Acid + bases

Question 1

What is a bronsted - lowry acid

Answer 1

A proton donor

Question 2

What is a bronsted - lowry base

Answer 2

A proton acceptor

Question 3

How to calculate pH

Answer 3

pH = -log[H+]

Question 4

When calculating pH of a strong acid, what is the assumption made?

Answer 4

That the acid is fully dissociated and acid concentration = H+ concentration

Question 5

How to calculate H+ concentration from given pH

Answer 5

[H+] = 10^-pH

Question 6

Difference between strong and weak acids

Answer 6

Strong acids fully dissociate in water while weak acids partially dissociate

Question 7

Reaction of strong acid with water

Answer 7

HA + H2O –> H3O^+ + A-

Question 8

Reaction of weak acid with water

Answer 8

HA + H2O <–> H3O^+ + A-

Reversible

Question 9

What is the ionic product of water Kw

Answer 9

Kw = [H+][OH-]

Question 10

Modification of Kw for pure water + assumption

Answer 10

Kw = [H+]^2

H+ and OH- concentration are equal as water splits

Question 11

Why is pure water always neutral regardless of pH

Answer 11

H+ concentration = OH- concentration

Question 12

How to calculate pH of a strong base

Answer 12

Assume concentration of base = OH- conc, then use Kw expression

Question 13

Calculate pKa

Answer 13

pKa = -log Ka

Question 14

Calculate Ka from pKa

Answer 14

Ka = 10^-pKa

Question 15

Expression for Ka

Answer 15

Ka = [H+][A-] / [HA]

Question 16

Define buffer solution

Answer 16

A solution that resists change in pH when a small amount of acid or alkali is added

Question 17

Modified expression for Ka during buffer calculations

Answer 17

Ka = [H+] X (salt/acid)

Question 18

h