1. Chemistry Chapter 18:Acids and Bases
Most acids have an H+ that dissociates to a solution.
Most bases have an OH- that dissociates to a solution.
Properties of acids.
Acids mostly dissociate H+ into solution and are electron acceptors.
Acids turn litmus red.
Acids are electrolytes and conduct electricity in solution.
Mg and Zn react with acids to make H2.
An acid solution has more H+ than OH-.
Acids taste sour.

2. Base Properties
Bases form electrolyte solutions and conduct electricity.
Bases turn litmus blue.
Bases taste bitter.
Most bases dissociate to release OH- to solution.
Bases are electron donators.

3. Acid Base Models Arrhenius acids dissociate to produce H+.
Arrhenius bases dissociate to produce OH-.
HCl, H2SO4, H3PO4 are all Arrhenius acids.
NaOH, Mg(OH)2, and Al(OH3) are all Arrhenius bases.
HCl is monoprotic acid, H2SO4 is a diprotic acid, H3PO4 is a triprotic acid.

4. Bronstead-Lowry Model
Acids are hydrogen-ion donors.
Bases are hydrogen-ion acceptors.
These can be considered together to make Bronstead-Lowry acid/base pairs.
H3O+= hydronium

5. The Lewis Model Lewis acids is an electron-pair acceptor.
(Think of H+ …it has no electrons and can only accept.)
Lewis bases are electron-pair donors.
ACID BASE FINAL PRODUCT

6. 18-2 Strengths of Acids and Bases
Strength of Acids…the strength of an acid is related to how much the acid tends to lose H+.
Concentration of an acid is how many moles/L of the acid is present.

7. Ka and Kb Ka and Kb are acid and base constants that tell us strength.
Example: Solve for the Ka of an acid if an original
.100 molar solution of HX dissociates .001M H+.
Answer: Ka=1.01 x 10-5