Today’s lesson is brought to you by Today’s lesson is brought to you by 7, 14, and the letters7, 14, and the letters

Kw, pHKw, pH

Kw: the ion-product constant of waterKw: the ion-product constant of waterQ: will pure distilled water conduct electricityA: As the demo shows, it will (slightly).• If water conducts electricity, ions must exist• Water exists as an equilibrium, which is

referred to as the self-ionization of water: H2O + H2O H3O+(aq) + OH–(aq)

Simplified reaction: H2O H+(aq) + OH–(aq)

Kc =[H3O+] [OH–]

[H2O]2Kw =or [H3O+] [OH–]

Note: H+ is just shorthand for H3O+

Kc =[H+] [OH–]

[H2O]Kw =or [H+] [OH–]

KwKw• What is the value of Kw?• It has been measured at 1.0 x 10–14 (25 °C)• Notice (pg. 600) that by definition:

when the solution is [H+] > [OH–] acidic [H+] < [OH–] basic [H+] = [OH–] neutral

• Pure water is neutral since [H+] and [OH–] must be identical (both come from one H2O)

• As temperature increases Kw increasesQ: Rewrite the equilibrium of water with heat as a

product or reactant (based on above point)Q: Do PE 1 (refer to example 15.1)

AnswersAnswersAs temperature increases Kw increases.

It must be that: H2O + heat H+ + OH–

(increase temp = shift right = Kw)

PE 1Kw = [H+] [OH–]1.0 x 10–14 = [H+] [7.8 x 10–6] [H+] =1.28 x 10–9

Thus, the solution is basic: [H+] < [OH–]

pHpH• Notice (PE1) that a change in [H+] is matched by

a change in [OH–], since Kw is constant (see middle columns of table 15.2 – pg. 603)

• [H+] is commonly referred to because it is critical to chemical and biochemical reactions

• A quick method of denoting [H+] is via pH• By definition pH = – log [H+]• The pH scale, similar to the Richter scale,

describes a wide range of values• An earthquake of ‘6’ is10x as violent as a ‘5’• Thus, the pH scale condenses possible values

of [H+] to a 14 point scale• Also, it is easier to say pH = 7 vs. [H+] = 1 x 10–7

Calculations with pHCalculations with pH• pH = – log [H+], what is pH if [H+] = 6.3 x 10–5?

Enter 6.3 x 10–5 (‘6.3’, ‘exp’, ‘5’, ‘+/-’)Then hit ‘log’, followed by ‘+/-’ Ans: 4.2

3.98 x 10–8 M

• What is [H+] if pH = 7.4?• To solve this we must rearrange our equation

[H+] = 10–pH mol/LEnter ’10’, ‘xy’, ‘7.4’, ‘+/-’, ‘=‘

• Finally, notice on pg. 603 that pH + pOH = 14• This is related to Kw = 1.0 x 10–14 • You do not need to know how equations are

derived; you need to know how to use them

Equations and practiceEquations and practice

• Read footnote on 601 about significant digits• Do PE 2 – 4 on pg. 605• Use examples 15.2 – 15.4 as reference

pH = – log [H+]

• You will need to memorize the following:

pOH = – log [OH–]

[H+] = 10–pH

[OH–] = 10–pOH

pH + pOH = 14

PE 2 answersPE 2 answersa)pH = – log [H+]

= – log [0.020]= 1.6989 = 1.70

pH + pOH = 14pOH = 14 – pHpOH = 14 – 1.70 =12.3

b)pOH = – log [OH–]= – log [0.0050]= 2.3pH = 14 – pOH= 14 – 2.3 =11.7

c) pH = – log [H+]= – log

[7.2x10-8]= 7.14

pOH = 14 – pHpOH = 14 – 7.14 = 6.86

(slightly basic)d)Ba(OH)2 Ba2+

+ 2OH–

pOH = – log [OH–]= – log

[0.00070]= 3.15

pH = 14 - pOH = 14 – 3.15 = 10.85

PE 3 answersPE 3 answersa) [H+] = 10–pH = 10–2.90 = 1.29 x 10–3 mol/L

pOH = 14 – pH = 14.00 – 2.90 = 11.1[OH–] = 10–pOH = 10–11.1= 7.94 x 10–12 mol/L

b) [H+] = 10–pH = 10–3.85 = 1.41 x 10–4 mol/LpOH = 14 – pH = 14.00 – 3.85 = 10.15[OH–] = 10–pOH = 10–10.15 = 7.08 x 10–12 mol/L

c) [H+] = 10–pH = 10–10.81 = 1.55 x 10–11 mol/LpOH = 14 – pH = 14.00 – 10.81 = 3.19[OH–] = 10–pOH = 10–3.19 = 6.46 x 10–4 mol/L

PE 3, 4 answersPE 3, 4 answersd) [H+] = 10–pH = 10–4.11 = 7.76 x 10–5 mol/L

pOH = 14 – pH = 14.00 – 4.11 = 9.89[OH–] = 10–pOH = 10–9.89= 1.29 x 10–10 mol/L

e) [H+] = 10–pH = 10–11.61 = 2.45 x 10–12 mol/LpOH = 14 – pH = 14.00 – 11.61 = 2.39[OH–] = 10–pOH = 10–2.39 = 4.07 x 10–3 mol/L

PE 4a) acidic, b) acidic, c) basic, d) acidic, e) basic

Measuring pHMeasuring pH• pH can be measured in several ways• Usually it is measured with a coloured acid-

base indicator (see pg. 606) or a pH meter• Coloured indicators are a crude measure of

pH, but are useful in certain applications• pH meters are more accurate, but they must

be calibrated prior to use• Calibration means setting to a standard• A pH meter is calibrated with a solution of

known pH often called a buffer• “Buffer” indicates that the pH is stable

Using pH metersUsing pH meters1. Always rinse pH meter in distilled water prior

to placing it in a solution (buffer or otherwise)2. Place the pH meter in a buffer with about the

same pH as that of your solution (4, 7, or 10)3. Turn on the pH meter only when in solution• Start with with buffer 7. Hit “cal” once.• Wait upto a minute until it automatically sets• Rinse, dry, and place in second buffer (4/10)• Hit “cal” once. Wait until it automatically sets• There is no need to use “read”.4. Measure the pH of your solution

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