1. Chapter 14: Acids and Bases and pH

2. Acids are proton donors (give a hydrogen away)
1) Sour taste
2) Litmus paper (common indicator) changes from blue to red in an acid or red litmus paper stays red.
3) Acids always contain hydrogen.
Acids are proton donors (give a hydrogen away)
Bronsted-Lowry definition of an acid
4) Acids react with metals to form hydrogen gas
and a metal compound called corrosion

3. HCl(g) + H2O (l) ----- H3O+ (aq) + Cl- (aq)
Acids – produce hydronium ions in water.
HCl(g) + H2O (l) ----- H3O+ (aq) + Cl- (aq)
Also known as Arrhenius Acids
When a hydrogen atom is attached to a water molecule. Hydronium ion: H3O+ ion is positively charged.
Conduct an electrical current (charged particles).
Hydrogen is always written first in an acid.
If there is Only one hydrogen – HCl – monoprotic
Diprotic (2) and polyprotic (more than 2)
Example: H2SO4 – sulfuric acid - diprotic

4. Note: if hydrogen is not written first – not an acid!
BUT not all hydrogen containing compounds are acids.
Example: sugar C11H22 O11
Note: if hydrogen is not written first – not an acid!

5. Bases
1) taste bitter, feel slippery
2) turn litmus paper from red to blue or blue paper stays blue.
3) emulsify (dissolve) fats and oils
Arrhenius bases produce hydroxide ion (OH-) when dissolved in water. (need to know name and symbol)
5) Bases are called proton acceptors
Proton acceptors- Bronsted – Lowry definition of a base

6. NaOH (s) ------- Na+ (aq) + OH- (aq) OH- hydroxide ion
Common Base - Sodium Hydroxide (NaOH) also known as ‘lye’ common base – very strong.
NaOH (s)  Na+ (aq) OH- (aq)
OH- hydroxide ion
Example: NH3 (g) + H2O (l) --- NH4+ (aq) + OH- (aq)
Ammonia – covalent base
Water does play a role in this reaction
Since NH3 accepts a proton (H+) and is now NH4+ it is considered a base.
H2O

7. 14.2 Strengths of Acids and Bases
Strong Acids and Bases Completely ionize in water

8. Common acids – know these Strong: H2SO4 – sulfuric acid
HNO3 – nitric acid
HCl – hydrochloric acid
– highest production of any acid in the United States. Used in the production of paper, fertilizers, petroleum refining and car batteries.
used in the production of rubber, plastics, pharmaceuticals, fertilizers and explosives
used in the pickling of steel, used to purify magnesium from sea water, correct swimming pool pH, found in your gastric juices (aids in the digestion of proteins) Sold commerically as “Muriatic Acid”

9. Strong acids :
ionize well in water (lose hydrogen quickly) = good electrolytes

10. Weak acids:
HC2H3O2 – acetic acid (acid in vinegar) know this one
H2CO3 – carbonic acid (used for carbonating soda)
H3PO4 – phosphoric acid (a flavoring agent in soda)
H3BO3 – boric acid (eye wash)
Weak acids do not ionize well in solution (produce only a few H+ in solution)
Poor Electrolytes!
Acetic acid

11. Common Bases –
Strong bases ionizes completely in water, produce large # of ions therefore Good Electrolytes.
Strong Bases:
KOH – battery electrolyte
NaOH – used for making soap, Drano; know this one
Ca(OH)2 – leather production, making plaster
Mg(OH)2 – laxative, antacid

12. Weak Bases: do not produce large amount of ions, weak electrolytes.
NH4OH – ammonium hydroxide (household cleaner)
Al(OH)3 – aluminum hydroxide (antacid, deodorant)
NH3 Ammonia – household cleaning products
know this one

13. pH scale is used to measure the acidity of solution.
Definition:
The pH (‘potential of hydrogen’) is a measure of hydronium ion (H3O+)concentration.
It is a Mathematical scale 0-14.
Logarithmic Scale – based on powers of 10.
Example: pH of 3 is 10 times more acidic than a pH 4.
pH of 3 is 100 (10 x 10) times more acidic than the pH of 5.

14. 7 = neutral (distilled water)
pH less than 7 = acidic
pH above 7 = basic
7 = neutral (distilled water)
To calculate pH scale = take the negative
of the exponent of the
hydronium ion concentration = -log [H3O+]
Concentrations of hydronium and hydroxide in water:
[H3O+] x [OH-] = 1 x
Example: If concentration of the hydronium ion [H3O+] is 10-8 M. Then the solution has a pH of 8.
Example: If the hydroxide ion [OH-] concentration is 10-5 M, then the pH = / =  pH of 9.

15. pH of common materials showing the relationship between pH and the hydronium ion concentration.
Pure water has a pH of 7.0. show demo
Normal rain is slightly acidic because carbon dioxide (CO2) dissolves into it forming weak carbonic acid, giving the resulting mixture a pH of approximately 5.6 at typical atmospheric concentrations of CO2.
As of 2000, the most acidic rain falling in the U.S. has a pH of about 4.3.

16. Neutral Solution: [H3O+] = [OH-] Acid Solution: [H3O+] > [OH-]
Gizmo - pH
Neutral Solution: [H3O+] = [OH-]
Acid Solution: [H3O+] > [OH-]

17. 15.1 Acid and Base Reactions
The reaction between an acid and a base is called a Neutralization Reaction.
Usually neutralization reactions produce water and a salt.
NaOH (aq) + HCl (aq)  NaCl (aq) + H2O (l)
pH = 7

18. Salt – Ionic compound formed from the negative part of the acid and the positive part of the base. Neutral substance.
NaCl is not the only ionic compounds that are salts. Others include: KCl, KBr, NH4NO3

19. Indicators are used to test whether a substance is an acid or a base.
Phenolphthalein – common indicator, colorless in an acid; pink in a base.
pink in a base.
colorless in an acid