3.1.12 Acids and bases Flashcards
the point that represents the solution is acting as a buffer
the straight part of the graph - no change in pH
what is a Bronsted - Lowry acid
proton donor
strong acid definition
completely ionising to give H+ ions in water
what do you use when calculating the HA
use the equivalence point
HA ->
H+ + A-
Ka =
conc H+ x conc A-
divided by
conc ACID HA
pH
-Log10 H+conc
pka
-Log 10 ka
kw
CONC H+ x conc OH-
what assumption can you make in weak acid calculations but not in buffer calculations
H+ conc = A- conc at eqm
p =
- P = - log
pure water
- Pure water = conc of H+ = conc of OH-
- Dilution questions
- Strong acid and water - conc H+ final = conc H+ initial x ( initial volume/ final volume)
just use OH- for bases
half neutralization point
- Half neuralization point
- Conc HA = conc A-
- Meaning pH = pKa
- Buffer calculations
- Initial to final
1. Start with mols of initial HA and A- ( and H+ / OH- from substance added)
2. Draw out the weak acid dissociation equation and the equation of the substance added
3. Workout mols of final - If an acid is added – then add h+ mols to the acid and take them away form the A-
- If a base is added – Oh- mols take away from acid and add them to A-
4. Rearrange Kw and wat not to workout what needed
why is pure water not acidic
as conc OH- = conc H+ by definition
what to do with a di basic and diprotic acid
- Di basic / di protic – have to multiple the conc of H+ or OH- by 2
- Example of a di protic acid = sulfuric acid – example of a di basic = group 2
working out the end poInt Ha
- Color change of the indicator = the end point
Alkali added - n(end point ) = (concentration x volume at the eq point)
- n end point HA = n point (oh-)
workout the pH of a neutralization Acid + Base
- workout the pH of a neutralization Acid + Base
1. workout which is in excess between the Oh- and the H+
2. use the leftover to calculate the pH
relation between H+ and pH
- as the concentration of H+ increases pH decreases
explain why H2O is not shown in the Kw equation
- explain why H2O is not shown in the Kw equation – the concentration of water is (almost) constant
- suggest why the Ph probe is washed with distilled water before new reading
– different solutions must not contaminate each other
- why volume added of base to acid decreases as the end point get closer –
to avoid missing the end point
why indicator is suitable
all have color change within the vertical/ steep part of the titration curve