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Titration

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a) Write balanced half equations for the redox reaction of Cr^ n+ and MnO4- in acidic solution .In terms of n, how many moles of electrons per mole of Cr^ n+ , are involved in the oxidation reaction ?Write the balanced overall chemical equation for the above reaction .b)An acidified solution... 顯示更多 a) Write balanced half equations for the redox reaction of Cr^ n+ and MnO4- in acidic solution .In terms of n, how many moles of electrons per mole of Cr^ n+ , are involved in the oxidation reaction ? Write the balanced overall chemical equation for the above reaction . b)An acidified solution containing 1.5x10 ^-3 mol of Cr^n+ is titrated with 0.0250 M KMnO4 solution .The equivalence point of the reaction is reached after 48 cm^3 of KMnO4 has been added. Calculate the value of n.

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a) Half equations: 2Crn+ + 7H2O → Cr2O72- + 14H+ + (12 - 2n)e- MnO4- + 8H+ + 5e- → Mn2+ + 4H-2OH No. of moles of electrons per mol of Crn+ = (12 - 2n)/2 = (6 - 2n) mol Overall equation: 10Crn+ + (12-2n)MnO4- + (8n-13)H2O→ 5Cr2O72- + (12-2n)Mn2+ + (16n-26)H+ OR: 10Crn+ + (12-2n)MnO4- + (26-16n)H+ → 5Cr2O72- + (12-2n)Mn2+ + (13-8n)H2O b) Mole ratio Crn+ : MnO4- (1.5 x 10-3) : (0.025 x 48/1000) = 10 : (12 - 2n) (1.5 x 10-3) : (1.2 x 10-3) = 10 : (12 - 2n) 5 : 4 = 5 : (6 - n) 6 - n = 4 n = 2 =

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