Answered: If the ?b of a weak base is 1.7×10−6,…

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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Question

If the ?b of a weak base is 1.7×10−6, what is the pH of a 0.18 M solution of this base?

Expert Solution

Step 1

The base dissociation constant is K_b, which indicates the dissociation of base in water. The dissociation of base is more, when K_b is large and the base is strong.

Given:

K_b of weak base = 1.7 x 10^-6

Molarity of solution = 0.18 M

Step 2

To find the pOH of the solution,

$\begin{array}{rcl} For weak base, K_{b} & = & 1.7 \times 10^{- 6} \\ Concentration of weak base, C & = & 0.18 M \end{array}$

Substituting the values in the following equation,

$\begin{array}{rcl} pOH & = & \frac{1}{2} [{pK}_{b} - \log C] \\ pOH & = & \frac{1}{2} [- \log K_{b} - \log C] \\ = & \frac{1}{2} [- \log (1.7 \times 10^{- 6}) - \log (0.18)] \\ = & 3.257 \end{array}$

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