A student was titrating a solution of hydrazine, H₂NNH2, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. 1 NEXT 40.0 mL of a 0.200 M H₂NNH₂ solution was titrated with 80 mL of 0.100 M HNO3 (a strong acid). Fill in the ICE 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) 6.00 × 10³ -6.00 × 10³ 0 Initial (M) Change (M) Equilibrium (M) 0.100 + x 0 H₂NNH₂(aq) 0.100 7.00 x 10" 0.100 - x H₂NNH3*(aq) + 2 Question 8 of 23 0.100 0.200 + x 0.200 -7.00 x 10³ 2 + 0.200 A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. < PREV 1 3 4 NEXT > Upon completion of the acid-base reaction, the H₂NNH₂* ion is in equilibrium with water. Set up the ICE table in order to determine the unknown concentrations of reactants and products.. HạO*(aq) + H₂NNH₂(aq) 0.200 - x 3 1.00 × 10 -1.00 x 10 8.00 × 10³ H₂O(l) H*(aq) 0.0333 -8.00 × 10³ 0.0333 + x 4 0.0667 2.00 x 10³ 0.0333 - x H₂NNH3*(aq) +X RESET 0.0667 + x -2.00 x 10³ RESET -x 0.0667 - x
A student was titrating a solution of hydrazine, H₂NNH2, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. 1 NEXT 40.0 mL of a 0.200 M H₂NNH₂ solution was titrated with 80 mL of 0.100 M HNO3 (a strong acid). Fill in the ICE 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) 6.00 × 10³ -6.00 × 10³ 0 Initial (M) Change (M) Equilibrium (M) 0.100 + x 0 H₂NNH₂(aq) 0.100 7.00 x 10" 0.100 - x H₂NNH3*(aq) + 2 Question 8 of 23 0.100 0.200 + x 0.200 -7.00 x 10³ 2 + 0.200 A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. < PREV 1 3 4 NEXT > Upon completion of the acid-base reaction, the H₂NNH₂* ion is in equilibrium with water. Set up the ICE table in order to determine the unknown concentrations of reactants and products.. HạO*(aq) + H₂NNH₂(aq) 0.200 - x 3 1.00 × 10 -1.00 x 10 8.00 × 10³ H₂O(l) H*(aq) 0.0333 -8.00 × 10³ 0.0333 + x 4 0.0667 2.00 x 10³ 0.0333 - x H₂NNH3*(aq) +X RESET 0.0667 + x -2.00 x 10³ RESET -x 0.0667 - 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...
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Transcribed Image Text:A student was titrating a solution of hydrazine, H₂NNH2, with a strong acid solution.
Determine the pH at a particular point in the titration. Do this by constructing a BCA table,
constructing an ICE table, writing the equilibrium constant expression, and use this
information to determine the pH. Complete Parts 1-4 before submitting your answer.
1
NEXT
40.0 mL of a 0.200 M H₂NNH₂ solution was titrated with 80 mL of 0.100 M HNO3 (a strong acid). Fill in the
ICE 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)
6.00 × 10³ -6.00 × 10³
0
Initial (M)
Change (M)
Equilibrium (M)
0.100 + x
0
H₂NNH₂(aq)
0.100
7.00 x 10"
0.100 - x
H₂NNH3*(aq) +
Question 8 of 23
2
0.100
0.200 + x
0.200
-7.00 x 10³
+
0.200
A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution.
Determine the pH at a particular point in the titration. Do this by constructing a BCA table,
constructing an ICE table, writing the equilibrium constant expression, and use this
information to determine the pH. Complete Parts 1-4 before submitting your answer.
0.200 - x
3
1.00 × 10 -1.00 x 10
8.00 × 10³
< PREV
1
2
3
4
NEXT >
Upon completion of the acid-base reaction, the H₂NNH₂* ion is in equilibrium with water. Set up the ICE
table in order to determine the unknown concentrations of reactants and products..
HạO*(aq) + H₂NNH₂(aq)
H₂O(l)
H*(aq)
0.0333
-8.00 × 10³
0.0333 + x
4
0.0667
2.00 × 10³
0.0333 - x
H₂NNH3*(aq)
+X
RESET
0.0667 + x
-2.00 x 10³
RESET
-x
0.0667 - x
![A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution.
Determine the pH at a particular point in the titration. Do this by constructing a BCA table,
constructing an ICE table, writing the equilibrium constant expression, and use this
information to determine the pH. Complete Parts 1-4 before submitting your answer.
< PREV
2
3
4
NEXT
The value of Kb for H₂NNH₂ is 3.0 x 10-6. Based on your ICE table and the equilibrium expression for Ka,
set up the expression for Ka in order to determine the unknown concentrations. Each reaction participant
must be represented by one tile. Do not combine terms.
[0]
[0.100 -x]
3.0 x 10-8
0
[0.100]
1.00
1
[0.200 + x]
3.3 × 10-⁹
9.17
1
Ka
[0.200]
6.74 x 10-1⁰
[0.200 -x]
3.3 x 10-7
[0.0333]
[0.0333 + x]
2.88
2
A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution.
Determine the pH at a particular point in the titration. Do this by constructing a BCA table,
constructing an ICE table, writing the equilibrium constant expression, and use this
information to determine the pH. Complete Parts 1-4 before submitting your answer.
< PREV
Based on your ICE table and the equilibrium expression for Ka, determine the pH of this final solution..
pH
[0.0667]
=
1.48 x 10-5
[0.0333 -x]
||
1.11
[x]
3
[0.0667 + x]
[2x]
[0.0667 -x]
0.100
RESET
[0.100 + x]
3.0 x 10-6
4.83
RESET
2.30](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F84d3fdf0-b73f-4040-a051-97beff994827%2F56a80778-9b31-4fd4-8d97-9a4c2a82ed47%2F2ievb7_processed.png&w=3840&q=75)
Transcribed Image Text:A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution.
Determine the pH at a particular point in the titration. Do this by constructing a BCA table,
constructing an ICE table, writing the equilibrium constant expression, and use this
information to determine the pH. Complete Parts 1-4 before submitting your answer.
< PREV
2
3
4
NEXT
The value of Kb for H₂NNH₂ is 3.0 x 10-6. Based on your ICE table and the equilibrium expression for Ka,
set up the expression for Ka in order to determine the unknown concentrations. Each reaction participant
must be represented by one tile. Do not combine terms.
[0]
[0.100 -x]
3.0 x 10-8
0
[0.100]
1.00
1
[0.200 + x]
3.3 × 10-⁹
9.17
1
Ka
[0.200]
6.74 x 10-1⁰
[0.200 -x]
3.3 x 10-7
[0.0333]
[0.0333 + x]
2.88
2
A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution.
Determine the pH at a particular point in the titration. Do this by constructing a BCA table,
constructing an ICE table, writing the equilibrium constant expression, and use this
information to determine the pH. Complete Parts 1-4 before submitting your answer.
< PREV
Based on your ICE table and the equilibrium expression for Ka, determine the pH of this final solution..
pH
[0.0667]
=
1.48 x 10-5
[0.0333 -x]
||
1.11
[x]
3
[0.0667 + x]
[2x]
[0.0667 -x]
0.100
RESET
[0.100 + x]
3.0 x 10-6
4.83
RESET
2.30
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