ACIDS AND BASES

Acids Bases Operational Definitions (properties) A. Electrolytes Strong acids: completely dissociate into ions (hydrochloric, nitric, sulfuric, hydrobromic, and hydroiodic) Weak acids: do not completely dissociate into ions. (all other acids) Operational Definitions (properties) A. Electrolytes Strong bases: completely dissociate into ions. (soluble hydroxides on table F) Weak bases: do not completely dissociate into ions. (insoluble hydroxides on table F)

Acids Bases B. Taste sour Ex: citric acid in oranges Lactic acid in milk B. Taste bitter, feel soapy and slippery

C. Change the color of acid-base indicators. (table M) Acids pH: between 1 & 7 Litmus: red stays red, blue turns red Bromothymol blue: Yellow Phenolphtalein: Clear Bases Between 7 and 14 Red turns blue, blue stays blue Blue Pink

D. Undergo neutralization Acid + Base →Salt + Water ex: HCl + NaOH→NaCl + HOH

Acid Bases E. Metal + acid →salt + hydrogen Use table J (only metals above hydrogen can replace it) Ex: Mg + 2HCl→MgCl2 + H2 E. Emulsify (breaks down) fats and oils

Acids Bases Conceptual definitions (explanations) A. Arrhenius: Acids contain the hydrogen ion or hydronium ion as the only positive ion. Table K Ex: HCl, HBr, HF Conceptual definitions (explanations) A. Arrhenius: Bases contain the hydroxide ion as the only negative ion. Table L Ex: NaOH (note: first element is a metal)

Acids Bases B. Bronsted-Lowry: An acid is a proton donor Example: NH3 + H2O → NH4+ Base 1 + acid 2 B. Bronsted-Lowry A base is a proton acceptor NH4+ + OH- Acid 1 + base 2

Acids Bases C. Lewis: Electron Pair Acceptor C. Lewis: Electron Pair Donor

Acids Bases Additional information: Monoprotic (1H: HCl) Diprotic (2H: H2SO4) Polyprotic (more than 2H: H3PO4) Additional information: Amphiprotic or amphoteric: acts as either an acid or a base. Example: H2O and HSO4-

Acids Bases Naming acids Binary acids: H nonmetal Hydro stem of nonmetal ic acid Ex: HCl: hydrochloric Ternary acids H – polyatomic ion Table E ate becomes ic acid and ite becomes ous acid Example: H2SO4 : sulfuric acid (no hydro) Naming bases Name the metal (use a roman numeral if a metal has more than one oxidation number) followed by hydroxide Example: KOH: potassium hydroxide