Ch. 16: Equilibrium in Acid-Base Systems 16.3a: Acid-Base strength and equilibrium law

Definitions Arrhenius Arrhenius A: produce H + in aqueous solution A: produce H + in aqueous solution B: produces OH - in aqueous solution B: produces OH - in aqueous solution very limited very limited Bronsted-Lowry Bronsted-Lowry A: H + donor A: H + donor B: H + acceptor B: H + acceptor more general more general

Acid ionization constant equilibrium expression where H + is removed to form conjugate base equilibrium expression where H + is removed to form conjugate base so for: HA + H 2 O H 3 O + + A - so for: HA + H 2 O H 3 O + + A -

Strength determined by equilibrium position of dissociation reaction determined by equilibrium position of dissociation reaction strong acid: strong acid: lies far to right, almost all HA is dissociated lies far to right, almost all HA is dissociated large K a values large K a values creates weak conjugate base creates weak conjugate base weak acid: weak acid: lies far to left, almost all HA is stays as HA lies far to left, almost all HA is stays as HA small K a values small K a values creates strong conjugate base creates strong conjugate base

Water is a stronger base than the CB of a strong acid but a weaker base than the CB of a weak acid Water is a stronger acid than the CA of a strong base but a weaker acid than the CA of a weak base

[H 2 O], pH and K w conc. of liquid water is omitted from the K a expression conc. of liquid water is omitted from the K a expression we assume that this conc. will remain constant in aqueous sol’n that are not highly concentrated we assume that this conc. will remain constant in aqueous sol’n that are not highly concentrated pH= -log[H + ] pH= -log[H + ] pOH = -log[OH - ] pOH = -log[OH - ] 14.00= pH + pOH 14.00= pH + pOH

Example 1 The [OH - ] of a solution at 25 o C is 1.0x10 -5 M. Determine the [H + ], pH and pOH. The [OH - ] of a solution at 25 o C is 1.0x10 -5 M. Determine the [H + ], pH and pOH. K w = 1.0x = [OH - ] x [H + ] K w = 1.0x = [OH - ] x [H + ] [H + ] = 1.0x10 -9 [H + ] = 1.0x10 -9 pH= -log(1.0x10 -9 ) = 9.00 pH= -log(1.0x10 -9 ) = 9.00 pOH = -log(1.0x10 -5 ) = 5.00 pOH = -log(1.0x10 -5 ) = 5.00 acidic or basic? acidic or basic? basic basic

Approximations If K is very small, we can assume that the change (x) is going to be negligible If K is very small, we can assume that the change (x) is going to be negligible “rule of thumb” is if initial conc. of the acid is >1000 times its K a value then cancel x “rule of thumb” is if initial conc. of the acid is >1000 times its K a value then cancel x this makes the answer true to +/- 5% and why K a values are given to 2 sig. digs this makes the answer true to +/- 5% and why K a values are given to 2 sig. digs 0

Calculating Weak Acids 1. Write major species 2. Decide on which can provide H + ions 3. Make ICE table 4. Put equilibrium values in K a expression 5. Check validity of assumption (x must be less than 5% of initial conc) 6. Find pH

Example 2 Calculate the pH of 1.00 M solution of HF (K a = 7.2 x ) Calculate the pH of 1.00 M solution of HF (K a = 7.2 x ) HF, H 2 O HF, H 2 O HF  H + + F - K a = 7.2x10 -4 HF  H + + F - K a = 7.2x10 -4 H 2 O  H + + OH - K w = 1.0 x H 2 O  H + + OH - K w = 1.0 x HF will provide much more H + than H 2 O – ignore H 2 O HF will provide much more H + than H 2 O – ignore H 2 O

Example 2 HF  H + + F - HF  H + + F - I 1.00 M 00 C-x+x+x E x xx

Example 2 Check assumption: Check assumption:  pH = -log(0.027) = 1.57

Example 3 Find pH of M solution of HOCl (K a = 3.5x10 -8 ) Find pH of M solution of HOCl (K a = 3.5x10 -8 ) HOCl, H 2 O HOCl, H 2 O HOCl will provide much more H + than H 2 O, so we ignore H 2 O HOCl will provide much more H + than H 2 O, so we ignore H 2 O HOCl  H + + OCl - HOCl  H + + OCl - I M 00 C-x+x+x E x xx

Example 3  Check assumption:  pH = -log(5.9x10 -5 ) = 4.23

Example 4 Find K a for propanoic acid given the following information Find K a for propanoic acid given the following information [C 2 H 5 COOH] = 0.10M and pH = 2.96 [C 2 H 5 COOH] = 0.10M and pH = 2.96 [H 3 O + ] = 1.1 x M [H 3 O + ] = 1.1 x M C 2 H 5 COOH + H 2 O  C 2 H 5 COO - + H 3 O + C 2 H 5 COOH + H 2 O  C 2 H 5 COO - + H 3 O + I 0.10 M 00 C-x -1.1 x M +x +1.1 x M +x E 0.10 – x(1.1 x M) 1.1 x M 1) C 2 H 5 COOH + H 2 O  C 2 H 5 COO - + H 3 O + Sol’n 2) Calculate [H 3 O + ] using pH 1.1 x M [H 3 O + ] = 10 -pH [H 3 O + ] = [H 3 O + ] = 1.1 x M Pure water is not included as it does not change 3)

Example 4 con’t  % ionization: 4) Solve for K a < 5% indicates a weak acid

Homework Textbook p743 #2a,c,e 5,7,9 LSM 16.3A and 16.3D