EXPERIMENT GUIDES
Pick one. Book a bench. Run it.
Full protocols with apparatus lists, step-by-step technique, safety notes, and the results you should expect — so you know when you've nailed it.
5 of 19 experiments
Titration: ethanoic acid vs sodium hydroxide
The classic weak acid–strong base titration. Standardise 0.1 M ethanoic acid against 0.1 M NaOH using phenolphthalein, and see why the endpoint lands above pH 7.
Double-indicator titration: phosphoric acid against sodium hydroxide
Phosphoric acid holds three protons and gives up the first two at clearly separate points. Put two indicators in one flask and catch both end-points in a single run — red to orange, then yellow to green.
Redox titration: ethanedioic acid vs potassium manganate(VII)
A self-indicating redox titration. Heat ethanedioic acid (oxalic acid) with dilute sulfuric acid to about 70°C, then titrate against acidified potassium manganate(VII) — no indicator needed, because KMnO4 is its own: the flask stays colourless until the very last drop leaves it permanently pale pink.
Thermal decomposition: water of crystallisation in hydrated zinc sulfate
Heat hydrated zinc sulfate, FA 4 (ZnSO₄·yH₂O), in a crucible until its mass stops changing, then use the mass of water driven off to calculate y — the number of water molecules per formula unit.
Qualitative analysis: a mislabelled salt and three manganese oxidation states
A bottle labelled hydrated zinc sulfate that isn't, and three manganese compounds that turn out to be the same element at different oxidation states. Devise your own cation/anion tests on the first, then run a fixed three-test comparison across the second.