Part 2 Procedure, Data & Analysis: Recall: The amount of ionization or dissociation of ions determines the strength of an acid or base. The concentration of [H3O*], hydronium ion and [OH]. hydroxide ion, can be used to calculate pH and pOH as shown on the diagram here: Note: we use [H₂O*] and [H] interchangeably. 1. Click on Water Solution, Graph View, Probe Tool. Insert the probe in the water. Notice that given before 2. Fill in the hydronium the the pH. 3. Use the the pOH. Equilibrium Concentration (mol/L) 10² 10¹ 10⁰ 101 10° 10⁰ 101 100 10⁰ 107 104 PH: 7.00 2 H₂O H3O+ + OH 1L [H,₂0*] or [H] H')-10 LHIS-Hd pH (OH)-1x10¹4 [H] TOHT POH-14-pH pH-14-POH [OH] Show work: HoỘI -LHO pOH the initial concentration of the solution is any ionization or dissociation takes place. POH= -log[OH'] missing concentration values for the and hydroxide ions on the chart here: Use concentration value for [H3O+] to calculate Show work: concentration value for [OH] to calculate Show work: 4. Did your answer to # 2 match the pH given in the simulation? 5. Is the answer to #3 equal to: (14 - pH)? 6. Is the solution an acid, a base or neutral, based upon the calculated pH?_ Attach notebook paper to show calculations for the pH and pOH for the other solutions.
Part 2 Procedure, Data & Analysis: Recall: The amount of ionization or dissociation of ions determines the strength of an acid or base. The concentration of [H3O*], hydronium ion and [OH]. hydroxide ion, can be used to calculate pH and pOH as shown on the diagram here: Note: we use [H₂O*] and [H] interchangeably. 1. Click on Water Solution, Graph View, Probe Tool. Insert the probe in the water. Notice that given before 2. Fill in the hydronium the the pH. 3. Use the the pOH. Equilibrium Concentration (mol/L) 10² 10¹ 10⁰ 101 10° 10⁰ 101 100 10⁰ 107 104 PH: 7.00 2 H₂O H3O+ + OH 1L [H,₂0*] or [H] H')-10 LHIS-Hd pH (OH)-1x10¹4 [H] TOHT POH-14-pH pH-14-POH [OH] Show work: HoỘI -LHO pOH the initial concentration of the solution is any ionization or dissociation takes place. POH= -log[OH'] missing concentration values for the and hydroxide ions on the chart here: Use concentration value for [H3O+] to calculate Show work: concentration value for [OH] to calculate Show work: 4. Did your answer to # 2 match the pH given in the simulation? 5. Is the answer to #3 equal to: (14 - pH)? 6. Is the solution an acid, a base or neutral, based upon the calculated pH?_ Attach notebook paper to show calculations for the pH and pOH for the other solutions.
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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Question
![I
Part 2 Procedure, Data & Analysis:
Recall: The amount of ionization or dissociation of ions
determines the strength of an acid or base. The
concentration of [H3O+], hydronium ion and [OH].
hydroxide ion, can be used to calculate pH and pOH as
shown on the diagram here:
Note: we use [H3O+] and [H*] interchangeably.
1. Click on Water Solution, Graph View, Probe Tool.
Insert the
probe in the
water.
Notice that
given before
2. Fill in the
hydronium
the
the pH.
3. Use the
the pOH.
Equilibrium Concentration (mol/L)
10²
10¹
10⁰
10¹
10
10ª
104
10%
10⁰
107
10⁰
pH: 7.00
2 H₂O H3O+ + OH-
H
1L
4
[H₂O*]
or [H*]
pH
(OH)-1x10¹4
H
(H)-1x10-¹4
-LOUISE
POH-14-PH
pH-14-POH
Show work:
[OH]
LIO - امي
the initial concentration of the solution is
any ionization or dissociation takes place.
4. Did your answer to # 2 match the pH given in the simulation?
5. Is the answer to #3 equal to: (14 - pH)?
6. Is the solution an acid, a base or neutral, based upon the calculated pH?
Attach notebook paper to show calculations for the pH and pOH for the other solutions.
Page 2 /
+
LHOS-HO
POH
missing concentration values for the
and hydroxide ions on the chart here: Use
concentration value for [H3O+] to calculate
Show work:
O
concentration value for [OH] to calculate
Show work:](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F10088e78-d43b-4c26-8ee3-a5c015264f28%2Fc1879d47-09e9-40f8-bc66-dfed7b64330b%2Ftvb6fcl_processed.jpeg&w=3840&q=75)
Transcribed Image Text:I
Part 2 Procedure, Data & Analysis:
Recall: The amount of ionization or dissociation of ions
determines the strength of an acid or base. The
concentration of [H3O+], hydronium ion and [OH].
hydroxide ion, can be used to calculate pH and pOH as
shown on the diagram here:
Note: we use [H3O+] and [H*] interchangeably.
1. Click on Water Solution, Graph View, Probe Tool.
Insert the
probe in the
water.
Notice that
given before
2. Fill in the
hydronium
the
the pH.
3. Use the
the pOH.
Equilibrium Concentration (mol/L)
10²
10¹
10⁰
10¹
10
10ª
104
10%
10⁰
107
10⁰
pH: 7.00
2 H₂O H3O+ + OH-
H
1L
4
[H₂O*]
or [H*]
pH
(OH)-1x10¹4
H
(H)-1x10-¹4
-LOUISE
POH-14-PH
pH-14-POH
Show work:
[OH]
LIO - امي
the initial concentration of the solution is
any ionization or dissociation takes place.
4. Did your answer to # 2 match the pH given in the simulation?
5. Is the answer to #3 equal to: (14 - pH)?
6. Is the solution an acid, a base or neutral, based upon the calculated pH?
Attach notebook paper to show calculations for the pH and pOH for the other solutions.
Page 2 /
+
LHOS-HO
POH
missing concentration values for the
and hydroxide ions on the chart here: Use
concentration value for [H3O+] to calculate
Show work:
O
concentration value for [OH] to calculate
Show work:
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