1. Chapter 19: Acids and Bases Sections 19.1 to 19.4

3. Acid Properties Sour taste (citrus fruits) Sour taste (citrus fruits) Conduct electric current Conduct electric current Change the color of indicators Change the color of indicators React with bases to produce salt and water: React with bases to produce salt and water: HCl + NaOH  H 2 O + NaCl Some react with metals to release H 2 gas: Some react with metals to release H 2 gas: Mg + HCl  MgCl 2 + H 2

4. Naming Acids Review Binary Acids: Binary Acids: –Hydroiodic Acid HI HI –HF Hydrofluoric Acid Hydrofluoric Acid Ternary Acids (oxyacids) HClO 3 Chloric Acid HClO 2 Chlorous Acid

5. CATEGORIES OF ACIDS Monoprotic Monoprotic –ONE ionizable H + Example: HNO 3 Diprotic Diprotic –TWO ionizable H + Example: H 2 SO 4 Triprotic Triprotic –THREE ionizable H + Example: H 3 PO 4

6. Base Properties Bitter taste (coffee) Bitter taste (coffee) Feel slippery (soap) Feel slippery (soap) Change the color of indicators Change the color of indicators Caustic- attack the skin, cause severe burns Caustic- attack the skin, cause severe burns Conduct electric current Conduct electric current

7. Arrhenius Acids and Bases Arrhenius Acid: Arrhenius Acid: A compound that produces H + in solution. A compound that produces H + in solution. Ex: HCl (g) --------  H + (aq) + Cl - (aq) Ex: HCl (g) --------  H + (aq) + Cl - (aq) Arrhenius Base: Arrhenius Base: A compound that produces OH - in solution. A compound that produces OH - in solution. Ex: NaOH (s) ---------  Na+ (aq) + OH- (aq) Ex: NaOH (s) ---------  Na+ (aq) + OH- (aq) H2OH2O H2OH2O

8. Acid/Base Strength Strong Acid: Ionizes completely in aq. soln. Strong Acid: Ionizes completely in aq. soln. HClH 2 SO 4 HBrHNO 3 HIHClO 4 HClO 3 Strong Bases: Group 1 and 2 hydroxides

9. Acid-Base Theories Bronsted-Lowry: expands Arrhenius definition of acids and bases. Bronsted-Lowry: expands Arrhenius definition of acids and bases. –Bronsted-Lowry Acid: proton donor –Bronsted-Lowry Base: proton acceptor ex: HCl + NH 3  NH 4 + + Cl - ex: HCl + NH 3  NH 4 + + Cl - Monoprotic B-L Acid B-L Base ex2: H 3 PO 4 + H 2 O  H 3 O + + H 2 PO 4 - Which is the B-L Acid? B-L Base?

10. Lewis Acids and Bases Based on bonding and structure and include substances that may not include Hydrogen. Based on bonding and structure and include substances that may not include Hydrogen. –Lewis Acid: electron pair acceptor –Lewis Base: electron pair donor ex: BF 3 (aq) + F - (aq)  BF 4 - (aq) ex: BF 3 (aq) + F - (aq)  BF 4 - (aq) Draw the dot structure for these substances and classify as a Lewis Acid or Base. Lewis Acid Lewis Base

11. Conjugate Acids and Bases (Based on Bronsted-Lowry Classification) Conjugate Base: The substance that remains after an B-L acid has given up a proton (H + ). Conjugate Base: The substance that remains after an B-L acid has given up a proton (H + ). Conjugate Acid: The substance formed when a B-L base has gained a proton. Conjugate Acid: The substance formed when a B-L base has gained a proton. ex: HCl (aq) + H 2 O (l)  Cl - (aq) + H 3 O + (aq) AcidBase Conjugate Base Conjugate Acid Table 19.6: The stronger the acid, the weaker its conjugate base. Equilibrium favors weak acid/base formation.

12. Acid Reactions Neutralization: Neutralization: HCl (aq) + NaOH(aq)  NaCl (aq) + H 2 O (l) HCl (aq) + NaOH(aq)  NaCl (aq) + H 2 O (l) Acid Formation from Acid Anhydrides: Acid Formation from Acid Anhydrides: SO 3 (g) + H 2 O (l)  H 2 SO 4 (aq) SO 3 (g) + H 2 O (l)  H 2 SO 4 (aq) Base Formation from Basic Anhydrides: Base Formation from Basic Anhydrides: Na 2 O + H 2 O(l)  2NaOH Na 2 O + H 2 O(l)  2NaOH Acid Anhydride Acid Rain Basic Anhydride

13. Aqueous Solutions and pH Self Ionization of Water Self Ionization of Water –Water also supplies H 3 O + and OH - ions. H 2 O (l) + H 2 O (l) H 3 O + (aq) + OH - (aq) H 2 O (l) + H 2 O (l) H 3 O + (aq) + OH - (aq) 1.0 x 10 -7 M Conductivity Experiments show the concentrations of ions at 25 °C: 1.0 x 10 -7 M Ionization Constant of Water, K w Ionization Constant of Water, K w K w = [H 3 O + ][OH - ] = [[ K w = [H 3 O + ][OH - ] = [1.0 x 10 -7 M][1.0 x 10 -7 M] K w = 1.0 x 10 -14 M 2 Constant at a given temperature

14. Neutral, Acidic, and Basic Solutions Neutral: Neutral: [HO + ] = [OH - ] [H 3 O + ] = [OH - ] Acids: Acids: [HO + ] > [OH - ] [H 3 O + ] > [OH - ] Bases: Bases: [HO + ] < [OH - ] [H 3 O + ] < [OH - ] Determine the hydronium and hydroxide ion concentrations in a 1 x 10 -5 M HCl solution.

15. pH Scale A more convenient way to express acidity A more convenient way to express acidity pH = -log[H 3 O + ] pH = -log[H 3 O + ] pOH = -log[OH-] pOH = -log[OH-] pH + pOH = 14.0 pH + pOH = 14.0 Find the pH and pOH of a 1x10 -10 M solution of HBr. Find the pH and pOH of a 1x10 -10 M solution of HBr.

16. 1. HBr is an acid so we are looking at the [H + ] concentration. [H + ] = 1x10 -10 M [H + ] = 1x10 -10 M 2. pH = -log[1x10 -10 ] pH = 10 3. pH + pOH = 14 10 + pOH = 14 10 + pOH = 14 pOH = 4 pOH = 4

17. Calculating pH pH = -log [H + ] Ex: A solution has a H + concentration of 1x10 -5 pH = -log [1x10 -5 ] pH = 5 and we have an acidic solution Ex: A solution has a pH=8 8 = -log [H + ] [H + ] = 1 x 10 -8

19. Indicators and Titration Acid-Base Indicators: Compounds whose colors are sensitive to pH. Acid-Base Indicators: Compounds whose colors are sensitive to pH. Titration: Method used to determine an unknown concentration of solution. Titration: Method used to determine an unknown concentration of solution.

20. Equivalence Point The point at which the 2 solutions used in a titration are present in equal amounts. The point at which the 2 solutions used in a titration are present in equal amounts. End Point: The point in a titration during which an indicator changes color. End Point: The point in a titration during which an indicator changes color.

21. NEUTRALIZATION OF ACIDS & BASES If we need to neutralize an acid or a base, we use the following formula: M a V a C b = M b V b C a M x =Molarity (mol/L) of the acid or base M x =Molarity (mol/L) of the acid or base V x =Volume (L) of the acid or base V x =Volume (L) of the acid or base C x =Coefficient (balanced eq.) of the acid or base C x =Coefficient (balanced eq.) of the acid or base

22. M a V a C b = M b V b C a Example: A 25mL solution of H 2 SO 4 is neutralized by 18mL of a 1.0M NaOH using phenolphthalein as an indicator. What is the concentration (M) of the H 2 SO 4 ? What is the concentration (M) of the H 2 SO 4 ? Step 1: Write the neutralization rxn and balance H 2 SO 4 + 2NaOH Na 2 SO 4 + 2H 2 O Step 2: Solve for the unknown. M a = M b V b C a (1.0M)(0.018L)(1) V a C b (0.025L)(2) V a C b (0.025L)(2) M a = 0.36M M a = 0.36M