For the acids, use the formula pH = -log[H+). (Because HCl has 1 H+ ion per formula unit, [H+] equals the molarity.) For water, use what you know about the pH of neutral solutions. For the bases, examine and

extend the pattern. DONE

0.1 M

НСІ

0.001 M

НСІ

0.00001 M

НСІ

Distilled

Water

0.00001 M

NaOH

0.001 M

NaOH

0.1 M

NaOH

pH

pH:

pH:

pH: 7

pH:

pH:

pH:

pH = 1

pH = 3

pH = 5

pH = 9

pH = 11

pH = 13

Explanation:

The pH is defined as log [H⁺]. HCl in solution produce H⁺. That means HCl concentration is equal to H⁺ concentration. Thus:

- 0.1M HCl. pH = -log 0.1 = 1

- 0.001M HCl. pH = -log 0.001 = 3

- 0.00001M HCl. pH = -log 0.00001 = 5

For a base that produce OH⁻ in solution you can define a pOH as pOH = -log [OH⁻] knowing (For water equilibrium) pH = 14 - pOH

Thus, for the NaOH solutions:

- 0.00001M NaOH: pOH = -log 0.00001M = 5. pH = 14 - 5 = 9

- 0.001M NaOH: pOH = -log 0.001M = 3. pH = 14 - 3 = 11

- 0.00001M NaOH: pOH = -log 0.1M = 1. pH = 14 - 1 = 13

pH = 1

pH = 3

pH = 5

pH= 7

pH = 9

pH = 11

pH = 13

Explanation:

Just did the test :)

i can ! i just need to know what the paragraph is! : p

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."