Acid, Bases and Salts Intro 19-1

1.) Electrolytes A.) solutions which conduct electricity 1.) must have mobile ions B.) Acids, Bases and Soluble Salts 1.) Table K, L, and Table F C.) Salts are ionic compounds

2.) Arrhenius Acid/Base A.) Acids, when dissolved in water produce H + or H 3 O + ions as the only positive ions in solution. B.) Bases, when dissolved in water produce OH - ions as the only negative ions in solution. C.) Examples – 1.) acids= H and a negative ion (aq), HNO 3 (aq), HCl(aq), CH 3 COOH(aq) – 2.) bases= metal-OH, or NH 3 (aq), KOH(aq), Ca(OH) 2 (aq) (NOT ALCOHOLS)

3.) Brǿnsted-Lowry (alternative theory) A.) Acids are proton donors B.) Bases are proton acceptors C.) find the acids and bases in the following reaction and explain the movement of protons: NH 3 + H 2 O  NH OH -

D.) Conjugate Acid Base Pairs are acids and bases on opposite sides of a reaction. E.) A conjugate acid has an extra H. F.) A conjugate base has one less H. G.) What is the conjugate base of NH 3 ? H.) what is the conjugate acid of HSO 4 - ?

3.) Amphiprotic A.) definition: able to donate an H, and accept an H (Can act as an acid or a base) B.) examples NH 3, H 2 O, HSO 4 - C.) not examples: CN -, PO 4 -3