The density of a 0.0122 M KMnO4 is 1.037 g/mL. Suppose 26.35 g of 0.0122 M KMnO4 are required to titrate 1.072 g of a household H2O2 solution. Except for answers to (a) and (e), use E notation. Do not include units, just enter numerical values.
a) calculate the ml of MnO4- added to reach the endpoint.
b) calculate the moles of MnO4- added to reach the endpoint.
c) calculate the number of moles of H2O2 in the sample.
d)Calculate the number of grams of H2O2 in the sample.
e)Calculate the %m/m H2O2 in the household H2O2 solution
Ans :
a)
Density = mass / volume
putting values :
1.037 g/mL = 26.35 g / V
V = 25.41 mL
so mL of MnO4- = 2.541E+1
b)
Moles of MnO4- = molarity x volume (L)
putting values :
= 0.0122 M x 0.02541 L
= 0.00031 mol
So number of moles of MnO4- = 3.1E-4
c)
2 moles MnO4- react with 5 moles H2O2
so 0.00031 mol MnO4- will react with : ( 0.00031 mol x 5 mol) / 2 mol
= 0.000775 mol H2O2
so mol H2O2 = 7.75E-4
d)
Number of grams H2O2 in sample = mol x molar mass
= 0.000775 mol x 34.0147 g/mol
= 0.0264 g
so mass of H2O2 = 2.64E-2
e)
5m/m H2O2 = ( mass H2O2 / mass sample) x 100
= (0.0264 g / 1.072 g ) x 100
= 2.46
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