Chemistry Acids and Bases Unit Notes
Properties of Acids & Bases
Property
Majority of
ions present
Acids
pH range
Indicators
Taste
Reactivity
Electrolyte?
Examples
The pH Scale
• The “Potential of _____________”
•
Used to ____________ convey the acidity of a solution
Acid Base Theories
Arrhenius Theory
 Arrhenius acids increase [___] in aqueous solution
▫

[H+] = __________ ion concentration
Arrhenius bases increase [____] in solution
▫
[OH-] = __________ ion concentration
▫
ALL Arrhenius bases ______ contain hydroxide!
Bases
Bronsted-Lowry Theory
•
Bronsted-Lowry Acids ______ protons
▫
A proton is just _____!
•
Bronsted-Lowry Bases ________ protons
•
_______ Arrhenius bases are Bronsted-Lowry, but _____ _____ Bronsted-Lowry bases are
Arrhenius!
Ex. NaOH is a base according to Arrhenius and B-L, but NH3 is only a base according to B-L,
not Arrhenius.
Strength vs. Concentration
•
The ____________________ of an acid or base is simply its molarity
▫
•
Molarity (M) =
The _________________ of an acid or base is determined by the percent it ____________ in
solution
▫
Weak does ________ _________ harmless!!! You can have a very
weak but harmful acid.
▫
HF is ___________, but it sure looks painful!
STRONG Acids and Bases
Ionization
Ions
WEAK Acids and Bases
Strong or Weak???
H2SO4
HNO3
HClO4
HClO3
HCl
HBr
HI
Strong Acids
Sulfuric acid
Nitric acid
Perchloric acid
Chloric acid
Hydrochloric acid
Hydrobromic acid
Hydroiodic acid
Ca(OH)2
Sr(OH)2
Ba(OH)2
LiOH
NaOH
KOH
RbOH
CsOH
Strong Bases
Calcium hydroxide
Strontium hydroxide
Barium hydroxide
Lithium hydroxide
Sodium hydroxide
Potassium hydroxide
Rubidium hydroxide
Cesium hydroxide
Practice:
1. Arrhenius acids increase ______ ions when dissolved in water.
2. Arrhenius bases increase _____ ions when dissolved in water.
3. BrØnsted-Lowry acids ______ protons (H+) when dissolved in water.
4. BrØnsted-Lowry bases ______ protons (H+) when dissolved in water.
5. True or False: A concentrated weak acid can be just as harmful as a diluted strong acid.
6. If only 50% HF acid ionizes in water, it is a (strong/weak) acid.
7. If 100% of the base KOH ionizes in water, it is a (strong/weak) base.
Check the appropriate box for each substance in the chart below:
Substance
HC2H3O2 (acetic)
NH4OH
Mg(OH)2
HCl
H2O
HOH
Al(OH)3
HC7H5O3 (salicylic)
Acid
Base
Naming and Formulas of Acids
•
Almost all acids have 1 or more ___________ listed first
HCl
HNO2
HNO3
Carbonic acid
Hydrocyanic acid
Chlorous acid
Naming and Formulas of Bases
Since bases are __________________ compounds, they are named in the usual way:
NH4OH is _______________________________
Al(OH)3 is _______________________________
Practice!!!
Name the following acids and bases:
1)
NaOH ____________________________________
2)
H2SO3 ____________________________________
3)
H2S _______________________________________
4)
H3PO4 ____________________________________
5)
HCl _______________________________________
6)
HI ______________________________________
7)
Ca(OH)2 __________________________________
8)
Mg(OH)2 __________________________________
9)
H3P________________________________________
10)
HClO _____________________________________
Write the formulas of the following acids and bases:
11)
hydrofluoric acid ____________________________
12)
hydroselenic acid ___________________________
13)
carbonic acid ________________________________
14)
lithium hydroxide ___________________________
15)
nitrous acid __________________________________
17)
sulfuric acid _________________________________
19)
hydrobromic acid ___________________________
20)
hydrocyanic acid ___________________________
Calculating pH Notes & Practice
Calculating pH of Acids


To calculate the pH of a solution you
need to know the ________________
_______ concentration.
o [H+]
o You will either be told “the
hydrogen ion concentration is…”
or “the molarity (M) is…..”
To find the pH, you will use the log button on your calculator. Just type it in!!! 
Try these 
1. What is the pH of lemon juice if the hydrogen ion concentration is 0.005 M?
2. What is the pH of a 1.4 x 10-5 M HCl solution?
3. I have a mystery solution with a hydrogen ion concentration of 6.0 x 10-12 M. Find the pH of
this solution, and then identify the solution as acid or base.
Interpreting the relationship between ion concentration and pH:
1. pH refers to the ___________ ion concentration.
2. As the [H+] goes from 1 x 10-2 to 1 x 10-6, the pH goes from ____ to ____.
3. The concentration of the [H+] in question 2 is decreasing, making the solution less _____________.
This also means the [OH-] is going ______________.
4. If the [H+] goes up, the pH will go ______________.
5. If the [OH-] goes up, the pH will go _______________.
6. If the [H+] goes down, the [OH-] must go _____________.
7. When does the [H+] = [OH-] ? ________________________.
Complete the following chart over pH.
Concentration
pH
Acid, Base, or
Neutral?
0.01 M
1.0 x 10-10 M
5.0 x 10-3 M
hydrogen ion = 0.030 M
1 x 10-7 M
[H+] = 0.045
0.0000058 M
0.50 M
hydrogen ion = 0.00138 M
4.4 x 10-5 M
1.50 x 10-11 M
BOX
your answers below.
1. What is the pH of a solution with a [H+] of 5.78 x 10-6 M?
2. What is the pH of a 6.8 x 10-7 M HNO3 solution?
3. Calculate the pH of a solution with a hydrogen ion concentration of 2.1 x 10-4 M.
4. What is the pH of a solution with a hydrogen ion concentration of 3.11 x 10-9 M.
5. What is the pH of a 4.08 x 10-7 M solution?
Neutralization Reactions
Neutralization Reactions

When acids and bases are mixed together, their pH becomes more
______________. Therefore, we call these neutralization reactions.

The products of a neutralization reaction are always _________________
and a ______________.
o A “salt” can be any ________________ compound that dissociates in water.
Acid

+
Base 
Water +
Salt
Neutralization is a ________________________ _________________________ reaction. The
_________ from the acid bonds with the ___________ from the base, to form WATER. The
_____________ from the acid and the _____________ from the base bond to form the SALT.
_____HF
+
_____NaOH
_____H2CO3 +
_____Sr(OH)2
_____Ca(OH)2
+
_____Zn(OH)2
+


_____H3PO4
_____HNO3


Complete the neutralization reactions below.
1. _____HCl
+
2. _____CsOH
3. _____HF
4. _____HCl
_____NaOH 
+
+
+
_____H2CO3 
_____Mg(OH)2 
_____Al(OH)3