1. Acids and Bases

2. Acids: Compounds that contain. one or more hydrogen ions
Acids: Compounds that contain one or more hydrogen ions (H+) when dissolved in water
Bases: Compounds that contain one or more hydroxide ions (OH-) when dissolved in water

3. Arrhenius Acid
A substance that dissociates in water to form hydrogen ions (H+); that is, an acid increases the concentration of H+ ions in an aqueous solution

4. Arrhenius Base
a substance that dissociates in water to form hydroxide (OH−) ions; that is, a base increases the concentration of OH− ions in an aqueous solution.

5. Bronsted-Lowry Acid
A molecule or ion that is able to lose, or "donate," a hydrogen cation (proton, H+)
acid+base  conjugate base+conjugate acid.
The conjugate base is the ion or molecule remaining after the acid has lost a proton, and the conjugate acid is the species created when the base accepts the proton. The reaction can proceed in either forward or backward direction; in each case, the acid donates a proton to the base.

6. Bronsted-Lowry Base
Substance with the ability to gain, or "accept," a hydrogen cation (proton, H+).

7. Properties of Acids Acids taste sour Acids have a pH lower than 7
Acids effect indicators
Blue litmus turns red
Universal indicator turns red
Acids are proton (hydrogen ion, H+) donors
Acids react with active metals, produce H2
Acids react with carbonates
Acids neutralize bases

8. Acids Have a pH less than 7

9. Acids React with Active Metals
Acids react with active metals to form salts and hydrogen gas.
Mg + 2HCl  MgCl2 + H2(g)

10. Acids Neutralize Bases
HCl + NaOH  NaCl + H2O
Neutralization reactions ALWAYS produce a salt and water.

11. Acids you must know: Strong Acids Weak Acids Sulfuric acid, H2SO4
Phosphoric acid, H3PO4
Hydrochloric acid, HCl
Acetic acid, HC2H3O2
Nitric acid, HNO3

12. Sulfuric Acid Used in the production of paper
Highest volume production of any chemical in the U.S.
Used in the production of paper
Used in production of fertilizers
Used in petroleum refining

13. Nitric Acid Used in the production of fertilizers
Used in the production of explosives
Nitric acid is a volatile acid – its reactive components evaporate easily
Stains proteins (including skin!)

14. Hydrochloric Acid Used in the pickling of steel
Used to purify magnesium from sea water
Part of gastric juice, it aids in the digestion of protein
Sold commercially as “Muriatic acid”

15. Phosphoric Acid A flavoring agent in sodas
Used in the manufacture of detergents
Used in the manufacture of fertilizers
Not a common laboratory reagent

16. Acetic Acid Used in the manufacture of plastics
Used in making pharmaceuticals
Acetic acid is the acid present in vinegar

17. Acids are Proton Donors
Monoprotic acids
Diprotic acids
Triprotic acids
HCl
H2SO4
H3PO4
HC2H3O2
H2CO3
HNO3

18. Ionization of HCl and formation of hydronium ion, H3O+
H2O + HCl 
H3O+ + Cl-
Proton
acceptor
Proton
donor

19. Strong Acids vs. Weak Acids
Strong acids are assumed to be 100% ionized in solution (good proton donors).
HCl
H2SO4
HNO3
Weak acids are usually less than 5% ionized in solution (poor proton donors).
H3PO4
HC2H3O2
Organic acids

20. Strong Acid Dissociation

21. Weak Acid Dissociation

22. Effects of acid on the Environment
Rainwater is naturally acidic WHY? When CO2 (gas) + H2O H2CO3 (aqueous) react they form Carbonic acid Carbon dioxide (from the air) dissolves in rainwater, producing carbonic acid, a weak acid The normal pH of rainwater is about 5.6

23. Effects of acid on the Environment
Acid rain is rain with a pH less than 5.
Forms when air-polluting gases dissolve in
Rainwater
Sulfur dioxide (SO2) Further lowers the pH of rain.

24. Effects of acid on the Environment
Environmental Impact of Acid Rain
Dependent on local geology
Hill Country soil is rich in limestone (CaCO3), which is basic
Limestone neutralizes the effect of acid rain on lakes

25. Damages Caused by Acid Rain 1) Damage to aquatic life
In some sensitive lakes and streams, acidification has completely eradicated
fish species, such as the brook trout, leaving these bodies of water barren. Hundreds of the lakes in the Adirondacks have acidity levels unsuitable for the survival of fish

26. Damages Caused by Acid Rain (Cont.) 2.) Damage to vegetation

27. Damages Caused by Acid Rain (Cont
Damages Caused by Acid Rain (Cont.) 3) Damage to outdoor artwork (monuments & statues)

28. Properties of Bases Bases taste bitter Bases have a pH greater than 7
Bases effect indicators
Red litmus turns blue
Universal indicator turns blue
Phenolphthalein turns purple
Bases are proton (H+) acceptors
and usually have hydroxide ions- OH-
Solutions of bases feel slippery
Bases neutralize acids

29. Examples of Bases Sodium hydroxide (lye), NaOH
Potassium hydroxide, KOH
Magnesium hydroxide, Mg(OH)2
Calcium hydroxide (lime), Ca(OH)2

30. Bases Effect Indicators
Red litmus paper turns blue in contact with a base.
Phenolphthalein turns purple in a base.

31. Bases have a pH greater than 7

32. Bases Neutralize Acids
Milk of Magnesia contains magnesium hydroxide, Mg(OH)2, which neutralizes stomach acid, HCl.
2 HCl + Mg(OH)2
MgCl2 + 2 H2O

33. Products of Neutralization
HCl + NaOH 
NaCl + H2O
H2SO4 + Ca(OH)2 
CaSO H2O
HNO3 + KOH 
KNO3 + H2O
The products of neutralization are always a ______ and _______.
salt
water