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. Complete Parts 1-4 before submitting your answer. 1 3 4 NEXT > Two solutions are mixed: 40.0 mL of 0.500 M NH3 and 25.0 mL of 0.300 M HCI. 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. Before (mol) Change (mol) After (mol) -0.0075 Initial (M) Change (M) Equilibrium (M) E 0.313 - x 0 0.0100 0 0.500 + x 40.0 0.115 + x NH3(aq) -0.0100 NH3(aq) + 0.500 2 0.500 - x 0.115-x 0.500 2 0.0125 : on by constructing a BCA table, constructing an ICE table, ant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. -■· 0.300 + < PREV 1 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. 0.300 + x 25.0 H₂O(1) -0.0125 H*(aq) 0.192 0.300 0.300 - x 0.0200 0.300 - x -0.0200 0.313 0.192 + x 4 NH4*(aq) RESET OH(aq) + NH4* (aq) 0.115 0.0075 0.192 - x RESET +x 0.313 + 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...
icon
Related questions
icon
Concept explainers
Question
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. Complete Parts 1-4 before submitting your answer.
1
3
4
NEXT >
Two solutions are mixed: 40.0 mL of 0.500 M NH3 and 25.0 mL of 0.300 M HCI. 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.
Before (mol)
Change (mol)
After (mol)
-0.0075
Initial (M)
Change (M)
Equilibrium (M)
E
0.313 - x
0
0.0100
0
0.500 + x
40.0
0.115 + x
NH3(aq)
-0.0100
NH3(aq) +
0.500
2
0.500 - x
0.115-x
0.500
2
0.0125
:
on by constructing a BCA table, constructing an ICE table,
ant expression, and using this information to determine the
pH. Complete Parts 1-4 before submitting your answer.
-■·
0.300
+
< PREV
1
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.
0.300 + x
25.0
H₂O(1)
-0.0125
H*(aq)
0.192
0.300
0.300 - x
0.0200
0.300 - x
-0.0200
0.313
0.192 + x
4
NH4*(aq)
RESET
OH(aq) + NH4* (aq)
0.115
0.0075
0.192 - x
RESET
+x
0.313 + x
>
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. Complete Parts 1-4 before submitting your answer. 1 3 4 NEXT > Two solutions are mixed: 40.0 mL of 0.500 M NH3 and 25.0 mL of 0.300 M HCI. 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. Before (mol) Change (mol) After (mol) -0.0075 Initial (M) Change (M) Equilibrium (M) E 0.313 - x 0 0.0100 0 0.500 + x 40.0 0.115 + x NH3(aq) -0.0100 NH3(aq) + 0.500 2 0.500 - x 0.115-x 0.500 2 0.0125 : on by constructing a BCA table, constructing an ICE table, ant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. -■· 0.300 + < PREV 1 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. 0.300 + x 25.0 H₂O(1) -0.0125 H*(aq) 0.192 0.300 0.300 - x 0.0200 0.300 - x -0.0200 0.313 0.192 + x 4 NH4*(aq) RESET OH(aq) + NH4* (aq) 0.115 0.0075 0.192 - x RESET +x 0.313 + x >
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. Complete Parts 1-4 before submitting your answer.
< PREV
1
2
NEXT >
The value of Kb for NH3 is 1.8 x 10-5. 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.
[0]
[0.500 + x]
[0.115 + x]
[0.500]
0
[0.500 -x]
0.693
[0.115-x]
Kb
=
3.00 x 10-5
[0.300]
[0.300 + x]
[0.192]
[0.300 -x]
10.41
3
pH =
[0.313]
3.32 x 10-1⁰
=
[0.192 + x]
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. Complete Parts 1-4 before submitting your answer.
1.8 x 10-5
< PREV
1
2
Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3), determine the pH of
solution.
4.52
3
4
[0.115]
[0.192 -x] [0.313 + x]
9.48
RESET
[2x]
0.500
[0.313 -x]
RESET
0.301
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. Complete Parts 1-4 before submitting your answer. < PREV 1 2 NEXT > The value of Kb for NH3 is 1.8 x 10-5. 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. [0] [0.500 + x] [0.115 + x] [0.500] 0 [0.500 -x] 0.693 [0.115-x] Kb = 3.00 x 10-5 [0.300] [0.300 + x] [0.192] [0.300 -x] 10.41 3 pH = [0.313] 3.32 x 10-1⁰ = [0.192 + x] 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. Complete Parts 1-4 before submitting your answer. 1.8 x 10-5 < PREV 1 2 Based on your ICE table (Part 2) and the equilibrium expression for Kb (Part 3), determine the pH of solution. 4.52 3 4 [0.115] [0.192 -x] [0.313 + x] 9.48 RESET [2x] 0.500 [0.313 -x] RESET 0.301
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 6 steps with 6 images

Blurred answer
Knowledge Booster
Ionic Equilibrium
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.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY