1. 1 Chapter 14 Acids and Bases 14.6 The pH Scale Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

2. 2 pH Scale The pH scale: Is used to indicate the acidity of a solution. Has values that usually range from 0 to 14. Is acidic when the values are less than 7. Is neutral with a pH of 7. Is basic when the values are greater than 7.

3. 3 pH of Everyday Substances Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

4. 4 Identify each solution as 1. acidic 2. basic3. neutral A. ___ HCl with a pH = 1.5 B. ___ Pancreatic fluid [H 3 O + ] = 1 x 10 −8 M C. ___ Sprite soft drink pH = 3.0 D. ___ pH = 7.0 E. ___ [OH − ] = 3 x 10 −10 M F. ___ [H 3 O + ] = 5 x 10 −12 Learning Check

5. 5 A. 1 HCl with a pH = 1.5 B. 2 Pancreatic fluid [H 3 O + ] = 1 x 10 −8 M C. 1 Sprite soft drink pH = 3.0 D. 3 pH = 7.0 E. 1 [OH - ] = 3 x 10 −10 M F. 2 [H 3 O + ] = 5 x 10 −12 Solution

6. 6 Testing the pH of Solutions The pH of solutions can be determined using pH meter, pH paper, or indicators that have specific colors at different pH values. Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

7. 7 pH Range Table 14.8 Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

8. 8 pH is the negative log of the hydronium ion concentration. pH = - log [H 3 O + ] For a solution with [H 3 O + ] = 1 x 10 −4 pH =−log [1 x 10 −4 ] pH = - [-4.0] pH = 4.0 Calculating pH

9. 9 Significant Figures in pH When expressing log values, the number of decimal places in the pH is equal to the number of significant figures in the coefficient of [H 3 O + ]. [H 3 O + ] = 1 x 10 -4 pH = 4.0 [H 3 O + ] = 8.0 x 10 -6 pH = 5.10 [H 3 O + ] = 2.4 x 10 -8 pH = 7.62

10. 10 Guide to pH Calculations Copyright © 2008 by Pearson Education, Inc. Publishing as Benjamin Cummings

11. 11 Find the pH of a solution with a [H 3 O + ] of 1.0 x 10 −3 : STEP 1 Enter [H 3 O + ] Enter 1 x 10 -3 by pressing 1 (EE) 3 The EE key gives an exponent of 10 and change sign (+/- key or – key) STEP 2 Press log key and change sign - log (1 x 10 −3 ) = -[-3] STEP 3 Adjust significant figures after decimal point 3 3.00 Two significant figures in 1.0 x 10 −3 Calculating pH

12. 12 A. The [H 3 O + ] of tomato juice is 2 x 10 −4 M. What is the pH of the solution? 1) 4.02) 3.73) 10.3 B. The [OH − ] of a solution is 1.0 x 10 −3 M. What is the pH of the solution? 1) 3.002) 11.003) -11.00 Learning Check

13. 13 A. 2) 3.7 pH = - log [ 2 x 10 -4 ] = 3.7 2 (EE) 4 (+/-) log (+/-) B. 2) 11.00 Use the K w to obtain [H 3 O + ] = 1.0 x 10 −11 pH = - log [1.0 x 10 −11 ] 1.0 (EE) 11 (+/-) log (+/-) Solution

14. 14 pOH The pOH of a solution Is analogous to the pH value on the pH scale. Is based on the [OH − ]. Has high pOH values with low [OH − ] and high [H 3 O + ]. Is equal to the - log [OH - ] pOH = - log [OH - ]. Added to the pH value is equal to 14.0. pH + pOH = 14.0

15. 15 Calculation pOH Find the pOH of a solution with a [OH − ] of 2.0 x 10 −3. STEP 1 Enter [OH − ] STEP 2 Press log key and change sign - log (2.0 x 10 −3 ) = -[-2.69897] = 2.69897 STEP 3 Adjust figures after decimal point 2.70 Two significant figures in 2.0 x 10 −3

16. 16 Calculating [H 3 O + ] from pH The [H 3 O + ] can be expressed by using the pH as the negative power of 10. [H 3 O + ] = 1 x 10 −pH If the pH is 3.0, the [H 3 O + ] = 1 x 10 −3 On a calculator 1. Enter the pH value 3.0 2. Change sign -3.0 3. Use the inverse log key (or 10 x ) to obtain the [H 3 0 + ]. =1 x 10 −3 M

17. 17 A. What is the [H 3 O + ] of a solution with a pH of 10.0? 1) 1 x 10 −4 M2) 1 x 10 10 M 3) 1 x 10 −10 M B. What is the [H 3 O + ] of a solution with a pH of 5.75? 1) 1.8 x 10 − 6 M2) 1.778 x 10 −6 M 3) 2 x 10 −6 M Learning Check

18. 18 A. What is the [H 3 O + ] of a solution with a pH of 10.0? 3) 1 x 10 -10 M1 x 10 -pH B. What is the [H 3 O + ] of a solution with a pH of 5.75? 1) 1.8 x 10 − 6 M 5.75 (+/-) inv log (or 10 x ) = 1.8 x 10 -6 Note: Two decimal places (.75), indicate two significant figures in the coefficient of the answer. Solution

19. 19 Learning Check What is the pH and the pOH of coffee if the [H 3 O + ] is 1 x 10 −5 M? 1) pH = 5.0 pOH =7.0 2) pH = 7.0 pOH = 9.0 3) pH = 5.0pOH = 9.0

20. 20 Solution What is the pH and the pOH of coffee if the [H 3 O + ] is 1 x 10 −5 M? 3) pH = 5.0pOH = 9.0 pH = -log [1 x 10 −5 ] = -(-5.0) = 5.0 pH + pOH = 14.0 pOH = 14.0 – pH = 14.0 – 5.0 = 9.0 or [OH - ] = 1 x 10 −9 pOH = - log [1 x 10 −9 ] = -(-9.0) = 9.0