Sodium hypochlorite calculation
Thread Content
It is known that there is a 60-ton mixture of sodium hypochlorite and sodium chloride, and the effective chlorine content was determined using the iodometric method to be 6%. What is the mass fraction of NaClO? And what is the mass of sodium hypochlorite in 60 tons of solution? My calculation is as follows: in 100% NaClO, the content of available chlorine (Cl) is 35.5/74.5*100% = 47.65%. Therefore, the mass percentage of NaClO required for 6% available chlorine is (6%*100%)/47.65% = 12.59%, and the mass of sodium hypochlorite needed is 60*12.59% = 7.55 tons. I wonder if there’s an error in my calculation method? Or it's a misunderstanding. Thank you all!
Hello, my friend. I’m not here to answer questions, but our factory uses sodium hypochlorite as an oxidizing agent, with the concentration of this substance being controlled at around 0.085–0.12 each time it’s prepared. I have a question: does \"effective chlorine\" refer to chlorine atoms or to higher-valent chloride ions?
Indeed, what is the concept of effective chlorine?
Hello, the attachments contain two introductions on available chlorine and sodium hypochlorite; take a look and you’ll understand!
There are also a few papers here for your reference; the concept of effective chlorine can be understood from the formulas.
The definition of effective chlorine refers to the oxidizing power contained in hypochlorite, expressed as equivalent to that of pure chlorine gas (by strict definition: it is the ratio of the mass of chlorine gas [Cl2] required to oxidize an equal amount of elemental iodine [I2] from potassium iodide [KI] to the mass of the compound in question, usually expressed as a percentage). Thus, one unit of effective chlorine corresponds to the presence of one NaClO molecule, and it also corresponds to the presence of one Cl2 molecule (since the oxidizing power of NaClO is twice that of Cl2 due to the difference in oxidation states)