- #1
i_love_science
- 80
- 2
- Homework Statement
- Is OCl- both reduced and oxidized in the reaction between sodium hypochlorite and hydrogen peroxide?
- Relevant Equations
- Redox reactions
For the reaction between hydrogen peroxide and sodium hypochlorite, is the OCl- both reduced and oxidized?
H2O2 + NaOCl -> NaCl + H2O + O2
Oxidation states:
+1 -1 +1 -2 +1 +1 -1 +1 -2 0
From the oxidation states, it seems that Cl is reduced from +1 to -1, and O (of NaOCl) is oxidized from -2 to 0.
On the contrary, the half reactions given by the solution are:
2 e- + 2H+ + OCl- -> Cl- + H2O
H2O2 -> O2 + 2H+ + 2 e-
In this case, the OCl- is reduced only.
What is the real case? Thanks.
H2O2 + NaOCl -> NaCl + H2O + O2
Oxidation states:
+1 -1 +1 -2 +1 +1 -1 +1 -2 0
From the oxidation states, it seems that Cl is reduced from +1 to -1, and O (of NaOCl) is oxidized from -2 to 0.
On the contrary, the half reactions given by the solution are:
2 e- + 2H+ + OCl- -> Cl- + H2O
H2O2 -> O2 + 2H+ + 2 e-
In this case, the OCl- is reduced only.
What is the real case? Thanks.
Last edited: