You carried out the standardization of a potassium permanganate, KMnO4, solution using the procedure described in this laoratory experiment.
mass of sodium oxalate, Na2C2O4.........0.2783
potassium permanganate (KMnO4) solution:
initial buret reading.......0.72mL
final buret reading........33.84mL
(b) Calculate the number of moles of Na2C2O4.
(c) Calculate the number of moles of KMnO4
(d) Calculate the molarity of the KMnO4
Please show all work
B.
The number of moles of Na2C2O4
Given that amount of sodium oxalate, Na2C2O4= 0.2783 g
Number rof mole s= amount in g / molar mass
= 0.2783 g/ 133.998 g/mol
= 2.1*10^-3 mole Na2C2O4
(c) Calculate the number of moles of KMnO4
The balance reaction is as follows:
5Na2C2O4 + 2KMnO4 + 8H2SO4 → 10CO2 + 8H2O + 5Na2SO4 + 2MnSO4 + K2SO4
Now calculate the mole of KMnO4 as follows:
2.1*10^-3 mole Na2C2O4 * 2 mole KMnO4 / 5 mole Na2C2O4
= 8.31*10^-4 mole KMnO4
(d) Calculate the molarity of the KMnO4
Given that
initial buret reading.......0.72mL
final buret reading........33.84mL
volume of KMnO4 = 33.84 ml – 0.72 ml
= 33.12 ml
= 0.03312 L
Molarity = number of mole s/ volume in L
= 8.31*10^-4 mole KMnO4/ 0.03312 L
= 0.025 M
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