Question

# A mixture of H2SO4 and H2C2O4 (oxalic acid) and some inert impurity weighing 3.185g was dissolved in water and the solution was made up to 1litre.10mL of this solution required 3mL of 0.1N NaOH for complete neutralization. In another experiment, 100mL of the same solution in hot conditions, required 4mL of 0.02MKMnO4 solution for complete reaction. The weight % of H2SO4 in the mixture was:

A
40
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B
50
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C
60
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D
80
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Solution

## The correct option is C 40Let x and y be the milimoles of H2SO4 and H2C2O4 in given mixture when both reacted with base.Meq. of acids=Meq. of base(x+y)×2=3×0.1×100010 x+y=15In second experiment, only KMnO4 reacted with H2C2O4 in which Mn7+ converted into Mn2+ and C2O2−4 converted into CO2.∴ Milli-equivalent of H2C2O4= milli-equivalent of KMnO4.y×2=4×0.02×5×1000100y=2∴x=13Weight ofH2SO4=13×10−3×98=1.274g.Weight % of H2SO4 in sample =1.2743.185×100=40%. Hence, the correct option is A

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