This how it works covers How Precipitate Formation Works within Tests for Ions for GCSE Chemistry. Revise Tests for Ions in Chemical Analysis for GCSE Chemistry with 20 exam-style questions and 14 flashcards. This topic appears regularly enough that it should still be part of a steady revision cycle. It is section 5 of 14 in this topic. Use this how it works to connect the idea to the wider topic before moving on to questions and flashcards.
Topic position
Section 5 of 14
Practice
20 questions
Recall
14 flashcards
⚙️ How Precipitate Formation Works
All these anion tests work through precipitation reactions — two soluble ionic compounds react to form one insoluble product (the precipitate) and one soluble product that stays in solution.
For the sulfate test with barium chloride: when BaCl₂(aq) and Na₂SO₄(aq) are mixed, the Ba²⁺ and SO₄²⁻ ions have an extremely strong attraction for each other. Barium sulfate is virtually insoluble in water — so as soon as Ba²⁺ meets SO₄²⁻, they combine and immediately drop out of solution as a solid. The Na⁺ and Cl⁻ ions are spectator ions — they remain dissolved and play no part in the reaction.
The net ionic equation (removing spectator ions) is: Ba²⁺(aq) + SO₄²⁻(aq) → BaSO₄(s)
For halide tests: silver ions have very different affinities for different halides. Ag⁺ + Cl⁻ gives a very insoluble white precipitate. Ag⁺ + Br⁻ gives a slightly less insoluble cream precipitate. Ag⁺ + I⁻ gives an even less insoluble yellow precipitate. The colours and solubilities are a direct result of the physical properties of the silver halide crystal structures.