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Sodium Bromide with Sulfuric Acid

The sulfuric acid acts as an acid and donates a proton to the halide.Misty fumes of HBr are observed. NaBr + H2SO4 → NaHSO4 + HBr
A redox reaction also occurs: The bromide ions are strong enough reducing agents to reduce the concentrated sulfuric acid to sulfur dioxide gas.The bromide ions are oxidised to bromine. The oxidation state of the sulfur decreases from +6 in the sulfuric acid to +4 in the sulfur dioxide. Overall: 2HBr + H2SO4 → 2H2O + SO2 + Br2 You get a mixture of three gases including brown fumes of bromine gas. Sulfur dioxide is colourless.

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Specification: AQA Chemistry (7404), AS-level, 3.2.3.1 Trends in properties. Topic: Group 7.

Key terms in this lesson

Oxidation
The addition of oxygen, the removal of hydrogen, the loss of electrons, or an increase in oxidation number.
Oxidation number
A number that represents the number of electrons an atom has lost or gained, or would do if the compound were fully ionic.
Reducing agent
A species that donates electrons to another species, causing that species to be reduced.

More in Group 7

All 20 lessons in Group 7 · All AQA AS-level Chemistry topics