Question 4
25cm³ of iron(II) sulphate solution required 21cm³ of 0.7M KMnO₄ for oxidation.
MnO₄⁻(aq) + 8H⁺(aq) + 5Fe²⁺(aq) → Mn²⁺(aq) + 4H₂O(l) + 5Fe³⁺(aq)
Calculate the concentration of the iron (II) sulphate solution.
Please help me with this chemistry question.?
2017-10-29 1:10 pm
回答 (1)
2017-10-29 4:56 pm
✔ 最佳答案
MnO₄⁻(aq) + 8H⁺(aq) + 5Fe²⁺(aq) → Mn²⁺(aq) + 4H₂O(l) + 5Fe³⁺(aq)Mole ratio KMnO₄ : FeSO₄ = MnO₄⁻ : Fe²⁺ = 1 : 5
No. of moles of KMnO₄ reacted = (0.7 mmol/cm³) × (21 cm³) = 14.7 mmol
No. of moles of FeSO₄ required = (14.7 mmol) × 5 = 73.5 mmol
Concentration of the FeSO₄ solution = (73.5 mmol) / (25 cm³) = 2.94 M
收錄日期: 2021-04-18 17:55:33
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