How many milliliters of 0.750 M H2SO4 solution is needed to react with 55.0 mL of 2.50 M KOH solution?
回答 (2)
2016-12-13 12:37 pm
2KOH(aq) + H₂SO₄(aq) → 2 H₂O(l) + K₂SO₄(aq)
OR: Mole ratio KOH : H₂SO₄ = 2 : 1
No. of milli-moles of KOH reacted = (2.50 mmol/mL) × (55 mL) = 137.5 mmol
No. of milli-moles of H₂SO₄ needed = (137.5 mmol) × (1/2) = 68.75 mmol
Volume of H₂SO₄ needed = (68.75 mmol) / (0.750 mmol/mL) = 91.7 mL
OR: Mole ratio KOH : H₂SO₄ = 2 : 1
No. of milli-moles of KOH reacted = (2.50 mmol/mL) × (55 mL) = 137.5 mmol
No. of milli-moles of H₂SO₄ needed = (137.5 mmol) × (1/2) = 68.75 mmol
Volume of H₂SO₄ needed = (68.75 mmol) / (0.750 mmol/mL) = 91.7 mL
2016-12-13 12:37 pm
(55.0 mL) x (2.50 M KOH) x (1 mol H2SO4 / 2 mol KOH) / (0.750 M H2SO4) = 91.7 mL H2SO4
收錄日期: 2021-04-18 15:53:49
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https://hk.answers.yahoo.com/question/index?qid=20161213042633AA40Mck