1. Acids and Bases

2. Acids Taste sour Turn litmus paper red React vigorously with metals
Conduct electricity
Corrosive
Make H3O+
Proton donors (BrØnsted-Lowry)

3. Bases Turn litmus blue Taste bitter Feel slippery Conduct electricity
Corrosive
Make OH- ions
Proton acceptor (BrØnsted-Lowry)

4. Dissociation Ionic compound breaks apart into its ions
Write the dissociation equation for the following:
NaOH
Ca(OH)2
HCl
H2CO3

5. Strong vs. Weak (electrolytes/acids/bases)
Strong completely dissociate
Weak partially dissociate
A strong (acid/base) completely ionizes in a solvent.
In a weak (acid/base) only a small amount is ionized at any given time.
In equilibrium
Few H+/OH- are released in aqueous solution.

6. Arrhenius Acids
Any substance that, when added to water, increases the hydronium (H3O+) concentration.
Number of ionizable H determines how many H3O+ are made.
Ionizable H are at the beginning of the compound
HCl
H2SO4

7. Arrhenius Base
Any substance that, when added to water, makes hydroxide ions (OH-)
Number of OH- in formula is how many OH- are made
NaOH
Ca(OH)2

8. Problems w/Arrhenius Limited to aqueous solutions
Cannot classify substances that can act as either acids or bases.

9. Brønsted-Lowry Classification
Brønsted-Lowry acid - donates a proton
look at the reaction:
(1) HCl  H+ + Cl−
(2) H+ + H2O  H3O+
HCl is an Arrhenius acid- makes a H3O+.
HCl is a Brønsted-Lowry acid because it donates a proton (H+).

10. Brønsted and Lowry Base
A proton acceptor.
Ammonia (NH3)-proton acceptor
NH3- makes OH- in water so Arrhenius base
Arrhenius acids/bases are also Brønsted-Lowry acids/bases
Brønsted-Lowry acids/bases are not always Arrhenius acids/bases

11. Classification
Arrhenius acids/bases are also Brønsted-Lowry acids/bases
Brønsted-Lowry acids/bases are not always Arrhenius acids/bases

12. Conjugate Acids and Bases
When an acid looses a proton, it becomes a conjugate base
When a base gains a proton, it becomes a conjugate acid
Write the conjugate base for the following: HF
H2CO3
Write the conjugate acid for the following:
NO3-
HCO3-

13. Every acid has a conjugate base
Every base has a conjugate acid
We can look at an acid/base equations and determine acid/base pairs.

14. When the reaction is reversed, we can identify another acid and another base.
But it is the same acid/base pairs as before

15. HCl + H2O → H3O+ + Cl-

16. Amphoteric Substances that can be either both an acid or a base
can both donate and accept protons.
Example: Water
Has properties of both acid and base
Can donate or accept H+
Hydrogen carbonate
HCO3- + H2O → H2CO3 + OH- (base; H+ acceptor)
HCO3- + H2O → CO3-2 + H3O+ (acid; H+ donor)