Question

During the reaction, 3.50 μmol of HCl are produced. Calculate the final pH of the reaction solution. Assume that the HCl is completely neutralized by the buffer.

Answer 1

Answer:

The pH of the solution will be equal to 5.46

Explanation:

The dissociation reaction of HCl is equal to:

HCl → H+ + Cl-

To solve the exercise we must first convert the µmoles to moles using the following conversion factor:

3.5µmoles x $\frac{1 mol}{1x10^{6} umol}$ = 3.5x$10^{-6}$moles

Assuming a liter of solution, we can calculate the molar concentration by:

M = $\frac{Number of moles}{Liter of solution}$

Replacing:

M = $\frac{3.5x10^{-6}moles }{1 L}$ = 3.5x$10^{-6}$moles/L

As this acid dissociates completely, the concentration of protons and chloride will be equal to 3.5x$10^{-6}$moles/L

The pH will be equal to:

pH = -log[H+]

Replacing:

pH = -log[3.5x$10^{-6}$] = 5.46