Question

Calculate the isoionic pH of 0.010M lysine.

Short answer

The isoionic pH of the given lysine solution is 9.93

Step-by-step solution

Define the isoionic pH

The isoionic point, also known as the isoionic pH, is the result of dissolving a pure and neutral polyprotic acid into water.

The pH at which the average charge of polyprotic acid is zero, is known as the isoelectric point.

Calculate the isoionic pH of lysine.

We are required to find the isoionic of the pure neutral lysine solution.

$\left[\mathrm{H}+\right]=\sqrt{\frac{{\mathrm{K}}_2{\mathrm{K}}_3\mathrm{F}+{\mathrm{K}}_2{\mathrm{K}}_{\mathrm{w}}}{{\mathrm{K}}_2+\mathrm{F}}}$

$\left[\mathrm{H}+\right]=\sqrt{\frac{{\mathrm{K}}_2{\mathrm{K}}_3\left(0.010\right)+{\mathrm{K}}_2{\mathrm{K}}_{\mathrm{w}}}{{\mathrm{K}}_2+\left(0.010\right)}}$

pH = 9.93

Thus, the isoionic pH of the given lysine solution is 9.93