Acids, Bases & Salts

Naming Acids Binary acids Ternary acids Hydro(first syllable of element)ic acid Ternary acids Replace PAI suffix –ate with –ic Replace PAI suffix –ite with –ous

Name that Acid HF HBr HNO3 H2SO4 H3PO4 CH3COOH We will work mainly with the –ic acids, but you should know that the others exist.

Definitions of Acids Brønsted-Lowry Acids Arrhenius Acids Ionize to form H+ in water Brønsted-Lowry Acids Proton donor HCl + H2O  H3O+ (aq) + Cl- (aq)

? water hydrogen ion “proton” hydronium ion

Ionization of Acids H3PO4 + H2O 3 3H3O+(aq) + PO4-3(aq) CH3COOH + H2O H3O+(aq) + CH3COO-(aq) H3PO4 + H2O 3 3H3O+(aq) + PO4-3(aq) 1 H+ = Monoprotic 2 H+ = Diprotic 3 H+ = Triprotic

H2CO3 KH CH3OH KI Acid? Yes or No An Acid must ionize with H+ as the only positive ion in soln H2CO3 KH CH3OH KI

Acids are electrolytes …because they ionize in water The more ions, the stronger the electrolyte Strong acids completely ionize Form lots of ions Weaker acids do not

Acid dissociation constant Ka Acid dissociation constant Stronger acids larger Ka

. . . Other Acid Characteristics Acids change the colors of indicators blue litmus changes to red pH < 7 can be neutralized by bases Dilute acids taste sour

Characteristics of Bases Arrhenius Base Defined as a substance that provides OH- ions to solution BrØnsted-Lowry Base proton acceptor Ex: NH3 + H2O  NH4+ + OH-

all bases end in hydroxide Naming Bases Name the ca+ion all bases end in hydroxide KOH Mg(OH)2 NH4OH Exception?

NaOH  Na+ + OH - NH4OH  NH4+ + OH - Base ionization Metal ion Group 1 hydroxides are your strongest bases. Polyatomic Ion NH4OH  NH4+ + OH -

Change the colors of indicators Bases never contain carbon Feel Slippery ex. soap Taste bitter Change the colors of indicators Phenolphthalein Red litmus turns blue pH > 7 can be neutralized by acids

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