In a titration 25.0 cm3 of 0.040 mol dm-3 aqueous metal hydroxide exactly neutralises a 20.0 cm3 sample of 0.100 mol dm-3 sulfuric acid.Calculate the stoichiometric ratio and give the balanced equation.Moles of metal hydroxide = 0.040 × 25.0 ÷ 1000 = 1.00 × 10-3 mol.Moles of sulfuric acid = 0.100 × 20.0 ÷ 1000 = 2.00 × 10-3 mol.Ratio of metal hydroxide to acid = 1.00 × 10-3 : 2.00 × 10-3 = 1 : 2. Each H2SO4 releases two H+ ions, so one mole of the hydroxide reacts with four moles of H+. The hydroxide must therefore contain four OH- ions, M(OH)4.Balanced equation: M(OH)4 + 2H2SO4 → M(SO4)2 + 4H2O
Example Question - 1
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Specification: AQA Chemistry (7404), AS-level, 3.1.2.5 Balanced equations and associated calculations. Topic: Amount of Substance.
Key terms in this lesson
- Titration
- An analytical technique used to determine the volume of one solution that exactly reacts with a known volume of another solution.
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All 33 lessons in Amount of Substance · All AQA AS-level Chemistry topics