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Chemical Analysis

demonstrate knowledge and understanding that a pure substance is a single element or compound not mixed with any other substance; and
demonstrate knowledge and understanding that pure elements and compounds melt and boil at specific temperatures and melting point and boiling point can be used to distinguish pure substances from mixtures.

demonstrate knowledge and understanding that a formulation is a mixture that has been designed as a useful product and is formed by mixing together several different substances in carefully measured quantities to ensure the product has the required properties, for example alloys, medicines and fertilisers;


demonstrate knowledge and understanding of the terms soluble, insoluble, solute, solvent, solution, residue, filtrate, distillate, miscible, immiscible, evaporation and condensation;
investigate practically how mixtures can be separated using filtration, crystallisation, paper chromatography, simple distillation or fractional distillation (including using fractional distillation in the laboratory to separate miscible liquids, for example ethanol and water);

describe paper chromatography as the separation of mixtures of soluble substances by running a solvent (mobile phase) through the mixture on the paper (stationary phase), which causes the substances to move at different rates over the paper;

interpret a paper chromatogram including calculating Rf values;

analyse given data on mixtures to make judgements on the most effective methods of separation and plan experiments to carry out this separation;

Describe how water can be made potable, including the need for filtration, sedimentation and chlorination;) describe how seawater can be made potable using distillation; and. use anhydrous copper(ll) sulfate to test for water.

describe how to carry out a flame test using nichrome wire and concentrated hydrochloric acid to identify metal ions;
demonstrate knowledge of the flame colours of different metal ions:
•    lithium (crimson);
•    sodium (yellow/orange);
•    potassium (lilac);
•    calcium (brick red); and
•    copper(ll) (blue-green/green-blue);

describe the test for metal ions in solution using sodium hydroxide solution and ammonia solution;

.5 describe the tests for the following:
•    chloride, bromide and iodide (using silver nitrate solution);
•    sulfate (using barium chloride solution); and
•    carbonate (using dilute acid and identifying the carbon dioxide evolved);

.6 write ionic equations for the halide and sulfate ion tests and tests for metal ions using sodium hydroxide solution;7 demonstrate knowledge and understanding that many tests for anions and cations are precipitation reactions;.8

plan experiments to identify cations and anions present in an unknown or a given compound; 

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