Acids and Bases. HA H + + A - HCL H + + CL - CH 3 COOH H + + CH 3 COO -

Acids and Bases

HA ↔ H+ + A-

HCL ↔ H+ + CL-

CH3COOH ↔ H+ + CH3COO-

Strong

Weak

0.003M HCl

9M HNO3

7M CH3COOHethanoic acidor acetic acid

5% ethanoic acid

(vinegar)

Use ‘dilute’ or ‘concentrated’ and ‘weak’ or ‘strong’to describe the acids above.

2H2O↔ H3O+ + OH-

[H+] [OH-] [H2O]

H2O↔ H+ + OH-

Kc =

Kw = [H+] [OH-] = 10-14

Kw = [H+] [OH-] = 10-14

[H+] for pure water is 1 X 10-7

Kw = [10-7] [10-7] = 10-14

pH is -log [H+]

So the pH of pure water is 7

HA ↔ H+ + A-

H+ + OH- H2Oduring titration

Strong/weak acids cannot be differentiated by titration.

  Mohr burette

Remember to:

Remove bubbles from the

valve area

Record data as you titrate

including uncertainties

What is the second

burette for?

Flush your burette with

distilled water when finished

AcidicpH 0-8.2

BasicpH 8.2-12

Phenolphthalein