Asked by Dave
a)the E0 for the reactions 2HOCl + 2H+ + 2e- → Cl2 + 2H20 and Cl2 + 2e- → Cl- are 1.63 and 1.396 volts respectively. Write the half reaction of HOCl being reduced to Cl- and develop the full pE/pH equation for this reaction.
b)What is the pE of a HOCl/Cl- solution at pH 9.5 if the total chlorine ([HOCl] + [OCl-]) = 5.6E-5M and [Cl-] = 1.0E-3 M? Note that HOCl ↔H+ + OCl- and pKa for this reaction is 7.5. Would you describe this as an oxidizing or reducing solution?
b)What is the pE of a HOCl/Cl- solution at pH 9.5 if the total chlorine ([HOCl] + [OCl-]) = 5.6E-5M and [Cl-] = 1.0E-3 M? Note that HOCl ↔H+ + OCl- and pKa for this reaction is 7.5. Would you describe this as an oxidizing or reducing solution?
Answers
Answered by
DrBob222
2HOCl + 2H^+ + 2e ==> Cl2 + 2H2O..Eo=1.63
Cl2 + 2e ==> 2Cl^-..............Eo = 1.369
-----------------------------
2HOCl + 4e + 2H^+ ==> Cl2 + 2H2O E=
[(2*1.63)+(2*1.369)/4] = ?
b.
Use the Nernst equation.
Cl2 + 2e ==> 2Cl^-..............Eo = 1.369
-----------------------------
2HOCl + 4e + 2H^+ ==> Cl2 + 2H2O E=
[(2*1.63)+(2*1.369)/4] = ?
b.
Use the Nernst equation.
Answered by
Dave
After doing the math, how do you figure out if it is oxidizing or reducing?
How does the pKa apply?
How does the pKa apply?
There are no AI answers yet. The ability to request AI answers is coming soon!