1. Acid-Base Equilibria: The Nature of Acids and Bases What makes an Acid an Acid? An acid possess a sour tasteAn acid possess a sour taste An acid dissolves active metals like magnesiumAn acid dissolves active metals like magnesium An acid causes certain vegetable dyes to turnAn acid causes certain vegetable dyes to turn characteristic colors characteristic colors What makes a Base a Base? A bases possess a bitter tasteA bases possess a bitter taste A base feels slippery to the touchA base feels slippery to the touch A base causes certain vegetable dues to turn aA base causes certain vegetable dues to turn a characteristic color

2. Acid-Base Equilibria: The Nature of Acids and Bases The Arrhenius Definition of an Acid and a Base: An acid is a substance that produces H + ions in water solutions A base is a substance that produces OH - ions in a water solution If a solution contains more H + ions than OH - ions we say that the solution is acidic If a solution contains more OH - ions than H + ions we say that the solution is basic

3. Acid-Base Equilibria: The Proton in Water When HCl dissolves in water we write: HCl(g)  H + (aq) + Cl - (aq) H2OH2O H H O : : H+H+H+H+  hydronium ion (H 3 O + )

4. Acid-Base Equilibria: The Proton in Water When HCl dissolves in water we write: HCl(g)  H + (aq) + Cl - (aq) H2OH2O

5. Acid-Base Equilibria: The Proton in Water When HCl dissolves in water we write: HCl(g)  H + (aq) + Cl - (aq) H2OH2OH2OH2O HCl(aq) + H 2 O(aq)  H 3 O + (aq) + Cl - (aq) Acidic solutions are formed by a chemical reaction in which and acid transfers a proton (H + ) to water.

6. Acid-Base Equilibria: The Proton in Water The Bronsted-Lowry Concept of Acids and Bases An acid may be defined as a substance that is capable of donating protons and a base may be defined as substance than accepts protons. Cl H : : : + N H H H : Bronsted acid Bronsted base  Cl : : : : _ + N H H H H +

7. Water is an acid Acid-Base Equilibria: The Proton in Water The Bronsted-Lowry Concept of Acids and Bases NH 3 (aq) + H 2 O(aq)  NH 4 + (aq) + OH - (aq) Describing the relationship between the Arrhenius and Bronsted definitions of acids and bases, The Arrhenius definition says that this solution is basic The Bronsted definition says that H 2 O is a an acid because it donated a proton and NH 3 is a base because it accepted the proton

8. HC 2 H 3 O 2 (aq) + H 2 O(aq)  H 3 O + (aq) + C 2 H 3 O 2 (aq) Acid-Base Equilibria: The Proton in Water The Bronsted-Lowry Concept of Acids and Bases Water is also a base The Bronsted definition says that acetic acid is a an acid because it donates a proton to water and and water is a base because it accepts the proton from the acetic acid

9. NH 3 (aq) + H 2 O(aq)  NH 4 + (aq) + OH - (aq) HC 2 H 3 O 2 (aq) + H 2 O(aq)  H 3 O + (aq) + C 2 H 3 O 2 (aq) Bronsted acid Bronsted base Conjugate acid Conjugate base Bronsted base Bronsted acid Conjugate acid Conjugate base Acid-Base Equilibria: The Proton in Water The Bronsted-Lowry Concept of Acids and Bases The stronger the acid, the weaker its conjugate base; the weaker the acid, the stronger its conjugate base.

10. Acid-Base Equilibria: The Proton in Water The Bronsted-Lowry Concept of Acids and Bases Of course all this Bronsted-Lowry ‘stuff’ raises a number of questions. If water can be an acid and a base, can it act as a proton donor and acceptor to itself? What makes one acid or base strong and another acid or base weak?

11. Acid-Base Equilibria: The Proton in Water The Relative Strengths of Acids and Bases What makes one acid or base strong and another acid or base weak?

12. If water can be an acid and a base, can it act as a proton donor and acceptor to itself? Acid-Base Equilibria: The Proton in Water The Dissociation of Water and the pH Scale Water is capable of auto-ionizing. H H O : : H H O : : +  H H O : H + + H O :.. The reaction occurs to a very small extent; about 1 in 10 8 molecules is ionized at any given moment Protons transfer from one molecule to another at a rate of about 1000 times per second  H + (aq) + OH - H 2 O (l)  H + (aq) + OH - (aq)

13. Acid-Base Equilibria: The Proton in Water If this is true: H 2 O (l)  H + (aq) + OH - (aq) Than this is true: K = [H + ] [OH - ] [H 2 O] And since water is a liquid and its concentration is therefore constant, this expression may be written as: K w = [H + ] [OH - ] where K w is the ion product constant and is equal to 1.0 x 10 -14 Note that [H + ] = [OH - ] = 1.0 x 10 -7 M, water is therefore said to be neutral However, in most solutions these concentrations vary. If If [H + ] > [OH - ], solution is acidic If [H + ] > [OH - ], solution is basic The Dissociation of Water and the pH Scale

14. Acid-Base Equilibria: The Proton in Water The Bronsted-Lowry Concept of Acids and Bases Sample exercise: Indicate whether each of the following solutions is neutral, acidic, or basic: (a) [H + ] = 2 x 10 -5 M, (b) [OH - ] = 0.010 M, ( c) [OH - ] = 1.0 x 10 -7 M Sample exercise: Calculate the concentration of H + (aq) in (a) a solution in which the [OH - ] is 0.020M, (b) a solution in which the [OH - ] = 2.5 x 10 -6 M. Indicate whether the solution is acidic or basic

15. Acid-Base Equilibria: The Proton in Water The Dissociation of Water and the pH Scale

16. Because the concentration of H + ions is often quite small, it can be conveniently expressed in terms of pH = -log [H + ] Acid-Base Equilibria: The Proton in Water The Dissociation of Water and the pH Scale For example, solution with a [H + ] = 2. 5 x 10 5 has a pH of: pH = -log [2. 5 x 10 -5 ] = 4.6 Likewise a solution with a pH of 3.8 has a H + concentration of: Antilog -3.8= 1.58 x 10 4 M

17. Now, you try it! In a sample of lemon juice, [H + ] = 3.8 x 10 -4 M. What is the pH. A commonly available window cleaner has a [H + ] = 5.3 x 10 -9 M Acid-Base Equilibria: The Proton in Water The Dissociation of Water and the pH Scale In a sample of freshly pressed apple juice has a pH of 3.76. Calculate the [H]

18. Because the concentration of OH - ions is often quite small, it can be conveniently expressed in terms of p)H = -log [OH - ] Acid-Base Equilibria: The Proton in Water The Dissociation of Water and the pH Scale Now lets think about this, if the [H] = [OH - ], then the pH = pOH = 7 Sooooo… if K w = [H + ] [OH - ] and K w = 1.0 x 10 -14, then: -log K w = 14 = pH + pOH -log K w = 14 = pH + pOH Sample exercise: What is the pH of a solution with a pOH of 2.5? Is the solution acidic or basic?

19. Acid-Base Equilibria: The Proton in Water Measuring the pH Using Indicators

20. Acid-Base Equilibria: The Differences Between Strong and Weak Acids Initial Equilibrium HX H + X - HX HX H + X -

21. Acid-Base Equilibria: The Differences Between Strong and Weak Acids

22. Dealing with a Strong Acid: What is the pH of 0.010 M solution of HCl? Dealing with a weak acid that is only partially ionizable: Since HX (aq)  H + (aq) + X - (aq), then K a = [H + ][X - ] [HX] The smaller the value of the acid dissociation constant K a, the weaker the acid What is the K a of a 0.10 M solution of formic acid (HCHO 2 ) which has a pH = 2.38? HCHO 2  H + + CHO 2 I C E Acid-Base Equilibria: The Differences Between Strong and Weak Acids

23. What is the concentration of H + ions in a 0.10 M solution of HC 2 H 3 O 2 (K a = 1.8 x 10 -5 ) HC 2 H 3 O 2  H + + C 2 H 3 O 2 I C E What is the pH of the solution? What is the percent ionization of this solution? Acid-Base Equilibria: The Differences Between Strong and Weak Acids

24. What is the pH and percent ionization of a 0.20 M solution of HCN? K a = 4.9 x 10 -10 I C E Acid-Base Equilibria: The Differences Between Strong and Weak Acids

25. Acid-Base Equilibria: Dealing with Polyprotic Acids Substances that are capable of furnishing more than one proton to water are called polyprotic acids. H 2 SO 3 (aq)  H + (aq) + HSO 3 - (aq) K a1 = 1.7 x 10 -2 HSO 3 - (aq)  H + (aq) + SO 3 2- (aq) K a2 = 6.4 x 10 -8 Because K a1 is so much larger than subsequent dissociation constants for most polyprotic acids, almost all the H + (aq) in the solution come from the first ionization reaction.

26. Acid-Base Equilibria: Dealing with Polyprotic Acids

27. What is the pH of 0.0037 M solution of carbonic acid (H 2 CO 3 ) I C E I C E H 2 CO 3  H + + HCO 3 - HCO 3 -  H + + CO 3 2-

28. Acid-Base Equilibria: Strong Bases The most common soluble strong Bases are the hydroxides of group IA and heavier group 2A metals What is the pH of a 0.010 M solution of Ba(OH) 2 ?

29. NH 3 + H 2 O  NH 4 + + OH - I C E Acid-Base Equilibria: Dealing with Weak Bases Weak base + H 2 O  conjugate acid + OH - NH 3 (aq) + H 2 O (l)  NH 4 (aq) + OH - (aq) K b = [NH 4 + ] [OH - ] [NH 3 ] The base dissociation constant K b refers to the equilibrium in which a base reacts with H 2 O to from the conjugate acid and OH - Calculate the [OH - ] in a 0.15 M solution of NH 3.

30. Acid-Base Equilibria: Classes of Weak Acids Amines Anions of Weak Acids

31. Acid-Base Equilibria: Anions of Weak Acids HC 2 H 3 O 2 (aq) + H 2 O(aq)  H 3 O + (aq) + C 2 H 3 O 2 - (aq) Bronsted base Bronsted acid Conjugate acid Conjugate base A second class of weak base is composed of the anions of weak acids Anions of weak acids can be incorporated into salts NaC 2 H 3 O 2  Na + (aq) + C 2 H 3 O 2 - (aq) C 2 H 3 O 2 - + H 2 O  HC 2 H 3 O 2 + OH - K b = 5.6 x 10 10

32. + H 2 O  + OH - I C E Calculate the pH of a 0.01 M solution of sodium hypochlorite (NaClO) Acid-Base Equilibria: Anions of Weak Acids

33. Now it’s you turn: the K b for BrO - is 5.0 x 10 -6. Calculate the pH of a 0.050 M solution of NaBrO

34. Acid-Base Equilibria: Relationship Between K a and K b NH 4 + (aq)  NH 3 (aq) + H + (aq) NH 3 (aq) + H 2 O  NH 4 + (aq) + OH - (aq) Ka =Ka =Ka =Ka = [H + ][NH 3 ] [NH 4 + ] Kb =Kb =Kb =Kb = [NH 4 ][OH - ] [NH 3 ] NH 4 + (aq)  NH 3 (aq) + H + (aq) NH 3 (aq) + H 2 O(l)  NH 4 + (aq) + OH - (aq) H 2 O  H + (aq) + OH - (aq) When two reactions are added to give a third reaction, the equilibrium constant for the third reaction reaction is given by the product of the equilibrium constants for the two added reactions K a x K b = K w pK a + pK b = pK w

35. Acid-Base Equilibria: Relationship Between K a and K b Calculate the (a) base-dissociation constant, K b, for the fluoride ion, is the pK a of HF = 3.17 pK a = -log K a 3.17 = -log K a Antilog -3.17 = 6.76 x 10 -4 Since K a x K b = K w (6.76 x 10 - 4)x K b = 1.0 x 10 -14 K b = 1.0 x 10 -14 / 6.76 x 10 -4 = 1.5 x 10 -11

36. Acid-Base Equilibria: Relationship Between K a and K b Now it’s your turn Calculate the pK b for carbonic acid (K a = 4.3 x 10 -7 )

37. Acid-Base Equilibria: Acid-Base Properties of Salt Solutions Anions of weak acids, HX, are basic and will react with H 2 O to produce OH - X - (aq) + H 2 O (l)  HX(aq) + OH - (aq) Anions of strong acids, such as NO 3 -, exhibit no basicitiy, these ions do not react with water and consequently do not influence the pH Anions of polyprotic acids, such as HCO 3 -, that still have ionizable protons are capable of acting as either proton donors or acceptors depending upon the magnitudes of the K a or K b This last one requires a bit of an explanation

38. Acid-Base Equilibria: Acid-Base Properties of Salt Solutions Anions of polyprotic acids, such as HCO 3 -, that still have ionizable protons are capable of acting as either proton donors or acceptors depending upon the magnitudes of the K a or K b Predict whether the salt Na 2 HPO 4 will form an acidic or basic solution on dissolving in water. Na 2 HPO 4  2Na + (aq) + HPO 4 - HPO 4 - (aq) + H 2 O  H 3 O + + PO 4 3- (aq) HPO 4 - (aq) + H 2 O  H 2 PO 4 2- (aq) + OH - (aq) K 3 = 4.2 x 10 -13 HPO 4 - acting like an acid HPO 4 - acting like an base So HPO - is the conjugate base of H 2 PO 4 -. Since the K 2 of H 2 PO 4 - = 6.2 x 10 -8 then: K b = KaKa = KwKw 1.0 x 10 -14 6.2 x 10 -8 = 1.6 x 10 -7 Since K b is larger than K a, HPO 4 - will act like a base

39. Acid-Base Equilibria: Acid-Base Properties of Salt Solutions Salt derived from a strong base and a strong acid will have a pH of 7 Salt derived from a strong base and a weak acid will have a pH above 7 Salt derived from a weak acid and a weak base depends upon whether the dissolved ion acts as an acid or a base as determined by the size of the K a or K b

40. Acid-Base Equilibria: Acid-Base Character and Chemical Structure A substance HX will transfer a proton only if the H X bond, is already polarized in the following way: HX In ionic compounds such as NaH, the H atom possess a negative charge and behaves like a proton acceptor. Very strong bonds in an HX are less easily ionizable than weak bonds

41. Acid-Base Equilibria: Acid-Base Character and Chemical Structure