Calculate the Moriarty of an aqueous NaOH solution if 28.93 mL of a 0.513 M H2SO4 is required to reach the end-point when titrated against 20.00 mL of the NaOH solution. The balanced chemical equation for this neutralization reaction is
H2SO4 2 NaOH > Na2SO4 2H2O
Please help!
Calculate the Moriarty of an aqueous NaOH solution if 28.93 mL of a 0.513 M H2SO4 is required to reach the end-point?
2016-06-13 9:39 am
回答 (2)
2016-06-13 1:42 pm
H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O
No. of moles of H₂SO₄ = (0.513 mol/L) × (28.93/1000 L) = 0.513 × 0.02893 mol
No. of moles of NaOH = 0.513 × 0.02893 × 2 mol
Molarity of NaOH = (0.513 × 0.02893 × 2 mol) / (20.00/1000 L) = 1.48 M
No. of moles of H₂SO₄ = (0.513 mol/L) × (28.93/1000 L) = 0.513 × 0.02893 mol
No. of moles of NaOH = 0.513 × 0.02893 × 2 mol
Molarity of NaOH = (0.513 × 0.02893 × 2 mol) / (20.00/1000 L) = 1.48 M
2016-06-18 1:24 pm
(28.93 mL) x (0.513 M H2SO4) x (2 mol NaOH / 1 mol H2SO4) / (20.00 mL NaOH) = 1.48 M NaOH
收錄日期: 2021-04-18 15:04:45
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