1. Acids: liberate H + ions in solution. Bases: liberate OH - ions in solution. Arrhenius Definitions:

2. An acid-base reaction in which water is formed is called a neutralization.

3. Acids: proton donors Bases: proton acceptors Br ӧ nsted- Lowry Definitions:

4. What volume of 0.20 M NaOH must be added to 25.0 mL of 0.15 M HC 2 H 3 O 2 to neutralize the acid? 25.0 mL acetic acid 1 0.15 mol 1000.0mL1 mole acetic acid 1 mole NaOH1000.0 mL 0.20 mol NaOH =19 mL NaOH Volume of acid present Molarity of acid Mole ratio Upside down molarity of base…1/M b = volume of base needed MaMa VaVa =(1/M b )VbVb MaMa VaVa =MbMb VbVb

5. What volume of 0.20 M NaOH must be added to 25.0 mL of 0.15 M HC 2 H 3 O 2 to neutralize the acid? 25.0 mL acetic acid 1 0.15 mol 1000.0mL1 mole acetic acid 1 mole NaOH1000.0 mL 0.20 mol NaOH = 19 mL NaOH Volume of acid present Molarity of acid Mole ratio Upside down molarity of base…1/M b = volume of base needed MaMa VaVa =(1/M b )VbVb MaMa VaVa =MbMb VbVb Ba(OH) 2 2 9.4 mLBa(OH) 2 2 (If base has 2 hydroxides/formula)

6. M a V a = M b V b (for one to one mole ratio neutralizations) M a V a = 2M b V b (for neutralizations involving bases with 2 hydoxides per FU) 2M a V a = M b V b (for neutralizations involving diprotic acids)

7. What is the molarity of an H 2 SO 4 solution if a volume of 22.3 mL of LiOH (with a concentration of 0.75 M) is needed to neutralize 100.0 mL of it? 2M a V a = M b V b 2M a (100.0 mL) = (0.75 M)(22.3mL) M a = 0.084 M