Calculate the percent ionization and the pH of the following solution of phenol, HC6H5O (Ka = 1.3 × 10-10):0.045 M percent ionization = pH=

The reaction taking place is, C6H5OH + H2O⇔C6H5O- + H3O+

Answered: Calculate the percent ionization and…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.125QE

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Question

Calculate the percent ionization and the pH of the following solution of phenol, HC₆H₅O (K_a = 1.3 × 10^-10):

0.045 M

percent ionization =

pH=

Expert Solution

Step 1

The reaction taking place is,

$C_{6} H_{5} {OH + H}_{2} O \Leftrightarrow C_{6} H_{5} O^{-} {+ H}_{3} O^{+}$

Step 2

The concentration of phenol solution is 0.045 M. At a certain time, if ‘x’ moles of phenol get dissociated, then the concentration of phenol becomes (0.045-x) M. At this point, there are ‘x’ moles of C₆H₅O^- and ‘x’ moles of H⁺.

$\begin{array}{rcl} K_{a} & = & \frac{[C_{6} H_{5} O^{-}] [H_{3} O^{+}]}{[C_{6} H_{5} OH]} \\ 1.3 \times 10^{- 10} & = & \frac{(x) . (x)}{(0.045 - x)} \\ Since, x & < & < 0.045, \\ x^{2} & = & (1.3 \times 10^{- 10}) (0.045) \\ = & \sqrt{0.0585 \times 10^{- 10}} \\ x & = & 2.42 \times 10^{- 6} M \end{array}$

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Calculate the percent ionization and the pH of the following solution of phenol, HC6H5O (Ka = 1.3 × 10-10): 0.045 M percent ionization = pH=