This document defines acids and bases and their key characteristics. It explains that acids lower the pH of solutions below 7 while bases raise the pH above 7. Acids can donate protons while bases can accept them. Strong acids and bases ionize completely while weak ones only ionize partially. Indicators are used to detect the presence of acids and bases based on color changes. Different models like Arrhenius, Brønsted-Lowry, and Lewis are presented to describe acids and bases. Examples of common acids and bases along with their pH levels are also provided.

1. Acids and Bases
By: Fernando Dueñas, Juan Pablo, and Héctor Abraham

2. Whats is an acid?
• An acid is a substance, and when it´s combined with a solution gives the
solution a pH lower than 7.

3. What is a base?
• A base is a substacnce that gives the solution a pH greater than 7.

4. Water, acid or base?
• Water, can be both an acid or a base. It can be consider an acid in some
cases and a base in some others, this is called Amphoteric.

5. Conjugate acid and conjugate base
• Acids can release protons and bases can accept them.

6. Conjugate Base
• When the acid releases a proton is able to acept one, so it can act like a base,
a Conjugate Base is an acid that can act like a base.

7. Conjugate Acid
• When the base accepts a proton is able to release it, so it can act like an acid,
a Conjugate Acid is a base that can act like a acid.

8. Ionization
• Ionization is a porcess in which a molecule separes into it´s ions.

9. Acid
• If an acid ionizes completely becomes a strong acid, but if it ionizes only
partially is a weak acid.

10. Base
• If a base ionizes completely becomes a strong base, but if it ionizes only
partially is a weak base.

11. Indicator
• An indicator is a substance that changes it´s color in the presence of an acid
or a base

12. Models
• The Arrhenius model said that acids almost everytime it contain H+ and
bases always contain OH-.

13. Models
• Lowry’s model: Lowry think of acids as being a proton donor and proton
acceptors, so bases do no need OH-.

14. Models
• Lewis: Lewis said that on a base-acid reactions, acids accept electrons and
bases donate electrons.

15. Physical Properties

16. Chemical properties
• Chemical Properties of acids:
• 1.Acids react with bases to
form salt+water
• 2.Acids are corrosive in nature
• 3. Acids release H+ ions in
water(aqueuos solution)
Chemical Properties of bases:
1.they are corrosive as well
2.reacts with acids to form salt+water
3. Bases release OH- ions in a water
solution

17. Acids and bases
• The acids and bases are two kinds of substances, in a simple way they can
be characterized by the properties manifested.

18. Acids
The acids characteristics are:
 Taste sour.
 Are corrosive to metals.
 Change litmus red.
 Become less acid when mixed with bases.

19. Bases
The bases characteristics are:
 Feel slippery.
 Change litmus blue.
 Become less basics when mixed with acids.

20. [H+] pH Example
Acids 1 X 10
0
0 HCl
1 x 10
-1
1 Stomach acid
1 x 10
-2
2 Lemon juice
1 x 10
-3
3 Vinegar
1 x 10
-4
4 Soda
1 x 10
-5
5 Rainwater
1 x 10
-6
6 Milk
Neutral 1 x 10
-7
7 Pure water
Bases 1 x 10
-8
8 Egg whites
1 x 10
-9
9 Baking soda
1 x 10
-10
10 Tums
®
antacid
1 x 10
-11
11 Ammonia
1 x 10
-12
12 Mineral lime - Ca(OH)2
1 x 10
-13
13 Drano
®
1 x 10
-14
14 NaOH

21. Bibliography
• Carpi, A. (2003, 01). Acids and Bases: An Introduction.VisionLearning. Info
got 06, 2015, de
http://www.visionlearning.com/en/library/Chemistry/1/Acids-and-Bases/58
• (2013, 07). Acids and Bases Are Everywhere. Chem4Kids. Info got 06, 2015,
de http://www.chem4kids.com/files/react_acidbase.html
• Our Notebook.