1. Acids and Bases

2. Acids and Bases Give off hydrogen (H+) ions in solution Properties
Taste sour
Conducts electricity
Feels like water but can burn
Turns blue litmus paper RED
Gives of hydroxide ions (OH-) in solution
Properties
Tastes bitter
Conducts electricity
Feels soapy/slippery
Turns red litmus paper BLUE

3. Both acids and bases Are considered electrolytes
Become ions when dissolved in water a process called ionization.
STRONG ACIDS or STRONG BASES ionize almost completely. Weaker ones don’t (AKA. All of the particles don’t break up into ions, some stay the way they were)

4. Definitions
Indicator – a substance that has a specific kind of color reaction – it “indicates” what the other substance is
Concentration – the relative amount of one substance present in another (concentration of H+ ions and OH- ions range from 100 to 10-14)
NOTE – concentrated versus dilute is different than weak versus strong

5. pH scale
A mathematical scale that represents the concentration of hydronium ions with a range of (in water, the extra H+ ions are picked up by H2O and make H3O+ which is the hydronium ion). The more H+ ions that are present the lower the pH.

6. pH (with universal indicator)

7. Conversions between pH and Concentration
pH 3 = 10-3 M = 1 x 10-3 M = M
Convert the following pH to concentration:
pH = 4
pH = 9
pH = 7
Convert the following concentrations to pH:
1 x 10-6 M
1 x M
1 x 10-1 M
3) Label all 6 as Acid, Base, or Neutral

8. Which acid would have a higher concentration of hydronium ions, lemon juice with a pH of 3 or tomato juice with a pH of 5?
What pH would a substance have if it’s concentration of H+ is 10 -4? Is it an acid or base?

9. What no explosion?
No, it won’t explode when I mix an acid with a base. What will happen, you ask?
NOTES -
Mixing an acid with a base will produce a salt and water.
The acid and base NEUTRALIZE each other.
NaOH + HCl → NaCl + H2O
Is this equation balanced? How many moles of each substance are used?

10. Naming Acids and Bases Acids: Ending changes and some prefixes change.
H bonded to a monatomic ion = Hydro ________ ic acid
example HF = Hydrofluoric acid
H bonded to an -ate polyatomic ion = __________ic acid
HNO3 = nitric acid
H bonded to an -ite polyatomic ion = __________ous acid
HNO2 = nitrous acid
Bases: Name the metal then Hydroxide
example: LiOH = Lithium Hydroxide