1. Bronsted Lowry Acid Base

2. Bronsted and Lowry An ACID donates a proton (loses an H+) An ACID donates a proton (loses an H+) A BASE accepts a proton (gains an H+) A BASE accepts a proton (gains an H+)

3. Conjugate Acid Base Pairs When an acid loses its hydrogen, it becomes a base (as it is able to gain a hydrogen again) When an acid loses its hydrogen, it becomes a base (as it is able to gain a hydrogen again) This is known as a conjugate base This is known as a conjugate base

4. At the same time, when a base gains a hydrogen in a reaction, it becomes a conjugate acid At the same time, when a base gains a hydrogen in a reaction, it becomes a conjugate acid Weak acids are found on pages 8 and 9 in your data booklet. The conjugate base formula for each acid is directly right to the acid formula. Each conjugate is the result of a loss of 1 hydrogen. Weak acids are found on pages 8 and 9 in your data booklet. The conjugate base formula for each acid is directly right to the acid formula. Each conjugate is the result of a loss of 1 hydrogen.

5. It is important to note that acids and bases may be noted as salts (ionic compounds) It is important to note that acids and bases may be noted as salts (ionic compounds) When this occurs, you must dissociate the ions and allow the demonstration of the proton transfer (omit the spectator ions) When this occurs, you must dissociate the ions and allow the demonstration of the proton transfer (omit the spectator ions)

6. Example Potassium hydrogen sulfate and sodium acetate are mixed in aqueous solution Potassium hydrogen sulfate and sodium acetate are mixed in aqueous solution

7. Strong acids form Weak Bases A strong acid will have a conjugate base that is weak A strong acid will have a conjugate base that is weak Strong acids lose its proton easily (and therefore will not accept a hydrogen easily) Strong acids lose its proton easily (and therefore will not accept a hydrogen easily)

8. A weaker acid will have a stronger conjugate base A weaker acid will have a stronger conjugate base Weak acids hold their protons more (and therefore will easily accept a hydrogen) Weak acids hold their protons more (and therefore will easily accept a hydrogen)

9. Kw = KaKb Kw is the equilibrium constant for water (1.0 x 10 -14 ) Kw is the equilibrium constant for water (1.0 x 10 -14 ) Ka is the equilibrium constant for acids and can be found on page 8 and 9 in the data booklet Ka is the equilibrium constant for acids and can be found on page 8 and 9 in the data booklet Kb is the equilibrium constant for bases and will have to be calculated using Kw = KaKb Kb is the equilibrium constant for bases and will have to be calculated using Kw = KaKb

10. Acid Reactions HA + H2O  H3O+ + A-

11. Base Reactions

12. Amphiprotic Substances An amphiprotic substance is a chemical species that can donate or accept a proton An amphiprotic substance is a chemical species that can donate or accept a proton Substance must contain a hydrogen to donate Substance must contain a hydrogen to donate Substance must be able to accept a hydrogen (usually have a negative charge) Substance must be able to accept a hydrogen (usually have a negative charge)

13. Reactions Favor if the weak acid has a higher Ka than the conjugate acid in the same equation, the reaction will proceed in the forward direction and favor the products if the weak acid has a higher Ka than the conjugate acid in the same equation, the reaction will proceed in the forward direction and favor the products if the weak acid has a lower Ka than the conjugate acid, the reaction will proceed in the reverse direction and favor the reactants if the weak acid has a lower Ka than the conjugate acid, the reaction will proceed in the reverse direction and favor the reactants

14. Example Write the Bronsted-Lowry equation for the reaction between acetic acid and sodium sulfate. Label the conjugate acid base pairs and comment on whether the products or reactants are favored: Write the Bronsted-Lowry equation for the reaction between acetic acid and sodium sulfate. Label the conjugate acid base pairs and comment on whether the products or reactants are favored:

15. Example 2 Write the Bronsted-Lowry equation for the reaction between lactic acid and potassium hydrogen carbonate. Label the conjugate acid base pairs and comment on whether the products or reactants are favored: Write the Bronsted-Lowry equation for the reaction between lactic acid and potassium hydrogen carbonate. Label the conjugate acid base pairs and comment on whether the products or reactants are favored:

16. C 2 H 5 OCOOH(aq) + HCO 3 1- (aq)   C 2 H 5 OCOO 1- (aq) + H 2 CO 3 (aq) acidbaseconj. Baseconj. Acid K = [H 2 CO 3 (aq)][C 2 H 5 OCOO 1- (aq)] [C 2 H 5 OCOOH(aq)][HCO 3 1- (aq)] Favors products! Kacid = 1.4x10 4 Kconjacid = 4.5x10 -7