Acids and bases (incomplete)

Question 1

What is the Bronsted- Lowry definition for an acid?

Answer 1

Proton donor.

Question 2

What is the Bronsted- Lowry definition for a base?

Answer 2

Proton acceptor

Question 3

What is the PH scale?

Answer 3

The PH scale is a logarithmic scale based on the concentration of H+ ions

Question 4

What do square brackets [ ] represent

Answer 4

Square brackets represent concentrations.

Question 5

What are the equations relating PH and H+ concentration?

Answer 5

pH = -log[H+]

[H+] = 10^-pH

Question 6

What is the Kw equation?

Answer 6

Kw = [H+][OH-]

Question 7

What is the value of Kw at 298k

Answer 7

1x10^-14

Question 8

Tell me about the equilibrium positions of weak and strong acid and base reactions.

Answer 8

Strong acid/base reactions have an equilibrium extremely far to the right, because of this they can be treated as a one way reaction.

Weak acid/base reactions have an equilibrium point extremely far to the left and are treated as reversible reactions.

Question 9

Examples of strong acids/bases?

Answer 9

HCl
NaOH

Question 10

Examples of weak acids/bases

Answer 10

Organic acid like ethanoic acid
citric acid
ammonia

Question 11

Definition of strong acids/bases?

Answer 11

Strong acids/bases ionise almost completely in water.

Question 12

Definition of weak acids/bases?

Answer 12

Weak acids/bases partially ionise in water.

Question 13

How does water react when an acid is added?

Answer 13

Water acts as a base
HA + H2O <~> H3O+ + A-

Question 14

Describe the dissociation of water?

Answer 14

Water dissociates into hydroxonium ions and hydrogen ions.
H2O + H2O <~> H3O+ + OH-
or
H2O <~> H+ + OH-
Water only dissosciates a small amount so equalibrium lies far to the left, because of this, H2O can be considered to remain constant.
Kw = Kc x H2O = [H+][OH-]