1. Chapter 4: Types of Chemical Reactions Goals: To be able to predict chemical reactivity. To know how to synthesize specific compounds.

2. Types of Reactions Acid-Base: proton-transfer Oxidation-Reduction: electron-transfer Precipitation: formation of insoluble salts Gas Forming Organic: –Substitution –Addition –Elimination

3. Reactions in Aqueous Solution Unless mentioned, all reactions studied this and next week occur in aqueous solution.

4. Electrolytes Strong Electrolytes: solute breaks apart to give ions in solution. NaCl  Na + + Cl - Weak Electrolytes: solute partially breaks apart to give ions. CH 3 CO 2 H  CH 3 CO 2 - + H + happens less than 5% Nonelectrolytes: no ions formed. CH 3 CH 2 OH

5. Brønsted-Lowery Acid-Base Definitions An acid is a substance that donates a proton (H + ) to a base A base is a substance that accepts a proton (H + ) from an acid

6. Brønsted-Lowery Definitions An acid is a substance that donates a proton (H + ) to a base A base is a substance that accepts a proton (H + ) from an acid Acid-base reactions can be reversible: reactants  products or products  reactants

7. Brønsted-Lowery Definitions An acid is a substance that donates a proton (H + ) to a base A base is a substance that accepts a proton (H + ) from an acid Acid-base reactions can be reversible: reactants  products or products  reactants

8. Important Acids and Bases Strong Acids: HClhydrochloric HBrhydrobromic HIhydroiodic HNO 3 nitric H 2 SO 4 sulfuric HClO 4 perchloric Weak Acid: CH 3 CO 2 Hacetic Any other acids are WEAK Strong Bases: LiOHlithium hydroxide NaOHsodium hydroxide KOH potassium hydroxide Ca(OH) 2 calcium hydroxide Weak Base: NH 3 ammonia

9. STRONG acids in water: 100% of acid molecules form ions: HCl(aq) + H 2 O(l)  H 3 O + (aq) + Cl - (aq) H 3 O + is hydronium ion

10. WEAK acids in water, ~5% or less of acid molecules form ions (acetic, H 3 PO 4, H 2 CO 3 )

11. Polyprotic Acids multiple acidic H atoms H 2 SO 4  H + + HSO 4 - HSO 4 -  H + + SO 4 2- Not all H’s are acidic: CH 3 CO 2 H

12. If H 3 PO 4 reacts as an acid, which of the following can it not make? 1. H 4 PO 4 + 2. H 2 PO 4 - 3. HPO 4 2- 4. PO 4 3-

13. If C 2 O 4 2- reacts in an acid-base reaction, which of the following can it not make? 1. H 2 C 2 O 4 2. HC 2 O 4 - 3. 2 CO 2

14. Acid-Base Reactions Strong Acid + Strong Base HCl(aq) + NaOH(aq)  NaCl(aq) + H 2 O(l) acid base “salt” water

15. Net Ionic Equations HCl(aq) + NaOH(aq)  NaCl(aq) + H 2 O(l) What really happens: H + (aq) + OH - (aq)  H 2 O(l) Sodium ion and chloride ion are “spectator ions”

16. Reactions involving weak bases HCl(aq) + NH 3 (aq)  NH 4 + (aq) + Cl - (aq) Net-Ionic Equation: NH 3 (aq) + H + (aq)  NH 4 + (aq)

17. CH 3 CO 2 H(aq) + NaOH(aq)  1. CH 3 CO 2 H 2 + (aq) + NaO(aq) 2. CH 3 CO 2 - (aq) + H 2 O(l) + Na + (aq) 3. CH 4 (g) + CO 2 (g) + H 2 O(l)

18. HCN(aq) + NH 3 (aq)  1. NH 4 + (aq) + CN - (aq) 2. H 2 CN + (aq) + NH 2 - (aq) 3. C 2 N 2 (s) + 3 H 2 (g)

19. Solution Concentration: Molarity Molarity = moles solute per liter of solution 0.30 mol NH 3 dissolved in 0.500 L Concentration = Written like: [NH 3 ] = 0.60 M

20. pH Scale In pure water, a few molecules ionize to form H 3 O + and OH – H 2 O + H 2 O  OH – + H 3 O + In acidic and basic solutions, these concentrations are not equal acidic: [H 3 O + ] > [OH – ] basic: [OH – ] > [H 3 O + ] neutral: [H 3 O + ] = [OH – ]

21. pH Scale Measure how much H 3 O + is in a solution using pH pH < 7.0 = acidic pH > 7.0 = basic pH = 7.0 = neutral Measure of H 3 O + and OH – concentration (moles per liter) in a solution As acidity increases, pH decreases

22. pH Scale The pH scale is logarithmic: 10010 2 log(10 2 ) = 2 1010 1 log(10 1 ) = 1 110 0 log(10 0 ) = 0 0.110 –1 log(10 –1 ) = –1 0.0110 –2 log(10 –2 ) = –2The pH scale is logarithmic: 10010 2 log(10 2 ) = 2 1010 1 log(10 1 ) = 1 110 0 log(10 0 ) = 0 0.110 –1 log(10 –1 ) = –1 0.0110 –2 log(10 –2 ) = –2 pH= –log [H 3 O + ]pH= –log [H 3 O + ] pH if [H 3 O + ] = 10 –5 ? 10 –9 ? Acidic or basic?pH if [H 3 O + ] = 10 –5 ? 10 –9 ? Acidic or basic? pH if [H 3 O + ] = 0.000057 M?pH if [H 3 O + ] = 0.000057 M?

23. [H 3 O + ] from pH Finding [H 3 O + ] from pH [H 3 O + ] = 10 -pH What is [H 3 O + ] if pH = 8.9?

24. pH: Quantitative Measure of Acidity Acidity is related to concentration of H + (or H 3 O + ) pH = -log[H 3 O + ]