H3o+] [A-]/ [HA]
Kb= [OH-] [B+] / [BOH]

weal base/acid has k<1

Question 14

conjugate acid

Answer 14

base gains protons

kb x ka acid =kw

Question 15

conjugate base

Answer 15

acid loses protons

ka x kb conjugate = kw

large Ka will have small Kb

Question 16

How does EN affect acidity

Answer 16

they withdraw electrons to weaken bonds and increase acidity