1. Acids and Bases Calculating Excess

2. Calculations involving strong acids and bases During an experiment, a student pours 25.0 mL of 1.40 mol/L nitric acid into a beaker that contains 15.0 mL of 2.00 mol/L sodium hydroxide solution. Is the resulting solution acidic or basic? What is the concentration of the ion that causes the solution to be acidic and basic? What is the final pH of the solution?

3. Mixing strong acids and bases Step 1: Write the chemical equation for the reaction. HNO 3 (aq) + NaOH (aq)  NaNO 3 (aq) + H 2 O (l)

4. Mixing strong acids and bases Step 2: Calculate the amount of each reactant using M=n/V 25.0mL of 1.40mol/L nitric acid n=M*V n=1.40mol/L * 0.0250 L = 0.0350 mol 15.0mL of 2.00mol/L sodium hydroxide n=M*V n=2.00mol/L * 0.0150 L = 0.0300 mol

5. Mixing strong acids and bases Step 3: Determine the limiting reagent HNO 3 : NaOH 1:1 The reactants combine in a 1:1 ratio. The amount of NaOH (0.0300mol) is less than that of HNO 3 (0.0350mol) so the NaOH is the limiting reagent.

6. Mixing strong acids and bases Step 4: The reactant in excess is a strong acid or base. Thus, the excess amount results in the same amount of H 3 O + or OH - Amount of excess HNO 3 = 0.0350 mol – 0.0300mol = 0.0050 mol Therefore, the amount of H 3 O + is 5.0 x 10 -3 mol.

7. Mixing strong acids and bases Step 5: Calculate the concentration of the excess ion by using the amount in excess and the total volume of the solution. Calculate the final pH. Total volume of solution = 25.0mL + 15.0mL=40.0mL [H 3 O + ]= (5.0x10 -3 mol) / 0.0400 L = 0.12 mol/L The final pH= - log[H 3 O + ] = 0.92 Acidic solution, [H 3 O + ]= 0.12 mol/L, pH= 0.92

8. Problem #2 During an experiment, a student pours 20.0 mL of 1.25 mol/L sulfuric acid into a beaker that contains 15.0 mL of 2.00 mol/L potassium hydroxide solution. Is the resulting solution acidic or basic? What is the concentration of the ion that causes the solution to be acidic and basic? What is the final pH of the solution?

9. Practice P 586 #1-4

10. Calculations involving Weak Acids and Bases Weak acids and bases only dissociate slightly, we must calculate pH differently. Using the acid dissociation constant, Ka. Using the base dissociation constant, Kb.

11. The Acid Dissociation Constant, Ka Weak acids dissolve in water, according to the following reaction: – HA (aq) + H 2 O (l)  H 3 O + (aq) + A − (aq) Ka is called the acid dissociation constant or acid ionization constant

12. Solving Equilibrium Problems That Involve Acids and Bases Step 1: – Write the chemical equation. – Use the chemical equation to set up an ICE table for the reacting substances whenever initial acid concentrations are involved. – Enter any values that are given in the problem. Represent the concentration of dissociated hydronium ion and conjugate base with a value of x.

13. Solving Equilibrium Problems That Involve Acids and Bases Step 2: – If you have initial concentration and Ka, use the approximation method. – If [HA] / Ka > 500, the change in the initial concentration, x, is negligible and can be ignored. – If [HA] / Ka < 500, the change in the initial concentration, x, is not negligible. Requiring the solution of a quadratic equation.

14. Percent Dissociation The percent dissociation (percent ionization) of a weak acid is the fraction of acid molecules that dissociate compared with the initial concentration of the acid, expressed as a percent.

15. Problem Propanoic acid, CH 3 CH 2 COOH, is a weak monoprotic acid that is used to inhibit mould formation in bread. A student prepared a 0.10 mol/L solution of propanoic acid and found that the pH was 2.96. What is the acid dissociation constant for propanoic acid? What percent of its molecules were dissociated in the solution?

16. Step 1 Write the equation for the dissociation equilibrium of propanoic acid in water. Then set up an ICE table.

17. Step 2 Write the equation for the acid dissociation constant. Substitute equilibrium terms into the equation.

18. Step 3 Calculate [H 3 O + ] using [H 3 O + ] = 10 −pH

19. Step 4 Use the stoichiometry of the equation and [H3O+] to substitute for the unknown term, x, and calculate Ka.

20. Step 5 Calculate the percent dissociation by expressing the fraction of molecules that dissociate out of 100.

21. Problem Formic acid, HCOOH, is present in the sting of certain ants. What is the pH of a 0.025 mol/L solution of formic acid?

24. Practice Problems P 591-592 # 5-10