I. Introduction to Acids & Bases Acids & Bases

A. Properties  electrolytes  sour taste  react with metals to form H 2 gas  slippery feel  bitter taste ChemASAP  vinegar, milk, soda, apples, citrus fruits  ammonia, lye, antacid, baking soda

B. Definitions  Arrhenius - In aqueous solution… HCl + H 2 O  H 3 O + + Cl – AcidsAcids form hydronium ions (H 3 O + ) H HHHH H Cl OO – + acid

B. Definitions  Arrhenius - In aqueous solution… BasesBases form hydroxide ions (OH - ) NH 3 + H 2 O  NH OH - H H H H H H N NO O – + H H H H base

B. Definitions  Brønsted-Lowry HCl + H 2 O  Cl – + H 3 O + AcidsAcids are proton (H + ) donors. BasesBases are proton (H + ) acceptors. conjugate acid conjugate base baseacid

B. Definitions H 2 O + HNO 3  H 3 O + + NO 3 – CBCAAB

B. Definitions - can be an acid or a base.  Amphoteric - can be an acid or a base. NH 3 + H 2 O  NH OH - CACBBA

B. Definitions F - H 2 PO 4 - H2OH2O HF H 3 PO 4 H 3 O +  Give the conjugate base for each of the following: - an acid with more than one H +  Polyprotic - an acid with more than one H +

B. Definitions Br - HSO 4 - CO 3 2- HBr H 2 SO 4 HCO 3 -  Give the conjugate acid for each of the following:

C. Neutralization Reactions  Acids react with bases to produce a salt and water NaOH (aq) + HCl(aq) → NaCl + H 2 O base acid salt water Ca(OH) HCl → CaCl 2 + 2H 2 O base acid salt water

C. Neutralization Salt  Acid + Base  Salt + Water  HCl + NaOH  NaCl + HOH salt water

Acids  Acids can be recognized because the start with H  Examples HCl H 2 SO 4 HI

Acids  Acids are in aqueous solution (aq)  For the purposes of this class, we will assume that if it begins with H, we will name it according to the rules of naming acids