Section 3 Week 1: Acid-Base Equilibrium

Question 1

What is an Acid?

Answer 1

Proton (H+) donor

Question 2

What is a Base?

Answer 2

Proton (H+) acceptor

Question 3

What does an Arrhenius base have?

Answer 3

OH

Question 4

What does a Bronstead Lowry acid have to have?

Answer 4

Must contain H in its formula

Question 5

What does a Bronstead Lowry base have to have?

Answer 5

Must contain a lone pair of electrons to bond to H+

Question 6

What process is an Acid Base reaction?

Answer 6

Proton-transfer process

Question 7

In Lowry-Bronstead, what does the reactants and products both need?

Answer 7

An acid and base with their conjugate base and acid

Question 8

What is acid ionization?

Answer 8

Proton exchange between an acid and water

Question 9

What is water in this case?

Answer 9

Amphiprotic

Question 10

What does Amphiprotic mean?

Answer 10

Can react with either an acid or a base

Question 11

What is base ionization?

Answer 11

Proton exchange reaction between a base and water

Question 12

Weak or strong acid reversible?

Answer 12

Weak

Question 13

Conjugate Acid/Base Pairs

Answer 13

Differ by H+

Question 14

What is the equilibrium constant called?

Answer 14

Kw

Question 15

In an Acidic solution:

Answer 15

H3O+ > OH-

Question 16

In a neutral solution:

Answer 16

H3O+ = OH-

Question 17

In a basic solution:

Answer 17

H3O+ < OH-

Question 18

Autoionization of Water: Kw = [H3O+][OH-] = ? At what temperature

Answer 18

1.00 x 10^-14 at 25c

Question 19

Which ions are present in aqueous solutions?

Answer 19

H3O+ and OH-

Question 20

pH + pOH = ?

Answer 20

14

Question 21

Logab = ?

Answer 21

Logab = log a + log b

Question 22

Higher the ___ , the lower the ____ and the _____ the solution.

Answer 22

pH, [H3O+], less acidic

Question 23

In an acidic solution:

Answer 23

pH < 7.00

Question 24

In a neural solution:

Answer 24

pH = 7.00

Question 25

In a basic solution:

Answer 25

pH > 7.00

Question 26

Since kw is ___, the values of pH, pOH, H3O+ and OH- are interrelated:

Answer 26

If H3O+ increases, OH- decreases and vice versa If pH increases, pOH decreases and vice versa

Question 27

K>>1 implies what

Answer 27

The forward reaction is favourable, which means HA wants to donate, B wants to accept

Question 28

Ka

Answer 28

Products/reactants

Question 29

What is Ka?

Answer 29

Acid dissociation constant

Question 30

When is Ka irrelevant?

Answer 30

For strong acids because there is no equilibria

Question 31

___ strong acids are equally strong in ____

Answer 31

All, water

Question 32

Strong acid we can expect the value to be what?

Answer 32

Ka > 1

Question 33

Stronger acid = ___ Ka

Answer 33

Larger

Question 34

Weaker acid = ____ Ka

Answer 34

Smaller