Chemistry
17. Determination of an equilibrium constant
- 00:33 What is happening in the flasks during this period?
- 00:38 How do you calculate the mass? How do you convert mass into number of moles?
- 01:15 What colour-change are you expecting? Forgotten titration technique? View earlier recordings of the experiments for more details.
- 01:32 Is the phenolphthalein the colour you expected?
communal burette of glacial ethanoic acid
communal burette of ethanol
communal burette of de-ionised water
communal burette of 1.0 mol dm-3 HCl solution
2 x 100 cm3 conical flask with stopper
2 x 250 cm3 conical flask
50.0 cm3 burette and funnel
burette clamp and stand
1 cm3 measuring cylinder (or 1 cm3 volumetric pipette with filler)
100 cm3 measuring cylinder
de-ionised water in wash-bottle
| Hazard | Risk | Control measure |
|---|---|---|
Standard solution 0.1 mol dm-3 NaOH - not harzardous |
Contact with eye or skin.
|
Eye: flood with tap water (10min). Skin: drench with water. |
Phenolphthalein - flammable. |
Ignite if in contact with flame. |
Extinguish flame using fire-blanket. |
Glacial ethanoic acid - flammable, corrosive. Use fume cupboard. |
Contact with eye or skin. |
Eye: flood with tap water (10min). Skin: drench with water. |
Ethanol - highly flammable. |
Contact with eye or skin. |
Extinguish flame using fire-blanket. |
1.0 mol dm-3 HCl solution - not hazardous. |
- |
Eye: flood with tap water (10min). Skin: drench with water. |