Answered: A 40.0-mL solution of 0.100 M ammonia…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 40.0-mL solution of 0.100 M ammonia (NH₃; K_b = 1.8 x 10^–5) is titrated with 0.100 M HCl solution. What is the pH of the solution after 20.0 mL of the acid solution is added? The net ionic equation is:

NH₃(aq) + H₃O⁺(aq) --> NH₄⁺(aq) + H₂O

(A) 9.55

(B) 9.25

(D) 5.28

Expert Solution

Step 1

Given that,

The net ionic equation is:

NH₃(aq) + H₃O⁺(aq) --> NH₄⁺(aq) + H₂O

Molarity of NH₃solution = 0.1 M

Moles in NH₃ solution = 0.1 M × 40 mL = 4 mmol

Molarity of HCl solution = 0.1 M

Moles in HCl solution = 0.1 M × 20 mL = 2 mmol

Ionisation constant for NH_3,K_b= 1.8 x 10^–5

since, pK_b= -log (1.8 x 10^–5)

= 4.74

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