CAS Number for Bleaching Powder

Hi IC,

It's called calcium hypochlorite:

http://www.jtbaker.com/msds/englishhtml/c0418.htm

Mike

Thanks Mike.

So, in other words, CaCl₂O₂ (as presented in the MSDS which you linked) should be considered identical to Ca(OCl)Cl; thereby clearing up the whole nomenclature issue.

Is this true?

Thanks again . . .

I have always seen bleach bottles with "calcium hypochlorite" listed as the main/active ingredient, with the formula being CaCl2O2. The formula Ca(OCl)Cl is not the same (lacking an Oxygen) formula. However, the long list you gave in your original post leads me to believe that there are different "interpretations" of what the exact chemical formula is.

What application is this for? Maybe that would clarify things a little.

Mike

Hmmm... I thought the extra O would be an issue. This substance is confused in the notation --

Well, if it helps, here's what I'm after:

• Ca(OCl)Cl + H₂SO₄ --> CaSO₄ + H₂O + Cl₂

The desired gaseous endproduct: Pure, simple Chlorine on-demand; with a minimum of apparatus. And yes, I do remember to AAA

Now, if we use "Calcium hypochlorite" (represented as CaCl₂O₂ in the Baker MSDS), won't we wind up with a mixture of gasses in place of neat Chlorine as the end product?

Specifically, where will the extra Oxygen wind up? Chlorine monoxide?

Thanks again.

OR, you could have something like this:

4CaCl₂O₂ + 2H₂SO₄ ---> 2CaSO₄ + 2CaO + 4Cl₂ + 3O₂

What do you think?

Mike

Er, wouldn't an excess of sulphuric acid react with the CaO to make more CaSO₄?

Hi PWSlack

I don't think so, but maybe. I'm sure that there other reactions going on as well.

I was just trying to make the dang stoichiometry work!

Mike

The reaction looks a bit dangerous

Try going to:

http://cameochemicals.noaa.gov/

and mixing Sulphuric Acid and Calcium Hypochlorite.

If you don't know it, the website above is very useful for properties, hazards and possible reactions if you mix two chemicals

Thanks for weighing in on this, folks. I do appreciate the helpful input

Thanks, tesser, for the link. One more resource to add to the collection --

However, don't you think that the reaction should be safe with ordinary care, as long as it is not rushed?

@Mikerho:

Your new eq doesn't seem to be balanced.

In any event, I'm concerned about the excess free Oxygen winding up in the end gasses. Then again, would an actual reaction as PWSlack suggests take the extra O up into the resultant CaSO₄? Could this be the real case?

Alternatively, here's a possibility which I'd like to run past everyone concerning the apparent difficulty in nailing down a source/CAS# for actual Ca(OCl)Cl in this application:

• CaCl₂O₂ + H₂SO₄ --> CaSO₄ + H₂O₂ + Cl₂

Is this the reaction which we'd be actually seeing with CAS #7778-54-3 (Calcium Hypochlorite) in place of Ca(OCl)Cl in the above equation? If correct, it'd appear that the extra O would simply be swept into solution with the water; eliminating any contamination of the gaseous Cl₂ endproduct. And, if this is indeed the case, would CaSO₄ be quietly settled sitting in a bath of hydrogen peroxide?

Is this how things would actually turn out by substituting CaCl₂O₂ in the mix???

Thanks again!

It is balanced, but I don't know if I predicted the products accurately, and I can't really say for sure that you would get H2O2 as a product. I've been too long away from chemistry.

As a safety concern, (http://cameochemicals.noaa.gov/reactivity#Pair_1) what conc. of H2SO4 are you thinking of using?

Mike

Try Google-ing your compound. Put in the formula. They have a partial print of a 1920's book on industrial chemistry by Mann which I think will answer your question.

@Guest:

I found this by Martin.

If you're still here, is that the citation which you saw?

Thanks . . .

@All:

Thanks again for your help; and have a good day