2HOCl + 2H^+ + 2e ==> Cl2 + 2H2O..Eo=1.63
Cl2 + 2e ==> 2Cl^-..............Eo = 1.369
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2HOCl + 4e + 2H^+ ==> Cl2 + 2H2O E=
[(2*1.63)+(2*1.369)/4] = ?
b.
Use the Nernst equation.
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?
2 answers
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?
1 answer