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Chapter 14 Acids and Bases. 14.6 The pH Scale. pH Scale. The pH of a solution 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. - PowerPoint PPT Presentation
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Basic Chemistry Copyright © 2011 Pearson Education, Inc.1
Chapter 14 Acids and Bases
14.6
The pH Scale
Basic Chemistry Copyright © 2011 Pearson Education, Inc.2
pH Scale
The pH of a solution
• 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
Basic Chemistry Copyright © 2011 Pearson Education, Inc.3
pH of Everyday Substances
Basic Chemistry Copyright © 2011 Pearson Education, Inc.4
Identify each solution as
A) acidic, B) basic, or N) neutral.
1. ___ HCl with a pH = 1.5
2. ___ pancreatic fluid [H3O+] = 1 x 10−8 M
3. ___ soft drink pH = 3.0
4. ___ pH = 7.0
5. ___ [OH−] = 3 x 10−10 M
6. ___ [H3O+ ] = 5 x 10−12
Learning Check
Basic Chemistry Copyright © 2011 Pearson Education, Inc.5
1. A) HCl with a pH = 1.5
2. B) pancreatic fluid [H3O+] = 1 x 10−8 M
3. A) soft drink pH = 3.0
4. N) pH = 7.0
5. A) [OH-] = 3 x 10−10 M
6. B) [H3O+] = 5 x 10−12 M
Solution
Basic Chemistry Copyright © 2011 Pearson Education, Inc.6
Testing the pH of Solutions
The pH of solutions is determined by using • a pH meter, • pH paper, or • indicators that have specific colors at different
pH values
Basic Chemistry Copyright © 2011 Pearson Education, Inc.7
Mathematically, pH is the negative logarithm (log) of the hydronium ion concentration.
pH = -log [H3O+]
For a solution with [H3O+] = 1 x 10−4
pH = −log [1 x 104 ]
pH = [4.0]
pH = 4.0
Calculating pH
Basic Chemistry Copyright © 2011 Pearson Education, Inc.8
Decimal Places in pH Values
When expressing pH values, the number ofdecimal places is equal to the number ofsignificant figures in the coefficient of [H3O+].
coefficient decimal places
[H3O+] = 1 x 104 pH = 4.0
[H3O+] = 8.0 x 106 pH = 5.10
[H3O+] = 2.4 x 108 pH = 7.62
Basic Chemistry Copyright © 2011 Pearson Education, Inc.9
Guide to Calculating pH
Basic Chemistry Copyright © 2011 Pearson Education, Inc.10
Find the pH of a solution with a [H3O+] of 1.0 x 10−3. STEP 1 Enter the [H3O+] value.
1.0 [EE or EXP] 3 [+/] Display: 1−03 or 103
STEP 2 Press the log key and change the sign.
[log (1 x 10−3)] [+/] = 3
STEP 3 Adjust the number of significant figures on the right of the decimal point to equal the SFs in the coefficient 1.0 x 10−3 3.00
2 SFs 2 SFs on the right of the decimal point
Example of Calculating pH
Basic Chemistry Copyright © 2011 Pearson Education, Inc.11
The [H3O+] of tomato juice is 2.2 x 10−4 M. What is the pH of the solution?1) 3.72) 3.663) 10.34
Learning Check
Basic Chemistry Copyright © 2011 Pearson Education, Inc.12
STEP 1 Enter the [H3O+] value. 2.2 [EE or EXP] 4 [+/] Display: 2.2−04 or 2.204
STEP 2 Press the log key and change the sign. log[2.2−04] [+/] = 3.657577 (Display)
STEP 3 Adjust the number of significant figures on the right of the decimal point to equal the SFs in the coefficient
2.2 x 104 3.66 (2) 2 SFs 2 SFs on the right of the decimal point
Solution
Basic Chemistry Copyright © 2011 Pearson Education, Inc.13
Calculating pH from [OH−]
Calculate the pH of a solution with [OH−] of 4.0 x 10−5.
STEP 1 Enter the [H3O+] value Kw = [H3O+][OH−] = 1.0 x 10−14 = 2.5 x 10 −10
[OH−] [OH−] 4.0 x 10−5
2.5 [EE or EXP] 10 [+/] Display: 2.5−10 or 2.5 10
STEP 2 Press the log key and change the sign.
log[2.5−10] = [9.60205] = 9.60205
Basic Chemistry Copyright © 2011 Pearson Education, Inc.14
Calculating pH from [OH−] (continued)
STEP 3 Adjust the number of significant figures on the right of the decimal point to equal the SFs in the coefficient.
2.5 x 10−10 M pH = 9.60 2 SFs 2SFs on the right of the decimal point
Basic Chemistry Copyright © 2011 Pearson Education, Inc.15
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
[H3O+]
• is equal to the - log [OH−] pOH = - log [OH−]• added to the pH value is equal to 14.00
pH + pOH = 14.00
Basic Chemistry Copyright © 2011 Pearson Education, Inc.
Example of Calculating pOH
Calculate the pOH of a solution that has a pH of 8.35.
pH + pOH = 14.00
pOH = 14.0 – pH = 14.00 - 8.35
= 5.65
16
Basic Chemistry Copyright © 2011 Pearson Education, Inc.17
Calculating [H3O+] from pH
The [H3O+] can be expressed by using the pH as the negative power of 10.
[H3O+] = 10−pH
If the pH is 3.0, the [H3O+] = 1 x 10−3 M.
Basic Chemistry Copyright © 2011 Pearson Education, Inc.
Example of Calculating [H3O+] from pH
Calculate the [H3O+] for a pH value of 8.0.
[H3O+] = 10−pH
STEP 1 Enter the pH value and change the sign.
8.0 [+/] Display = –8.0
STEP 2 Convert pH to [H3O+]. Press the second function key and then the 10x key or press the inverse key and then the log key.
1–08
18
Basic Chemistry Copyright © 2011 Pearson Education, Inc.
Example of Calculating [H3O+] from pH (continued)
STEP 3 Adjust the number of significant figures in the coefficient.
Because the pH value of 8.0 has one digit on the right of the decimal point, the [H3O+] is written with one significant figure.
For pH = 8.0, [H3O+] = 1 x 10−8 M
19
Basic Chemistry Copyright © 2011 Pearson Education, Inc.20
What is the [H3O+] of a solution with a pH of 3.80?
Learning Check
Basic Chemistry Copyright © 2011 Pearson Education, Inc.21
STEP 1 Enter the pH value and change the sign. 3.80 [+/] Display = –3.80
STEP 2 Convert pH to [H3O+]. Press the second function key and then the 10x key or press the inverse key and then the log key.
3.80 (+/-) inv log (or 10x) Display = 1.5848904
STEP 3 Adjust the number of significant figures in the coefficient. Because the pH value of 3.80 has two digits on the right of the decimal point, the [H3O+] is written with two significant figures in the coefficient.
pH 3.80 [H3O+] = 1.6 x 104 M
Solution
Basic Chemistry Copyright © 2011 Pearson Education, Inc.22
pH Range
Basic Chemistry Copyright © 2011 Pearson Education, Inc.23
Learning Check
What is the pH and the pOH of coffee if the [H3O+] is 1 x 10−5 M?
1) pH = 5.0 pOH =7.0
2) pH = 7.0 pOH = 9.0
3) pH = 5.0 pOH = 9.0
Basic Chemistry Copyright © 2011 Pearson Education, Inc.24
Solution
STEP 1 Enter the [H3O+] value.
1 [EE or EXP] 5 [+/] Display: 1−05 or 105
STEP 2 Press the log key and change the sign.
pH = –log [1 x 10−5] = –(–5.0) = 5.0
Basic Chemistry Copyright © 2011 Pearson Education, Inc.25
Solution (continued)
STEP 3 Adjust the number of significant figures on the right of the decimal point to equal the SFs in the coefficient.
Because the [H3O+] has one digit in the coefficient, the pH has one digit to the right of the decimal point.
pH = 5.0pH + pOH = 14.00pOH = 14.00 – pH = 14.00 – 5.0 = 9.0or [OH−] = 1 x 10−9 pOH = –log [1 x 10−9] = –(–9.0) = 9.0 (3)
Basic Chemistry Copyright © 2011 Pearson Education, Inc.26
What is the [H3O+] of a solution with a pOH of 11.15?
1) 1.0 x 10−2.85 M
2) 1.4 x 10−3 M
3) 8.5 x 10−2 M
Learning Check
Basic Chemistry Copyright © 2011 Pearson Education, Inc.27
STEP 1 Enter the pH value and change the sign. pH = 14.00 – pOH = 14.00 - 11.15 = 2.85
2.85[+/] = 2.85STEP 2 Convert pH to [H3O+].
Use second function key and then10x key or inverse key and then log key. 102.85 = 1.41253 x 10−03
STEP 3 Adjust the significant figures in the coefficient. In the pH value 2.85, there are two digits on the right of the decimal point; the [H3O+] has two significant figures.
pH = 2.85 [H3O+] = 1.4 x 10−3 M (2)
Solution