1. Ch. 15 – Acids & Bases
ACIDS – Have a H+ ion (Hydronium ion)
Corrosive
pH lower than 7
Electrolyte
Sour taste
Mix acid to water to dilute; never mix water to acid.

2. Hydrochloric acid – HCl Phosphoric acid – H3PO4 Sulfuric acid – H2SO4
Common Acids
Nitric acid – HNO3
Hydrochloric acid – HCl
Phosphoric acid – H3PO4
Sulfuric acid – H2SO4
Carbonic acid – HCO3
Acetic acid – HC2H3O2

3. Phosphoric acid
Flavor agent in beverages
Acetic acid
5% of vinegar
Fermentation product in juices, wines, & beer
Hydrochloric acid
Stomach acid
Used to pickle metals

4. Nitric acid
Making explosives
Turns skin yellow – protein indicator
Sulfuric acid
Strongest acid
Used in car batteries
Dehydrating agent (anhydrous)

5. Bases Base – has an OH- ion (hydroxide ion) Corrosive pH higher than 7
Electrolyte
Bitter taste
Pink with phenophalthene as an indicator
H+ & OH- ions tend to neutralize each other out  Neutralization

6. Common Bases Lithium hydroxide – LiOH  strong
Calcium hydroxide – Ca(OH)2  weak
Sodium hydroxide – NaOH  strong
Lye & drain cleaner
Potassium hydroxide – KOH  strong
Magnesium hydroxide – Mg(OH)2  weak
Ant-acid

7. A substance with OH- form a soluble base is called an alkaline.
An acid with a compound of H, O, & a third element is called an Oxyacid.
Ex. HNO3, H2SO4
NH4 is the only base without OH in it.

8. Basic anhydride is an oxide that reacts with water to form an alkaline solution.
A base without water
Takes water out of a substance when it come in contact with it.
Very strong bases (lye)
The stronger the base the more anhydric it is.

9. Acid anhydride is an oxide that reacts with water to form an acid.
An acid without water
Takes water out of substances when it comes in contact with them.
Very strong acids (sulfuric acid)
The stronger the acid the more anhydric it is.

10. ACIDS & BASES COMBINE TO FORM A SALT & WATER.
NaOH + HCl  H2O + NaCl
HCl + LiOH  H2O + LiCl
Amphoteric is any solution that can react as either an acid or a base.