1. Acids, Bases, and Salts

2. Electrolytes
An electrolyte is a substance that dissociates when dissolved in water. (Nonelectrolytes do not dissociate.)
These compounds conduct electricity based on this dissociation.
To dissociate means to separate into ions in solution.
Acids, bases, and salts (ionic compounds) are all electrolytes.

3. Strong vs. Weak Electrolytes
Strong electrolytes fully dissociate in water. (ex. Ionic compounds, strong acids, strong bases)
Weak electrolytes only partly dissociate in water. (ex. Weak acids and weak bases)
Nonelectrolytes do not dissociate in water. (nonpolar covalent compounds)

5. Write an equation for the dissociation of magnesium nitrate in water.

6. Write an equation for the dissociation of the weak acid, HF, in water.

7. Acids and Bases
Acids, bases, and salts make up compounds known as electrolytes.
Arrhenius acids – substances that ionize in water to produce the hydrogen ion, H+.
Arrhenius bases – substances that ionize in water to produce the hydroxide ion, OH-.

9. HCl(g) → H+(aq) + Cl-(aq)
NaOH(cr) → Na+(aq) + OH-(aq)
Dissociation – already formed ions separate
Ionization – neutral molecules react with water to form charged ions

10. Strength of Acids and Bases
Strength of acids and bases depends on how completely they ionize in water
- the strongest acids and bases fully ionize in water while weak acids and bases only ionize slightly

11. Strong acids (Know these)– HCl, HBr, HI are all strong, while all other binary acids are weak
As a rule, all acids with at least two more oxygens than hydrogens are strong (H2SO4, HNO3,HClO4)
Strong bases – Hydroxides of the Groups I and II elements except for Be are all strong.

12. Acid Nomenclature In general, names of acids will begin with hydrogen.
If the anion does not contain oxygen, the acid begins with hydro and ends in –ic
HCl = hydrochloric acid
HBr =
HCN =

13. Acids containing oxygen
If the acid contains oxygen, the acid does not have hydro at the start and either ends in ic or ous.
If the anion ends in –ate use –ic
HNO3 = nitric acid
If the anion ends in –ite use –ous
H2SO3 = sulfurous acid

14. What is the formula for hydroiodic acid?HI
HI2
H2I
HIO3

15. What is the formula for hydrocyanic acid?
H3N HN
HCN
HSCN

16. What is the formula for phosphoric acid?
H3PO3
H3PO4
HPO4
HPO3

17. What is the formula for sulfurous acid?
H2SO3
H2SO4
H2S
HS2

18. What is the name of HNO2? Hydronitric acid Hydronitrous acid

19. What is the name of HCl? Hydrochloric acid Hydrochlorous acid

20. What is the name of HClO4? Hydrochloric acid Chlorous acid
Perchloric acid

21. Relative Strength of Acids and Bases

22. Conjugate Acids and Bases
The strength of conjugate acids and bases are inversely proportional.

24. Kw Kw for water is based on the equation:
2H2O (l) -> OH- (aq) + H3O+ (aq)
Kw = [OH-][H3O+] = 10-14
Therefore, if you know either hydroxide or hydronium concentrations, you can solve for the other.

25. pH scale
pH is the measure of the concentration of hydronium ion in a water solution
pH = -log[H30+]
Scale goes from 0 to 14.
0 to 7 is acidic, 7 is neutral, 7 to 14 is basic

26. pH – log based
Every increase of 1 on the pH scale changes the concentration by a power of 10.
How much stronger is a substance with a pH of 4 vs a pH of 6?

27. pOH scale
pOH is the measure of the concentration of hydroxide ion in a water solution
pOH = -log[0H-]
Also, pH + pOH =14

28. Neutralization Reaction
A neutralization reaction occurs when and acid and a base react to form water and a salt.
Acid + Base -> Water + Salt
***When the base has a CO32- ion, CO2 is also produced.

29. Titrations
Titrations are a quantitative lab technique that helps identify an unknown concentration of acid or base by titrating it against a titrant, or known acid or base concentration.

30. Titration Method
Add an accurately measured volume of unknown acid (or base) to an Erlenmeyer flask
Put 2-3 drops of phenolphthalein indicator to the unknown solution.
Start adding the titrant and continue until the solution turns pink and stays pink.

32. Titration Tips
Record the unknown’s volume by subtracting the ending vs. starting amount from buret (use the right amount of sig figs).
You can add the titrant quickly at first but once it starts turning pink, swirl the flask and start adding more slowly. Swirl after each drop towards the equivalence point.