a. 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) Determine the K₂ for the above solution Determine the pH for the above solution ş С6H5NH3* (aq) + OH (aq)
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Grade 12 Chemistry - Kindly review each step and fill out the table. Your assistance is greatly appreciated.
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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?
С6H5NH₂ (aq)
+ H₂O (l)
2. Determine the K, 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%2F66a4250c-c541-48c2-9c59-dbec97eb3a97%2Fc1a35801-2027-4bd5-8231-795b90e166dd%2Fmrc3hx_processed.png&w=3840&q=75)
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