Practice Exercise 2 H*] Calculate the concentration of OH (aq) in a solution in which (a) [H*] = 2 × 10-° M; (b) [H*] = [OH]; [H*Í = 200 × [OH"]. The pH Scale
Practice Exercise 2 H*] Calculate the concentration of OH (aq) in a solution in which (a) [H*] = 2 × 10-° M; (b) [H*] = [OH]; [H*Í = 200 × [OH"]. The pH Scale
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Question
Number 2
![Safari
File
Edit
View
History
Bookmarks
Window
Help
X X
Sun Aug 8 7:40 PM
Theodore E. Brown, H. Eugene H LeMay, Bruce E. Bursten, Cather...
Page 719 of 1,246 – Shared
Q
Search
[Un ]- [ j
Ch
Theodore E. Brown, H. Eu...
Is
(1.0 × 10¬14)
1.0 X 10-14
(b) In this instance
[H*]
5.6 X 10-6 M
R aIn N
[OH¯]
1.8 × 10-9
N
This solution is acidic because
[H*] > [OH¯]
16.3|The Autoionization of Water
Practice Exercise 1
Practice Exercise 2
Cell m
A solution has [OH¯] = 4.0 × 10-8. What is the value of [H*]
for the solution?
Calculate the concentration of OH¯(ag) in a solution in which
(a) [H*] = 2 x 10–6 M;
(c) [H*] = 200 × [OH¯].
оpert
W
i the mld d
ugl . delg M
(b) [H*] = [OH¯];
I pa
(a) 2.5 × 10¬8 M
(d) 2.5 × 10
(b) 4.0 × 10
(e) 4.0 × 10'
M
(c) 2.5 × 10¬7 M
-6
9-
M
M
678
rON I e
16.4 | The pH Scale
The len Prodsct of Water
The twer
The n
e
JE nur e t
The molar concentration of H(aq) in an aqueous solution is usually very small. For
convenience, we therefore usually express [H*] in terms of pH, which is the negative
logarithm in base 10 of [H*]:*
r d en .c wdte t
T ounag e
rigger Feel
Love Within
S ema nc g t
pH = -log[H*]
[16.17]
Ne
If you need to review the use of logarithms, see Appendix A.
In Sample Exercise 16.4, we saw that [H*]
solution at 25 °C. We can now use Equation 16.17 to calculate the pH of a neutral solution
ari-
Derefe
BAMPLE
CE 4 Cdg h Witr
S e
= 1.0 × 10-7 M for a neutral aqueous
erie I
-XI-sr-
at 25 °C:
Male
Еxp
pH
-log(1.0 X 10-7) = -(-7.00) = 7.00
679
By: Jam
*Because [H*] and [H3O*] are used interchangeably, you might see pH defined as -log [H;O*].
indne
syser
d.e om r
MIRKISTM MM
eNIN N
w ud e l
M ES Crng m O
BOUTON
SECTION 16.4 The pH Scale
681
NHIT E
16.4 The pH Scale
The I f
air n
PDF
Table 16.1 Relationships among [H*], [OH¯], and pH at 25 °C
Light
Solution Type
[H*](M)
[OH-](M)
pH
680
Acidic
>1.0 × 10–7
<1.0 × 10-7
<7.00
Neutral
10 X 10-7
10 X 10-7
7.00
AUG
8.
étv](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffcbd669c-f16c-4186-8647-cce1c8793c67%2F9177c9a9-0221-4749-9240-5a14a6d187b0%2Finvbt5j_processed.png&w=3840&q=75)
Transcribed Image Text:Safari
File
Edit
View
History
Bookmarks
Window
Help
X X
Sun Aug 8 7:40 PM
Theodore E. Brown, H. Eugene H LeMay, Bruce E. Bursten, Cather...
Page 719 of 1,246 – Shared
Q
Search
[Un ]- [ j
Ch
Theodore E. Brown, H. Eu...
Is
(1.0 × 10¬14)
1.0 X 10-14
(b) In this instance
[H*]
5.6 X 10-6 M
R aIn N
[OH¯]
1.8 × 10-9
N
This solution is acidic because
[H*] > [OH¯]
16.3|The Autoionization of Water
Practice Exercise 1
Practice Exercise 2
Cell m
A solution has [OH¯] = 4.0 × 10-8. What is the value of [H*]
for the solution?
Calculate the concentration of OH¯(ag) in a solution in which
(a) [H*] = 2 x 10–6 M;
(c) [H*] = 200 × [OH¯].
оpert
W
i the mld d
ugl . delg M
(b) [H*] = [OH¯];
I pa
(a) 2.5 × 10¬8 M
(d) 2.5 × 10
(b) 4.0 × 10
(e) 4.0 × 10'
M
(c) 2.5 × 10¬7 M
-6
9-
M
M
678
rON I e
16.4 | The pH Scale
The len Prodsct of Water
The twer
The n
e
JE nur e t
The molar concentration of H(aq) in an aqueous solution is usually very small. For
convenience, we therefore usually express [H*] in terms of pH, which is the negative
logarithm in base 10 of [H*]:*
r d en .c wdte t
T ounag e
rigger Feel
Love Within
S ema nc g t
pH = -log[H*]
[16.17]
Ne
If you need to review the use of logarithms, see Appendix A.
In Sample Exercise 16.4, we saw that [H*]
solution at 25 °C. We can now use Equation 16.17 to calculate the pH of a neutral solution
ari-
Derefe
BAMPLE
CE 4 Cdg h Witr
S e
= 1.0 × 10-7 M for a neutral aqueous
erie I
-XI-sr-
at 25 °C:
Male
Еxp
pH
-log(1.0 X 10-7) = -(-7.00) = 7.00
679
By: Jam
*Because [H*] and [H3O*] are used interchangeably, you might see pH defined as -log [H;O*].
indne
syser
d.e om r
MIRKISTM MM
eNIN N
w ud e l
M ES Crng m O
BOUTON
SECTION 16.4 The pH Scale
681
NHIT E
16.4 The pH Scale
The I f
air n
PDF
Table 16.1 Relationships among [H*], [OH¯], and pH at 25 °C
Light
Solution Type
[H*](M)
[OH-](M)
pH
680
Acidic
>1.0 × 10–7
<1.0 × 10-7
<7.00
Neutral
10 X 10-7
10 X 10-7
7.00
AUG
8.
étv
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 3 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY