The state after the sodium hypochlorite solution becomes saturated
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This post was last edited by sunjl1981 on 2013-1-6 at 23:25. Sodium hydroxide reacts with chlorine to produce sodium hypochlorite; if a certain amount of solution continues to react until sodium hypochlorite becomes saturated, can the solution still react with chlorine? # hcbbs
Sodium hypochlorite cannot become saturated at normal temperature and pressure; it is a product of the reaction between a base and chlorine gas! When a certain control value is reached, continuing the reaction will lead to hyperchlorination, with sodium hypochlorite decomposing instantly! (As long as there is alkali, chlorine will react with it.)
Continuing to pass chlorine will produce a large amount of sodium chloride, until the reaction stops due to the absence of alkali
In the production process, sodium hypochlorite is obtained by using a 16–17% dilute alkaline solution to absorb chlorine gas and carry out a chlorination reaction; this process releases a certain amount of heat. The effective chlorine content is then controlled at 10–13%, while the excess of alkali is kept at 0.1–1%. Near the end of the process, once the effective chlorine content reaches 8%, it is necessary to measure the pH value, free chlorine content, sodium hydroxide content, and oxidation potential every 5 minutes. Prevent the chlorination reaction from going past its limit, which could trigger a chain reaction that leads to the complete decomposition of sodium hypochlorite. For safety reasons in industrial production, the effective chlorine content is generally kept at around 11%.
I don’t quite understand what you mean. Are you saying that if a saturated solution of sodium hypochlorite is placed in a sealed container, and chlorine gas is added to it, it will keep decomposing?
Could everyone discuss the conditions under which sodium hypochlorite decomposes instantly? What specific factors could lead to such a situation?
Once the sodium hypochlorite concentration reaches saturation, and the temperature remains constant, if there is still free base present, continuing to introduce chlorine will cause sodium hypochlorite to crystallize out.
Sodium hypochlorite will decompose; is the decomposition rate fast?
I believe sodium hypochlorite does not decompose at a pH above 11. Unless you introduce an excessive amount of chlorine, causing the sodium hydroxide to be completely consumed and the pH value to drop below 9, the decomposition rate becomes quite fast once that occurs, with a large amount of chlorine being released from the solution.
Does sodium hypochlorite decompose quickly when exposed to light?
It is estimated that the original poster is asking whether, if the concentration of the alkaline solution is 400 g/L and chlorine gas is continuously introduced, a higher-concentration sodium hypochlorite solution can be produced. It should be like this within the solubility range of sodium hypochlorite. If it is exceeded and there is still unreacted alkali, sodium hypochlorite crystals are likely to form.