E' I C E 1. Phenylamine is an aromatic amine that is used in the manufacture of dyes. When absorbed through the skin it causes the Fe*2 in hemoglobin to become oxidized into Fe+³, resulting in the formation of methemoglobin which cannot bind to or transport oxygen. Phenylamine is soluble in water and acts as a weak base. a. a. C6H5NH₂ (aq) + H₂O () C6H5NH3+ (aq) + OH (aq) When you measure the concentrations of the ionized substances you find them to be: [C6H5NH₂] = 0.234 mol/L [C6H5NH3*] = 2.8 x 10³ mol/L [OH-]= 2.8 x 10³ mol/L If the K, is 4.27 x 10-10, is the reaction at equilibrium? If not, which direction does it need to move (right or left) to reach equilibrium? Explain. At equilibrium the concentrations of the ionized substances are: [C6H5NH₂] = 0.0537 mol/L [C6H5NH3*] =4.79 x 10€ mol/L [OH-]= 4.79 x 10 mol/L If this reaction is taking place in a 2.0L container, and 1.5 moles of phenylamine were added to the reaction, what will the new concentrations of the three ionic species be when equilibrium is re-established? CoHsNHz (aq) + H₂O (l) 2. Determine the K, for the above solution 3. Determine the pH for the above solution S CH5NH3* (aq) + OH(aq)
E' I C E 1. Phenylamine is an aromatic amine that is used in the manufacture of dyes. When absorbed through the skin it causes the Fe*2 in hemoglobin to become oxidized into Fe+³, resulting in the formation of methemoglobin which cannot bind to or transport oxygen. Phenylamine is soluble in water and acts as a weak base. a. a. C6H5NH₂ (aq) + H₂O () C6H5NH3+ (aq) + OH (aq) When you measure the concentrations of the ionized substances you find them to be: [C6H5NH₂] = 0.234 mol/L [C6H5NH3*] = 2.8 x 10³ mol/L [OH-]= 2.8 x 10³ mol/L If the K, is 4.27 x 10-10, is the reaction at equilibrium? If not, which direction does it need to move (right or left) to reach equilibrium? Explain. At equilibrium the concentrations of the ionized substances are: [C6H5NH₂] = 0.0537 mol/L [C6H5NH3*] =4.79 x 10€ mol/L [OH-]= 4.79 x 10 mol/L If this reaction is taking place in a 2.0L container, and 1.5 moles of phenylamine were added to the reaction, what will the new concentrations of the three ionic species be when equilibrium is re-established? CoHsNHz (aq) + H₂O (l) 2. Determine the K, for the above solution 3. Determine the pH for the above solution S CH5NH3* (aq) + OH(aq)
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter15: Acid–base Equilibria
Section: Chapter Questions
Problem 7P
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Question
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1. Phenylamine is an aromatic amine that is used in the manufacture of dyes. When absorbed through
the skin it causes the Fe+2 in hemoglobin to become oxidized into Fe+3, resulting in the formation of
methemoglobin which cannot bind to or transport oxygen. Phenylamine is soluble in water and acts as
a weak base.
a.
a.
CøHşNHz (aq) + H2O (l) = CHşNH;* (aq) + OH (aq)
When you measure the concentrations of the ionized substances you find them to be:
[C6H5NH₂] = 0.234 mol/L [C6H5NH3*] = 2.8 x 10³ mol/L [OH-]= 2.8 x 10³ mol/L
If the K is 4.27 x 10-10, is the reaction at equilibrium? If not, which direction does it need to
move (right or left) to reach equilibrium? Explain.
At equilibrium the concentrations of the ionized substances are:
[C6H5NH₂] = 0.0537 mol/L [C6H5NH3*] =4.79 x 10€ mol/L
[OH-]= 4.79 x 10¹ mol/L
If this reaction is taking place in a 2.0L container, and 1.5 moles of phenylamine were added to
the reaction, what will the new concentrations of the three ionic species be when equilibrium is
re-established?
CoHsNHz (aq)
+ H₂O(l)
2. Determine the K, for the above solution
3. Determine the pH for the above solution
S
C6H5NH3* (aq) +
OH (aq)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F34af2e55-eb3e-48d0-914c-e1a2f86a241e%2Fbede72d0-34b6-4db1-92e3-a60ff3134a47%2F7lmzp8d_processed.png&w=3840&q=75)
Transcribed Image Text:E'
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1. Phenylamine is an aromatic amine that is used in the manufacture of dyes. When absorbed through
the skin it causes the Fe+2 in hemoglobin to become oxidized into Fe+3, resulting in the formation of
methemoglobin which cannot bind to or transport oxygen. Phenylamine is soluble in water and acts as
a weak base.
a.
a.
CøHşNHz (aq) + H2O (l) = CHşNH;* (aq) + OH (aq)
When you measure the concentrations of the ionized substances you find them to be:
[C6H5NH₂] = 0.234 mol/L [C6H5NH3*] = 2.8 x 10³ mol/L [OH-]= 2.8 x 10³ mol/L
If the K is 4.27 x 10-10, is the reaction at equilibrium? If not, which direction does it need to
move (right or left) to reach equilibrium? Explain.
At equilibrium the concentrations of the ionized substances are:
[C6H5NH₂] = 0.0537 mol/L [C6H5NH3*] =4.79 x 10€ mol/L
[OH-]= 4.79 x 10¹ mol/L
If this reaction is taking place in a 2.0L container, and 1.5 moles of phenylamine were added to
the reaction, what will the new concentrations of the three ionic species be when equilibrium is
re-established?
CoHsNHz (aq)
+ H₂O(l)
2. Determine the K, for the above solution
3. Determine the pH for the above solution
S
C6H5NH3* (aq) +
OH (aq)
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