1. Acids and Bases

2. Definitions Arrhenius – Acid is an H+ donor – Base is an OH- donor Bronsted-Lowrey – Acid is an H+ donor – Base is an H+ receptor Lewis – Acid is an electron pair acceptor – Base is an electron pair donor

3. Classification Oxy acids – H + an oxygen containing polyatomic anion Binary acids – H + a monoatomic anion – OR – H+ a non oxygenated polyatomic anion (ie, CN-)

4. Oxy acids To name: – Name the associated polyatomic anion – Replace –ate with –ic acid – Replace –ite with –ous acid To write the formula – Replace the –ic with -ate and write the polyatomic anion OR – Replace the –ous with –ite and write the polyatomic anion – Balance your charge out with hydrogen

5. Examples HNO 3 H 2 SO 4 H 2 CO 3 HNO 2 H 3 PO 4 H 2 CrO 4 H 2 Cr 2 O 7

6. Binary acids: no oxygen To name: – Prefix is hydro – Name anion with –ic acid ending To write the formula: – Write the H – Write the anion formula or symbol – Balance you charge with the subscripts if necessary

7. Examples HCl HF H 2 S HCN HI

8. pH Measures acidity = -log [H+] 7 is neutral Below 7 is acid, above 7 is base Close to 7 is weaker, farther away from 7 is stronger [H+] = inv log (-pH) pH + pOH = 14

9. Neutralization HCl + NaOH  NaCl + HOH You take the H from the acid and combine it with the OH from the base. That makes water. What’s left is called a salt.

10. Acid strength Refers to percent dissociation Measured by Ka

11. Normality Equivalents / Liter of solution Typically, M x subscript of H or OH = N Need to use normality in titration equation

12. Titration N A X V A = N B X V B

13. Common names Vinegar Acetic acid Battery acid Sulfuric acid Muriatic acid HCl Stomach acid HCl Aqua regia HCl + HNO 3 Aspirin Acetylsalicylic acid

14. HNO 3 HCl H 2 SO 4 Carbonic acid Nitrous acid Chromic acid Hydrocyanic acid