Acid-Base And pH (w4) Flashcards
pKa shows …
How strong an acid is
Strong acid =
Completely ionised in water
pH =
-log10[H+]
Strong base =
Completely dissociated
Kw = 1 x 10^(-14)
Kw =
[H+][OH-]
Weak acids =
Don’t completely ionise in water.
The amount of ionisation is governed by the equilibrium.
pKa?
The pH at which it is exactly half dissociated.
If pH is increased (more basic) ?
The acid will become more ionised, pH > pKa dissociated.
If pH is lowered (more acidic) ?
The acid becomes less ionised, pH < pKa undissociated.
Ratio of ionised: non-ionised forms …
A shift in pH by one unit to either side of the pKa value must change the ration by a factor of 10.
Outline an equation for a neutralisation reaction …
ACID + BASE —> SALT + WATER
What does salt hydrolysis usually effect ?
The pH of a solution
Strong acid + strong base =
Neutral salt
PH = 7
Strong acid + weak base =
Acidic salt
pH <7
Weak acid + strong base =
Basic salt
pH >7
Weak acid + Weak base =
Dependant on which one is stronger
Weak acid + weak base concepts :
- Ka cation > Kb anion = acidic solution
- Kb anion > Ka cation = basic solution
- if Ka and Kb are similar the solution is close to neutral.
What is the half equivalence point ?
The half point - the half of the total amount of base (added) needed to neutralise the acid it has been added to.
PH = pKa of the weak acid
What us the equivalence point ?
The end point of the reaction = there are equal stoichiometric amounts.
The reaction has completed as all the acid has been converted to its conjugate Base.
What is an acid-base titration (neutralisation) ?
The quantitative analysis of the concentration of an unknown acid or base solution.
What us a buffer solution ?
A solution which is able to resist changes in pH on addition of small amounts of acid or base.
Define buffer capacity ….
The number of moles per litre of a strong acid or base required to produce an increase or decrease of one pH unit in the solution.
IN CLASS TEST ;
What is the pH of a buffer solution containing 0.042M NaH2PO4 and 0.058M Na2HPO4 ?
HINT
Use the Henderson-Hasselbalch equitation;
PH = pKa + log10 x ([A-]/[HA-])
Figure out which one is the base [A-]
And which is the acid [HA-]
What do we do to move the pH of the buffer solution up by one unit of pH = pKa ? (More basic)
We need to insure the ionised form is 10 times higher.
Dibasic acid =
2 ionisable groups
Tribasic acid =
3 ionisable groups
Ionisable groups ;
Some acids have more than one ionisable group this means more than one H+ is released.
Is it more difficult to lose a H+ from an anion or uncharged molecule ?
It is more difficult to lose a H+ form and anion.
What do basic oxides react with ?
Acids
What to acid oxides react with ?
Bases
What to amphoteric substances react with ?
Both acids and bases
What happens when there are more double bonded oxygens in a molecule ?
The more acidic it will be
Why does acidity increase as number of double bonded oxygens increase ?
There is more resonance forming so greater e- delocalisation making a more stable conjugate base.
How do you know a reaction is completed ?
All the acid has been converted to its conjugate base
What does it mean if there is a large pKa difference ?
The reaction is irreversible
What happens to H20 in an aqueous solution ?
The H2O will donate the H+ to any base stronger than OH-
What do amphiprotic compounds act as ?
They act as a proton donor and as a proton acceptor
What do amphoteric compounds function as ?
Either an acid or base depending upon conditions it is in.
What is an amino acid ?
And amphoteric compound, contains separate acidic and basic groups
What is the isoelectric point (pI) ?
The pH at which concentration of the zwitterion is maximum Or pH at which the concentrations of cationic and anionic forms are equal.
When are amino acids positively charged, negatively charged and neutral ?
- positively charged at low acidic pH
- negatively charged at high basic pH
- NEUTRAL (zwitterionic) at neutral pH (7)
What’s are some properties of an ionised species ?
- very low lipid solubility
- unable to permeate through membranes
- only non - ionised drug is usually able to cross membranes
Give an example of a compound commonly used to prepare buffers for biochemical experiments …
Glycine