U E a. At equilibrium the concentrations of the ionized substances are: [C6H5NH₂] = 0.0537 mol/L [C6H5NH3*] = 4.79 x 10-6 mol/L [OH-]= 4.79 x 10-6 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)
U E a. At equilibrium the concentrations of the ionized substances are: [C6H5NH₂] = 0.0537 mol/L [C6H5NH3*] = 4.79 x 10-6 mol/L [OH-]= 4.79 x 10-6 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)
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section15.6: Disturbing A Chemical Equilibrium
Problem 15.7CYU: Equilibrium exists between butane and isobutane when [butane] = 0.020 M and [isobutane] = 0.050 M....
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PLEASE USE THE TABLE AND FILL IN EVERYTHING AS WELL AS SOLVE THE PROBLEM> HAND WRITTEN WOULD BE GREAT!
![U
E
a.
At equilibrium the concentrations of the ionized substances are:
[CH5NH₂] = 0.0537 mol/L [C6H5NH3*] = 4.79 x 10-6 mol/L
[OH-]= 4.79 x 10-6 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 K₂ for the above solution
3. Determine the pH for the above solution
S
С6H5NH3* (aq) +
OH(aq)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2353b354-afd7-4909-9448-0417ddbb2247%2F1759abbe-04ec-434f-a667-4616a313b0d3%2Fzoux0tm_processed.png&w=3840&q=75)
Transcribed Image Text:U
E
a.
At equilibrium the concentrations of the ionized substances are:
[CH5NH₂] = 0.0537 mol/L [C6H5NH3*] = 4.79 x 10-6 mol/L
[OH-]= 4.79 x 10-6 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 K₂ for the above solution
3. Determine the pH for the above solution
S
С6H5NH3* (aq) +
OH(aq)
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