E' I C 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? С6H5NH₂ (aq) + H₂O (l) 2. Determine the K₂ for the above solution 3. Determine the pH for the above solution 누 С6H5NH3* (aq) + OH (aq)

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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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 K, for the above solution
3. Determine the pH for the above solution
S
C6H5NH3* (aq) +
OH (aq)
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 K, for the above solution 3. Determine the pH for the above solution S C6H5NH3* (aq) + OH (aq)
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