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Question

A mixture of H2SO4 and H2C2O4 (oxalic acid) and some inert impurity weighing 3.185 g was dissolved in water and the solution made up to 1 L, 10 mL of this solution required 3 mL of 0.1 N NaOH for complete neutralization. In another expriment 100 mL of the same solution in hot condition required 4 mL of 0.02 M KMnO4 solution for complete reaction. The weight percentage of H2SO4 in the mixture was:

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Solution

Let x and y are milli moles H2SO4 and H2C2O4 in given mixture when both reacted with base
m eq. of acids = m eq. of base;
(x+y)×2=3×0.1×100010
x+y=15
In second experiment only KMnO4 reacted with H2C2O4 in which Mn7+ converted into Mn2+ and C2O24 converted into CO2

milli equivalent of H2C2O4=milli equivalent of KMnO4
y×2=4×0.02×5×1000100y=2x=13,weight of H2SO4=13×103×98=1.274 g
weight % of H2SO4 in sample =1.2743.185×100=40%

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