1. They are everywhere.. In your food In your house EVEN IN YOU!!!!!
Acids & Bases
They are everywhere..
In your food
In your house
EVEN IN YOU!!!!!

2. What is an acid?
An acid is a solution that has an excess of H+ ions. It comes from the Latin word acidus that means "sharp" or "sour".
The more H + ions, the more acidic the solution.

3. Properties of an Acid Tastes Sour Conduct Electricity
Corrosive, which means they break down certain substances. Many acids can corrode fabric, skin,and paper
Some acids react strongly with metals
Turns blue litmus paper red
“Blue to red A-cid”
Picture from BBC Revision Bites

4. Uses of Acids Acetic Acid = Vinegar
Citric Acid = lemons, limes, & oranges. It is in many sour candies such as lemonhead & sour patch.
Ascorbic acid = Vitamin C which your body needs to function.
Sulfuric acid is used in the production of fertilizers, steel, paints, and plastics.
Car batteries

5. What is a base? A base is a solution that has an excess of OH- ions.
Another word for base is alkali.
Bases are substances that can accept hydrogen ions

6. Properties of a Base Feel Slippery Taste Bitter Corrosive
Can conduct electricity. (Think alkaline batteries.)
Do not react with metals.
Turns red litmus paper blue.
“basic blue”

7. Uses of Bases
Bases give soaps, ammonia, and many other cleaning products some of their useful properties.
The OH- ions interact strongly with certain substances, such as dirt and grease.
Chalk and oven cleaner are examples of familiar products that contain bases.
Your blood is a basic solution.

8. pH Scale pH is a measure of how acidic or basic a solution is.
The pH scale ranges from 0 to 14.
Acidic solutions have pH values below 7
A solution with a pH of 0 is very acidic.
A solution with a pH of 7 is neutral.
Pure water has a pH of 7.
Basic solutions have pH values above 7.

9. Acid Nomenclature Review
No Oxygen
w/Oxygen
An easy way to remember which goes with which…
“In the cafeteria, you ATE something ICky”

10. Acid/Base definitions Definition 1: Arrhenius
Arrhenius acid is a substance that produces H+ (H3O+) in water
Arrhenius base is a substance that produces OH- in water
4.3

11. Acid/Base Definitions
Definition: Brønsted – Lowry
Acids – proton donor
Bases – proton acceptor
A “proton” is really just a hydrogen atom that has lost it’s electron!

12. A Brønsted-Lowry acid is a proton donor
A Brønsted-Lowry base is a proton acceptor
conjugate acid
conjugate base
base
acid

13. ACID-BASE THEORIES
The Brønsted definition means NH3 is a BASE in water — and water is itself an ACID

14. Conjugate Pairs

15. Learning Check! HCl + OH-  Cl- + H2O H2O + H2SO4  HSO4- + H3O+
Label the acid, base, conjugate acid, and conjugate base in each reaction:
HCl + OH-    Cl- + H2O
Acid
Base
Conj.Base
Conj.Acid
H2O + H2SO4    HSO4- + H3O+
Conj.Base
Conj.Acid
Base
Acid

16. Lewis Acids & Bases
Formation of hydronium ion is also an excellent example.
Electron pair of the new O-H bond originates on the Lewis base.

17. pH = - log [H+] Calculating the pH ([ ] means Molarity)
Example: If [H+] = 1 X pH = - log 1 X 10-10
pH = - (- 10)
pH = 10
Example: If [H+] = 1.8 X 10-5 pH = - log 1.8 X 10-5
pH = - (- 4.74)
pH = 4.74

18. Try These! pH = - log [H+] pH = - log 0.15 pH = - (- 0.82) pH = 0.82
pH = - log 3 X 10-7
pH = - (- 6.52)
pH = 6.52
Find the pH of these:
A 0.15 M solution of Hydrochloric acid
2) A 3.00 X 10-7 M solution of Nitric acid

19. pOH Since acids and bases are opposites, pH and pOH are opposites!
pOH does not really exist, but it is useful for changing bases to pH.
pOH looks at the perspective of a base
pOH = - log [OH-]
Since pH and pOH are on opposite ends,
pH + pOH = 14

20. pH
[H+]
[OH-]
pOH

21. [H3O+], [OH-] and pH What is the pH of the 0.0010 M NaOH solution?
[OH-] = (or 1.0 X 10-3 M)
pOH = - log
pOH = 3
pH = 14 – 3 = 11
OR Kw = [H3O+] [OH-]
[H3O+] = 1.0 x M
pH = - log (1.0 x 10-11) = 11.00

22. pH Scale
A change of 1 pH unit represents a tenfold change in the acidity of the solution.
For example, if one solution has a pH of 1 and a second solution has a pH of 2, the first solution is not twice as acidic as the second—it is ten times more acidic.

23. Acid – Base Reactions
A reaction between an acid and a base is called neutralization. An acid-base mixture is not as acidic or basic as the individual starting solutions.

24. Acid – Base reactions
Each salt listed in this table can be formed by the reaction between an acid and a base.