< PREV 1 2 NEXT > Based on your ICE table (Part 2) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ко = = 4.3 x 10-10 RESET [0] [0.500] [0.100] [0.040] [0.700] [0.300] 闭 [2x] [0.500 + x] (0.500 - x] [0.100+x] [0.100-x] [0.040+x] (0.040-x] [0.700+x] [0.700 - x] [0.300 + x] [0.300 - x] < PREV 2 Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3), determine the pH of solution. pH = RESET 0 1.00 × 10° 1.00 × 10* 9.00 5.00 20.7 6.72 0.040 0.200 0.700 Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Kb for CH-NH2 is 4.3 x 10-10. Complete Parts 1-4 before submitting your answer. 3 NEXT > 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C&H NH>CI and 0.500 M C6H5NH2. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) CHÍNH: (84) + OH(aq) H:O(1) CHÍNH (99) RESET 0 0.040 -0.040 0.500 -0.500 0.100 -0.100 0.060 -0.060 0.140 -0.140 0.020 -0.020 < PREV 3 NEXT Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CHÍNH (89) H:O(1) OH(aq) + CHÍNH (99) RESET 0 0.500 0.100 0.040 0.700 0.300 +x 0.500 + x 0.500-x 0.100 + x 0.100-x 0.040 + x 0.040-x 0.700 + x 0.700-x 0.300 + x 0.300-x
< PREV 1 2 NEXT > Based on your ICE table (Part 2) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ко = = 4.3 x 10-10 RESET [0] [0.500] [0.100] [0.040] [0.700] [0.300] 闭 [2x] [0.500 + x] (0.500 - x] [0.100+x] [0.100-x] [0.040+x] (0.040-x] [0.700+x] [0.700 - x] [0.300 + x] [0.300 - x] < PREV 2 Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3), determine the pH of solution. pH = RESET 0 1.00 × 10° 1.00 × 10* 9.00 5.00 20.7 6.72 0.040 0.200 0.700 Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Kb for CH-NH2 is 4.3 x 10-10. Complete Parts 1-4 before submitting your answer. 3 NEXT > 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C&H NH>CI and 0.500 M C6H5NH2. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) CHÍNH: (84) + OH(aq) H:O(1) CHÍNH (99) RESET 0 0.040 -0.040 0.500 -0.500 0.100 -0.100 0.060 -0.060 0.140 -0.140 0.020 -0.020 < PREV 3 NEXT Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CHÍNH (89) H:O(1) OH(aq) + CHÍNH (99) RESET 0 0.500 0.100 0.040 0.700 0.300 +x 0.500 + x 0.500-x 0.100 + x 0.100-x 0.040 + x 0.040-x 0.700 + x 0.700-x 0.300 + x 0.300-x
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
![< PREV
1
2
NEXT >
Based on your ICE table (Part 2) and the definition of Kb, set up the expression for Kb in
order to determine the unknown. Each reaction participant must be represented by one
tile. Do not combine terms.
Ко
=
= 4.3 x 10-10
RESET
[0]
[0.500]
[0.100]
[0.040]
[0.700]
[0.300]
闭
[2x]
[0.500 + x]
(0.500 - x]
[0.100+x]
[0.100-x]
[0.040+x]
(0.040-x]
[0.700+x]
[0.700 - x]
[0.300 + x] [0.300 - x]
< PREV
2
Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3),
determine the pH of solution.
pH =
RESET
0
1.00 × 10°
1.00 × 10*
9.00
5.00
20.7
6.72
0.040
0.200
0.700](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff922ab2d-c754-4c9c-9d3b-bd784fecfd89%2F95a0c682-5f76-4e60-9c64-bec889aa5bd7%2Fhjqbwl_processed.png&w=3840&q=75)
Transcribed Image Text:< PREV
1
2
NEXT >
Based on your ICE table (Part 2) and the definition of Kb, set up the expression for Kb in
order to determine the unknown. Each reaction participant must be represented by one
tile. Do not combine terms.
Ко
=
= 4.3 x 10-10
RESET
[0]
[0.500]
[0.100]
[0.040]
[0.700]
[0.300]
闭
[2x]
[0.500 + x]
(0.500 - x]
[0.100+x]
[0.100-x]
[0.040+x]
(0.040-x]
[0.700+x]
[0.700 - x]
[0.300 + x] [0.300 - x]
< PREV
2
Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3),
determine the pH of solution.
pH =
RESET
0
1.00 × 10°
1.00 × 10*
9.00
5.00
20.7
6.72
0.040
0.200
0.700
Transcribed Image Text:Determine the pH of a solution by constructing a BCA table, constructing
an ICE table, writing the equilibrium constant expression, and using this
information to determine the pH. The value of Kb for CH-NH2 is 4.3 x
10-10. Complete Parts 1-4 before submitting your answer.
3
NEXT >
0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C&H NH>CI
and 0.500 M C6H5NH2. Fill in the table with the appropriate value for each involved
species to determine the moles of reactant and product after the reaction of the acid
and base. You can ignore the amount of water in the reaction.
Before (mol)
Change (mol)
After (mol)
CHÍNH: (84) +
OH(aq)
H:O(1)
CHÍNH (99)
RESET
0
0.040
-0.040
0.500
-0.500
0.100
-0.100
0.060
-0.060
0.140
-0.140
0.020
-0.020
< PREV
3
NEXT
Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to
determine the unknown concentrations of all reactants and products.
Initial (M)
Change (M)
Equilibrium (M)
CHÍNH (89)
H:O(1)
OH(aq)
+
CHÍNH (99)
RESET
0
0.500
0.100
0.040
0.700
0.300
+x
0.500 + x
0.500-x
0.100 + x
0.100-x
0.040 + x
0.040-x
0.700 + x
0.700-x
0.300 + x
0.300-x
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 2 steps
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