pH

Question 1

Acids

Answer 1

Proton donors

Question 2

Bases

Answer 2

Proton acceptors

Question 3

pKa

Answer 3

pKa = -logKa
Ka = 10^-pKa

Question 4

Strong acids

Answer 4

Dissociate completely in water
HCl -><- H+ + Cl-

Question 5

Weak acids

Answer 5

Partially dissociate in water
CH3COOH -><- H+ + CH3COOH-

Question 6

Ka

Answer 6

Ka = [H+] [A-] / [HA]
Ka = [H+]^2 / [HA]
If Ka is higher then it is a strong acid. However if it is lower then it is a weak acid.

Question 7

Assumptions

Answer 7

1. [H+] = [A-] – assuming that HA dissociates into H+ and A- equally
2. [HA]equ = [HA]start - [H+] equ – assuming that dissociation in weak acids is small so we can neglect any decrease in [HA] from dissociation.

Question 8

An acid-base indicator

Answer 8

A weak acid (HIn) that changes colour in acidic form and in its conjugate base form

Question 9

Equivalence point

Answer 9

The point in a titration at which the volume of one solution has reacted exactly with the volume of the second solution

Question 10

End point

Answer 10

The point in a titration where the indicator contains equal concentrations of its HA and A- forms hence it shows the in-between colour

Question 11

End point

Answer 11

The point in a titration where the indicator contains equal concentrations of its HA and A- forms hence it shows the in-between colour

Question 11

End point

Answer 11

The point in a titration where the indicator contains equal concentrations of its HA and A- forms hence it shows the in-between colour