Chapter 15 Acid–Base Equilibria Chapter 15 Table of Contents 15.1 15.2 15.3 15.4 15.5 Solutions of Acids or Bases Containing a Common Ion Buffered Solutions Buffering Capacity Titrations and pH Curves Acid–Base Indicators Copyright © Cengage Learning. All rights reserved 2 Section 15.1 Solutions of Acids or Bases Containing a Common Ion Common Ion Effect • Shift in equilibrium position that occurs because of the addition of an ion already involved in the equilibrium reaction. • An application of Le Châtelier’s principle. Return to TOC Copyright © Cengage Learning. All rights reserved 3 Section 15.1 Solutions of Acids or Bases Containing a Common Ion Example HCN(aq) + H2O(l) H3O+(aq) + CN-(aq) • Addition of NaCN will shift the equilibrium to the left because of the addition of CN-, which is already involved in the equilibrium reaction. • A solution of HCN and NaCN is less acidic than a solution of HCN alone. Return to TOC Copyright © Cengage Learning. All rights reserved 4 Section 15.2 Atomic Masses Buffered Solutions Key Points about Buffered Solutions • Buffered Solution – resists a change in pH. • They are weak acids or bases containing a common ion. • After addition of strong acid or base, deal with stoichiometry first, then the equilibrium. Return to TOC Copyright © Cengage Learning. All rights reserved 5 Section 15.2 Atomic Masses Buffered Solutions Adding an Acid to a Buffer Return to TOC Copyright © Cengage Learning. All rights reserved 6 Section 15.2 Atomic Masses Buffered Solutions Buffers Return to TOC Copyright © Cengage Learning. All rights reserved 7 Section 15.2 Atomic Masses Buffered Solutions Solving Problems with Buffered Solutions Return to TOC Copyright © Cengage Learning. All rights reserved 8 Section 15.2 Atomic Masses Buffered Solutions Buffering: How Does It Work? Return to TOC Copyright © Cengage Learning. All rights reserved 9 Section 15.2 Atomic Masses Buffered Solutions Buffering: How Does It Work? Return to TOC Copyright © Cengage Learning. All rights reserved 10 Section 15.2 Atomic Masses Buffered Solutions Henderson–Hasselbalch Equation pH = pK a A + lo g H A • For a particular buffering system (conjugate acid–base pair), all solutions that have the same ratio [A–] / [HA] will have the same pH. Return to TOC Copyright © Cengage Learning. All rights reserved 11 Section 15.2 Atomic Masses Buffered Solutions Exercise What is the pH of a buffer solution that is 0.45 M acetic acid (HC2H3O2) and 0.85 M sodium acetate (NaC2H3O2)? The Ka for acetic acid is 1.8 × 10–5. pH = 5.02 Return to TOC Copyright © Cengage Learning. All rights reserved 12 Section 15.2 Atomic Masses Buffered Solutions Return to TOC Copyright © Cengage Learning. All rights reserved 13 Section 15.2 Atomic Masses Buffered Solutions Buffered Solution Characteristics • Buffers contain relatively large amounts of weak acid and corresponding conjugate base. • Added H+ reacts to completion with the conjugate base. • Added OH reacts to completion with the weak acid. Return to TOC Copyright © Cengage Learning. All rights reserved 14 Section 15.2 Atomic Masses Buffered Solutions Buffered Solution Characteristics • The pH in the buffered solution is determined by the ratio of the concentrations of the weak acid and weak base. As long as this ratio remains virtually constant, the pH will remain virtually constant. This will be the case as long as the concentrations of the buffering materials (HA and A– or B and BH+) are large compared with amounts of H+ or OH– added. Return to TOC Copyright © Cengage Learning. All rights reserved 15 Section 15.3 The Mole Capacity Buffering • The amount of protons or hydroxide ions the buffer can absorb without a significant change in pH. • Determined by the magnitudes of [HA] and [A–]. • A buffer with large capacity contains large concentrations of the buffering components. Return to TOC Copyright © Cengage Learning. All rights reserved 16 Section 15.3 The Mole Capacity Buffering • Optimal buffering occurs when [HA] is equal to [A–]. • It is for this condition that the ratio [A–] / [HA] is most resistant to change when H+ or OH– is added to the buffered solution. Return to TOC Copyright © Cengage Learning. All rights reserved 17 Section 15.3 The Mole Capacity Buffering Choosing a Buffer • pKa of the weak acid to be used in the buffer should be as close as possible to the desired pH. Return to TOC Copyright © Cengage Learning. All rights reserved 18 Section 15.4 Titrations and pH Curves Titration Curve • Plotting the pH of the solution being analyzed as a function of the amount of titrant added. • Equivalence (Stoichiometric) Point – point in the titration when enough titrant has been added to react exactly with the substance in solution being titrated. Return to TOC Copyright © Cengage Learning. All rights reserved 19 Section 15.4 Titrations and pH Curves Neutralization of a Strong Acid with a Strong Base Return to TOC Copyright © Cengage Learning. All rights reserved 20 Section 15.4 Titrations and pH Curves The pH Curve for the Titration of 50.0 mL of 0.200 M HNO3 with 0.100 M NaOH Return to TOC Copyright © Cengage Learning. All rights reserved 21 Section 15.4 Titrations and pH Curves The pH Curve for the Titration of 100.0 mL of 0.50 M NaOH with 1.0 M HCI Return to TOC Copyright © Cengage Learning. All rights reserved 22 Section 15.4 Titrations and pH Curves Weak Acid–Strong Base Titration Step 1: Step 2: A stoichiometry problem (reaction is assumed to run to completion) then determine remaining species. An equilibrium problem (determine position of weak acid equilibrium and calculate pH). Return to TOC Copyright © Cengage Learning. All rights reserved 23 Section 15.4 Titrations and pH Curves Concept Check Consider a solution made by mixing 0.10 mol of HCN (Ka = 6.2 x 10–10) with 0.040 mol NaOH in 1.0 L of aqueous solution. What are the major species immediately upon mixing (that is, before a reaction)? HCN, Na+, OH–, H2O Return to TOC Copyright © Cengage Learning. All rights reserved 24 Section 15.4 Titrations and pH Curves Let’s Think About It… • Why isn’t NaOH a major species? • Why aren’t H+ and CN– major species? • List all possibilities for the dominant reaction. Return to TOC Copyright © Cengage Learning. All rights reserved 25 Section 15.4 Titrations and pH Curves Let’s Think About It… The possibilities for the dominant reaction are: 1. 2. 3. 4. 5. H2O(l) + H2O(l) H3O+(aq) + OH–(aq) HCN(aq) + H2O(l) H3O+(aq) + CN–(aq) HCN(aq) + OH–(aq) CN–(aq) + H2O(l) Na+(aq) + OH–(aq) NaOH Na+(aq) + H2O(l) NaOH + H+(aq) Return to TOC Copyright © Cengage Learning. All rights reserved 26 Section 15.4 Titrations and pH Curves Let’s Think About It… • How do we decide which reaction controls the pH? H2O(l) + H2O(l) H3O+(aq) + OH–(aq) HCN(aq) + H2O(l) H3O+(aq) + CN–(aq) HCN(aq) + OH–(aq) CN–(aq) + H2O(l) Return to TOC Copyright © Cengage Learning. All rights reserved 27 Section 15.4 Titrations and pH Curves Let’s Think About It… HCN(aq) + OH–(aq) CN–(aq) + H2O(l) • What are the major species after this reaction occurs? HCN, CN–, H2O, Na+ Return to TOC Copyright © Cengage Learning. All rights reserved 28 Section 15.4 Titrations and pH Curves Let’s Think About It… • Now you can treat this situation as before. • List the possibilities for the dominant reaction. • Determine which controls the pH. Return to TOC Copyright © Cengage Learning. All rights reserved 29 Section 15.4 Titrations and pH Curves Concept Check Calculate the pH of a solution made by mixing 0.20 mol HC2H3O2 (Ka = 1.8 x 10–5) with 0.030 mol NaOH in 1.0 L of aqueous solution. Return to TOC Copyright © Cengage Learning. All rights reserved 30 Section 15.4 Titrations and pH Curves Let’s Think About It… • What are the major species in solution? Na+, OH–, HC2H3O2, H2O • Why isn’t NaOH a major species? • Why aren’t H+ and C2H3O2– major species? Return to TOC Copyright © Cengage Learning. All rights reserved 31 Section 15.4 Titrations and pH Curves Let’s Think About It… • What are the possibilities for the dominant reaction? 1. 2. 3. 4. 5. H2O(l) + H2O(l) H3O+(aq) + OH–(aq) HC2H3O2(aq) + H2O(l) H3O+(aq) + C2H3O2–(aq) HC2H3O2(aq) + OH–(aq) C2H3O2–(aq) + H2O(l) Na+(aq) + OH–(aq) NaOH Na+(aq) + H2O(l) NaOH + H+(aq) • Which of these reactions really occur? Return to TOC Copyright © Cengage Learning. All rights reserved 32 Section 15.4 Titrations and pH Curves Let’s Think About It… • Which reaction controls the pH? H2O(l) + H2O(l) H3O+(aq) + OH–(aq) HC2H3O2(aq) + H2O(l) H3O+(aq) + C2H3O2–(aq) HC2H3O2(aq) + OH–(aq) C2H3O2–(aq) + H2O(l) • How do you know? Return to TOC Copyright © Cengage Learning. All rights reserved 33 Section 15.4 Titrations and pH Curves Let’s Think About It… HC2H3O2(aq) + OH– Before Change After 0.20 mol 0.030 mol –0.030 mol –0.030 mol 0.17 mol 0 C2H3O2–(aq) + H2O 0 +0.030 mol 0.030 mol K = 1.8 x 109 Return to TOC Copyright © Cengage Learning. All rights reserved 34 Section 15.4 Titrations and pH Curves Steps Toward Solving for pH H3O+ + C2H3O2-(aq) 0.170 M ~0 0.030 M –x +x +x 0.170 – x x 0.030 + x HC2H3O2(aq) + H2O Initial Change Equilibrium Ka = 1.8 x 10–5 pH = 3.99 Copyright © Cengage Learning. All rights reserved Return to TOC 35 Section 15.4 Titrations and pH Curves Exercise Calculate the pH of a 100.0 mL solution of 0.100 M acetic acid (HC2H3O2), which has a Ka value of 1.8 x 10–5. pH = 2.87 Return to TOC Copyright © Cengage Learning. All rights reserved 36 Section 15.4 Titrations and pH Curves Concept Check Calculate the pH of a solution made by mixing 100.0 mL of a 0.100 M solution of acetic acid (HC2H3O2), which has a Ka value of 1.8 x 10–5, and 50.0 mL of a 0.10 M NaOH solution. pH = 4.74 Return to TOC Copyright © Cengage Learning. All rights reserved 37 Section 15.4 Titrations and pH Curves Concept Check Calculate the pH of a solution at the equivalence point when 100.0 mL of a 0.100 M solution of acetic acid (HC2H3O2), which has a Ka value of 1.8 x 10–5, is titrated with a 0.10 M NaOH solution. pH = 8.72 Return to TOC Copyright © Cengage Learning. All rights reserved 38 Section 15.4 Titrations and pH Curves The pH Curve for the Titration of 50.0 mL of 0.100 M HC2H3O2 with 0.100 M NaOH Return to TOC Copyright © Cengage Learning. All rights reserved 39 Section 15.4 Titrations and pH Curves The pH Curves for the Titrations of 50.0-mL Samples of 0.10 M Acids with Various Ka Values with 0.10 M NaOH Return to TOC Copyright © Cengage Learning. All rights reserved 40 Section 15.4 Titrations and pH Curves The pH Curve for the Titration of 100.0mL of 0.050 M NH3 with 0.10 M HCl Return to TOC Copyright © Cengage Learning. All rights reserved 41 Section 15.5 Acid–Base Indicators • Marks the end point of a titration by changing color. • The equivalence point is not necessarily the same as the end point (but they are ideally as close as possible). Return to TOC Copyright © Cengage Learning. All rights reserved 42 Section 15.5 Acid–Base Indicators The Acid and Base Forms of the Indicator Phenolphthalein Return to TOC Copyright © Cengage Learning. All rights reserved 43 Section 15.5 Acid–Base Indicators The Methyl Orange Indicator is Yellow in Basic Solution and Red in Acidic Solution Return to TOC Copyright © Cengage Learning. All rights reserved 44 Section 15.5 Acid–Base Indicators Useful pH Ranges for Several Common Indicators Return to TOC Copyright © Cengage Learning. All rights reserved 45