HClO and hypochlorite both have strong oxidizing properties, that is, ClO- also has strong oxidizing properties and does not need to be converted into HClO when reacting with strong reducing agents
Hypochlorous acid When salt reacts with other strongly reducing solutions, it is not necessarily true whether all H2O participates in the reaction. In fact, it is a question of whether to balance with H or OH- when balancing. This ionic equation has not been examined much, but When encountered, pay attention to the acidity and alkalinity of the solution system to determine how to balance it.
For example, when NaClO reacts with Na2S, it should be noted that both NaClO and Na2S are strong bases and weak acid salts that hydrolyze, so their aqueous solutions are alkaline, so the balance of this reaction requires OH- and H2O, that is,
ClO-
S2-
H2O=
Cl-
S
2OH-
That is, H2O participates in the reaction
The reaction between NaClO and Na2SO3 should also be carried out under alkaline conditions, because both salts are alkaline when hydrolyzed, but after balancing, it was found that
ClO-
SO3^2-
=
Cl-
SO4^2-
So, just right, no other ions or H2O are needed
For example, if you pass excess SO2 into the NaClO solution, be aware that excess SO2 means that the final solution is acidic. , so use H and H2O when balancing
ClO-
SO2
H2O
=
Cl-
SO4^2-
2H
That is, H2O also participates in the reaction
For example, when NaClO and FeCl2 are reacted, it is noted that NaClO is alkaline when hydrolyzed, and FeCl2 is acidic when hydrolyzed. Therefore, when writing this equation, you must pay careful attention to the title. Description, if the question only says that the solution changes from light green to brown, that is, Fe3 is generated, then it means that it is balanced under acidic conditions
ClO-
2Fe2
2H
=
Cl-
2Fe3
H2O
It can be seen that H2O is a product