1. Acids and Bases Arrhenius acid – any HA, H2A, H3A, or R-COOH compound
where A- is any anion
Examples: HCl, H2CO3, H3PO3, CH3COOH
Arrhenius base – any MOH, M(OH)2, or M(OH)3 compound where M+ is either a metallic cation or the ammonium ion
Examples: KOH, Mg(OH)2, Al(OH)3

2. Bronsted-Lowry definition
Bronsted-Lowry acid – a proton donor
Bronsted-Lowry base – a proton acceptor
In acids and bases, to what proton are they referring? Right, the H+ ion is the proton.
Substances that can behave as either an acid or a base are amphoteric or amphiprotic.

3. Acid and Base Characteristics
Acids
Have pH < 7
Cause blue litmus paper to turn red
Taste sour
React with metals to produce H2 gas
Bases
Have pH > 7
Cause red litmus paper to turn blue
Taste bitter
Feel slippery

4. Neutralization Reactions
Acids and bases react together to form water and a salt. A salt is a chemical compound created from the combination of an acid and a base.
HA MOH  HOH + MA
acid base water salt

5. Titration Problems
Titration is a lab procedure used to determine the concentration of an unknown solution. Titration problems look no different from the solution stoichiometry problems with which you are already familiar. The only difference is the use of the word titrate. Read “titrate” as “reacts with.”

6. Solving a Titration Problem
What mass of phosphoric acid is needed to titrate 150 ml of 0.4 M solution of potassium hydroxide?
First, since there are two chemicals reacting, a balanced equation is in order
H3PO4 + 3KOH  K3PO4 + 3 H2O

7. Continuation of Titration Problem
Next, you have the volume and the molarity of the KOH solution. You are looking for the mass of the phosphoric acid.
0.150 L KOH ( 0.4 mol KOH) (1 mol H3PO4)(98 g H3PO4)
1 L KOH mol KOH mol H3PO4
= 1.96 g of H3PO4 needed for reaction

8. pH, pOH, [H+ ], [OH-]
pH is a measure of the acidity or basicity of a solution. Mathematically, it is expressed as
pH = - log [H+] where the brackets mean molarity
You may see H3O+ referred to as you are reading. H3O+ is the hydronium ion and simply means a hydrogen ion has attached to the water molecule.
For all intents and purposes, H3O+= H+ .

9. pH, pOH, [H+ ], [OH-]
You don’t have to understand logarithms to find pH.
It’s as easy as pushing a button on your calculator!
Ex: Find the pH of a solution with an [ H+ ] = 4.2 x 10-5 M.
In your calculator: (-) log 4.2 x and enter/ =.
The pH = Note that pH and pOH values do not have units on them. H+ and OH- have units of molarity as they are concentrations.

10. pH, pOH, [H+ ], [OH-]
A p function always means to take the negative logarithm of the term.
pH = - log [H+]
pOH = - log [OH-]
pH and pOH are related
pH + pOH = 14
If you know one value, you can find the other by subtracting from 14.

11. pH, pOH, [H+ ], [OH-] Water exists in equilibrium with its ions.
H2O (l)  H+ (aq) + OH- (aq)
We can write a relationship of the two ions called Kw.
Kw = 1 x = [ H+ ] [ OH- ]
This means that if you know one ion concentration, the other can easily be found by substitution into the equality to solve.

12. Finding [ H+ ] given pH
If you are given pH, you can work backwards to find the hydrogen ion concentration.
Ex: The pH of a solution is What is the [ H+ ]
pH = - log [H+]
10.8 = - log [H+] divide through by -1
-10.8 = log [H+]
On your calculator, push 2nd/shift log (-) You are raising 10 to the power of You find the [ H+ ] = 1.58 x M.