Problem: What is the pH of a 0.015 M aqueous solution of hydrazoic acid (HN3) (Ka = 1.9 x 10–5) at 25°C?a. 2.89b. 1.82c. 3.28d. 6.55e. 4.87

FREE Expert Solution

Equilibrium reaction:        HN3(aq) + H2O(l)  N3-(aq) + H3O+(aq) 


Step 1: Construct an ICE chart for the reaction.


Step 2: Write the Ka expression.

Ka=productsreactantsKa=[N3-][H3O+]HN3


Step 3: Calculate the equilibrium concentrations.

Ka=xx0.015-x1.9×10-5=x20.015-x

[HC3H5O2]initialKa>500; ignore -x

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Problem Details

What is the pH of a 0.015 M aqueous solution of hydrazoic acid (HN3) (Ka = 1.9 x 10–5) at 25°C?

a. 2.89
b. 1.82
c. 3.28
d. 6.55
e. 4.87

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