Acids  Arrhenius definition  Produces H + ions in aqueous solutions  Some completely dissociate, others partially dissociate in solutions

1) Strong Acids1) Strong Acids  Completely dissociate into ions in an aqueous solution, only a few acids  Strong electrolytes  [acid] = [ion concentration] in solution, no molecules left  HCl, HBr, HI, HNO 3, H 2 SO 4, HClO 4 (KNOW THEM!!!)  Ex. HBr

Ex. 1 HBrEx. 1 HBr

2) Weak Acids2) Weak Acids  Partially dissociate in an aqueous solution  Weak electrolytes  Some molecules break up into ions, other molecules stay together in solution  [weak acid] ≠ [ion]  Ex. CH 3 COOH

Ex. 2 CH 3 COOHEx. 2 CH 3 COOH

Multiple IonizationsMultiple Ionizations  Some acids can donate more than one H + ion and go through multiple ionizations  H 3 PO 4 and H 2 SO 4

How do we recognize acids in chemical formulas?  1) H + ion appears 1 st in chemical formula.  Ex. HCl, H 2 SO 4  2) H atom location in structural formula  Usually at the end  Indicates atom bonded to H  Ex. CH 3 COOH

Bases  Arrhenius definition  Produces hydroxide (OH - ) ions in aqueous solutions  Some completely dissociate, others partially dissociate in solutions

1) Strong Bases1) Strong Bases  Completely dissociate into ions in aqueous solutions  Strong electrolytes, mainly ionic compounds  [strong base] = [ion] in solution  Most Group IA and IIA metals combined with hydroxide ion  LiOH, NaOH, KOH, RbOH, CsOH, Mg(OH) 2, Ca(OH) 2, Sr(OH) 2, Ba(OH) 2 –KNOW THEM ! ! !

2) Weak Bases2) Weak Bases  Partially dissociate in an aqueous solution  Weak electrolytes, typically molecular compounds  Some molecules break up into ions, other molecules stay together in solution  [weak base] ≠ [ion]  Do not necessarily have hydroxide (OH - ) ion in chemical compound  React with water and produce the hydroxide ion as a product.

2) Weak Bases (cont.)2) Weak Bases (cont.)  Ex. NH 3

How do we recognize bases in a chemical formula? 1) Ionic Compound with metal cation + hydroxide (OH - ) anion  Strong base 2) Molecular compound has OH covalently bound, not existing as OH - ion  Consisting of nonmetals  Rely on chemical equation to show ionization  Most common weak bases: ammonia (NH 3 ) and amines (R-NH 2 )

Neutralization ReactionsNeutralization Reactions  Acids and bases cancel each other out, “neutralize” or even out the solution  ACID + BASE SALT + H 2 O  How do we determine when a solution is neutral?  Check pH with litmus paper, color changes  Acid/base indicator – compound where its color is influenced by the [H + ] and [OH - ] in solution

Special Net-Ionic Equations with Acids and Bases NH 3  Produces ammonium ion when combined with an acid, slightly basic  Acid-Base reaction, but no OH - ion released  HA + NH 3 NH 4 +