Chapter 20: Acids, Bases and pH Flashcards
Acids
- Proton donors
- dissociate + release H+ in aqueous solution
Alkalis
- proton acceptor
- dissociate + release OH- in aqueous solution
Neutralisation
H+(aq) + OH-(aq) -> H2O(aq)
Hydronium ion (H3O+)
active acid ingredient in any aqueous acid
Different types of acids
- Monobasic
- Dibasic
- Tribasic
- Refers to the total number of H+ ions in the acid that can be replaced per molecule in an acid-base reaction
Types of salts equations
MASH
AAWS
BAWS
CAWCS
pH
A logarithmic scale
Relationship between [H+] and pH
inversely proportional (as one increases, the other decreases)
pH = -log[H+]
[H+] = 10^-pH
What does a change in pH by 1 cause?
10 times difference in [H+]
10^x
Calculating the pH of strong acids
- Strong acids fully dissociate
HA -> H+ + A-
Therefore [H+] = [HA} for strong acids
How many significant figures do you give pH to?
2
Calculating the pH of weak acids
- Weak acids partially dissociate
Ka = [H+][A-]/[HA] = [H+]2/[HA]
Relationship between Ka value and strength of an acid
The larger the Ka value, the more dissociation, so the stronger the acid
Ka and pKa equations
pKa = -logKa
Ka = 10^-pKa
Relationship between Ka and pKa
Inversely proportional
Why is pKa used?
Easier to compare acid strengths
Approximation 1
[H+]eqm. = [A-]eqm.
There is a small dissociation of H+ from H2O but this is ignored
Approximation 2
[HA]start = [H+]eqm.
as you can neglect any decrease in the conc.. of HA from dissociation because dissociation of weak acids is small
Determination of Ka experimentally
- Prepare a standard solution of the weak acid of known concentration
- measure the pH using a pH meter
Ionisation of water
- Water ionises very slightly (very small dissociation)
Kw
[H+][OH-]
Kw at 298K (standard conditions)
1.00 x 10^-14
sets up the neutral point on the pH scale
Conc. of acidic solution
[H+]>[OH-]
Conc. of neutral solution
[H+]=[OH-]
Conc. of alkaline solution
[H+]<[OH-]
Alkali
Soluble base that releases OH- ions in aqueous solution
Strong base
alkali that completely dissociates in solution
What is needed to calculate the pH of a strong base
- Kw
- Conc. of base
What type of reaction is the ionisation of water?
Endothermic