Calculate the pH value of 0.01 M HCl.

Given Data:

Concentration of Acid = 0.01 M

Applying pH formula:

Since HCl is a strong monoprotic acid, the hydronium ion concentration is same as acid concentration.

So, $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$ = 0.01 M

Now, we know that

pH = - log$\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$

pH = -log(0.01)

pH = -log($\frac{1}{100}$)

pH = -log(${10}^{-2}$)

pH = -(-2)

pH =2

$\therefore$The pH value of HCl at a given concentration of 0.01 M is 2.

Also, if $7<\mathrm{pH}<14$ the solution is a basic solution.