Chapter 17, Problem 88IAE

The Henderson-Hasselbalch equation can be written as $pH=p{K}_a-\log \left(\frac{1}{a}-1\right)$ where $a=\frac{\left[A^{-}\right]}{\left[A^{-}\right]+\left[HA\right]}$ . Thus, the degree of ionization (a) of an acid can be determined W both the pH of the solution and the $p{K}_g$ , of the acid are known

a. Use this equation to plot the pH versus tie degree of ionization for me second ionization constant of phosphoric acid $\left(K_8=6.3\times {10}^{-8}\right)$

b. If $pH=p{K}_a$ what is the degree of ionization?

c. If the solution had a pH of 6.0, what would the value of a be?