Neutralize chlorine solution with sodium percarbonate solution

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SUMMARY

Neutralizing a 3% sodium hypochlorite solution with an 85% sodium percarbonate solution is not feasible due to both being oxidizing agents. The discussion highlights that while hydrogen peroxide can act as a reducing agent in certain conditions, mixing sodium hypochlorite with sodium percarbonate may leave harmful residues on vegetation. A safer alternative suggested is using sodium sulfite to neutralize sodium hypochlorite, or exposing it to direct sunlight to convert it into salt and oxygen, although caution is advised regarding potential sodium chlorate formation.

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  • Understanding of sodium hypochlorite properties and applications
  • Knowledge of sodium percarbonate and its chemical behavior
  • Familiarity with oxidation-reduction reactions
  • Basic principles of chemical safety in outdoor environments
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xilix
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Hello,

Would it be feasible to neutralize the effects of a 3% sodium hypochlorite and water solution by adding an appropriate proportion of an 85% sodium percarbonate powder and water? What would the appropriate proportion be to facilitate this premise? Would the resulting reaction be safe if performed in an open outside environment?

I will be using the chlorine solution to clean algae off of my roof but i am worried the SH solution will damage my plants. So the idea is to soak the surrounding vegetation with a sodium percarbonate and water solution that is proportionally correct to accomplish this task.

Thank you.
 
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Unless I am missing something you are talking about two oxidizing agents, so no, I don't see how it could work.
 
Hmm, I have seen experiments done with chlorine (sodium hypochlorite) and hydrogen peroxide (H202) with the product of the reaction being a release of 02 and salt water. Based on that, I figured that mixing the two mentioned solutions would have a similar end result.
 
On the second thought, in correct conditions hydrogen peroxide can work as a reducing agent. Still, I don't like the outcome - as it is impossible to follow the exact stoichiometry, you are left with the excess of either hypochlorite of peroxide, neither is a thing I would like on my grass. If anything, sodium sulfite would be much safer, at least IMHO.
 
OK, there are heavy metals that decompose NaOCl, but I agree (especially Copper Oxide and other copper salts which are generally deadly to lower organisms, fungi, fish,...) you may not want on your lawn.

However, Fe2O3 will also decompose, albeit slowly, NaOCl and Iron is certainly more acceptable.

The ultimate green solution is to expose the NaOCl to direct sunlight, resulting in NaCl and liberating O2. However, in diffused light it is possible that some Sodium Chlorate (a weed killer) will be formed (as a result of the disproportionation of the NaClO).
 

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