pH chemistry problem?

pH = -1 * log [H3O+1]

Let’s use 1.0 as the hydronium concentration in the equation to determine pH of the original solution.

pH = -1 * log 1

This is 0.

A 1.0 M solution contains one mole of the solute per liter of the solution. To determine the number of moles of HCl, multiply the molarity by the volume in liters

n = 0.01 * 1 = 0.01

To dilute this acid, 900 ml of water was added. Now there is this number of moles of HCl in one liter of the solution. So, this is new hydronium concentration.

pH = -1 * log 0.01 = 2

The ph of the HCl has increased 2 units.

1) Calculate pH of starting solution:

pH = -log 1.0 = 0 (yes, you can have a pH of zero)

2) Get the moles of acid in the 10 mL:

(1.0 mol/L) (0.0100 L) = 0.0100 mL

3) Get the molarity of the diluted solution:

0.0100 mol / 1.0 L = 0.0100 M

4) Calculate the new pH:

pH = -log 0.0100 = 2