## A buffer solution contains 0.475 M nitrous acid and 0.302 M sodium nitrite . If 0.0224 moles of potassium hydroxide are added to 150 mL of t

Question

A buffer solution contains 0.475 M nitrous acid and 0.302 M sodium nitrite . If 0.0224 moles of potassium hydroxide are added to 150 mL of this buffer, what is the pH of the resulting solution

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2 weeks 2021-07-22T07:06:54+00:00 1 Answers 2 views 0

1. Answer: The pH of the resulting solution will be 3.001

Explanation:

Molarity is calculated by using the equation: ……(1)

We are given:

Moles of NaOH = 0.0224 moles

Molarity of nitrous acid = 0.475 M

Molarity of sodium nitrite = 0.302 M

Volume of solution = 150 mL = 0.150 L          (Conversion factor: 1 L = 1000 mL)

Putting values in equation 1, we get:  The chemical equation for the reaction of nitrous acid and NaOH follows: I:                0.07125     0.0224     0.0453

C:             -0.0224     -0.0224   +0.0224

E:              0.04885         –          0.0677

The power of the acid dissociation constant is the negative logarithm of the acid dissociation constant. The equation used is: ……(2)

We know: for nitrous acid = Using equation 2: To calculate the pH of the acidic buffer, the equation for Henderson-Hasselbalch is used: …….(3)

Given values:   Putting values in equation 3. we get: Hence, the pH of the resulting solution will be 3.001