Chapter 15a

Question 1

Bronsted-Lowry acid definition

Answer 1

H+ ion donor

Question 2

Bronsted-Lowry base definition

Answer 2

H+ ion acceptor

Question 3

how do strong acids behave in solutions?

Answer 3

completely ionized

Question 4

how do weak acids behave in solutions?

Answer 4

partially ionized

Question 5

characteristics of strong acids

Answer 5

• goes 100% in the forward direction

- K is so large that it is not measured

Question 6

characteristics of weak acids

Answer 6

• can go in reverse direction

- can find/use K value

Question 7

how is Ka affected by the strength of an acid?

Answer 7

stronger acid means higher Ka value

Question 8

what makes something an acid?

Answer 8

something must be on the other side to accept the proton otherwise its not an acid

Question 9

conjugate-acid-base pairs

Answer 9

differ only by a proton (acid loses a proton and turns into a base)

Question 10

what does charge delocalization do to the compound?

Answer 10

makes it more stable

Question 11

what happens when a base gains a proton?

Answer 11

becomes an acid

Question 12

if an acid reacts with water whats the K thing?

Answer 12

Ka

Question 13

whats the K thing when a base reacts with water?

Answer 13

Kb

Question 14

what is the strongest H+ ion that can exist?

Answer 14

H30+

Question 15

are strong acids all the same in water?

Answer 15

ya

Question 16

what are strong acids converted into in water?

Answer 16

H3O

Question 17

how does a strong base affect a conjugate base?

Answer 17

makes the base more stable

Question 18

oxidation number

Answer 18

the greater the number of oxygen atoms, the stronger the acid