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Question

0.16 g N2H4(Kb=4×106) are dissolved in water and the total volume made up to 500 mL. Calculate the percentage of N2H4 that has reacted to water in this solution.

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Solution

The molar mass of hydrazine is 32 g/mol. 0.16 g of hydrazine in 500 mL corresponds to molarity of 0.1632×0.5=0.01M

N2H4
N2H+5
OH
Initial molarity (M)
0.01
0
0
Equilibrium (M)
001x
x
x
The expression for base dissociation constant Kb is Kb=[N2H+5][OH][N2H4]
Substitute values in the above expression.
4×106=x×x0.01x
Since Kb is very small, 0.01x0.01
Hence, x=2×104
The percentage dissociation of hydrazine is 2×1040.01×100=2%

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