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.

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

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

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

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

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

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.

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.

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.

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.