Did a copy and paste from a different group looking for answers.
It sounds to me like you can mix it with mms2 and the DMSO will take out the free chlorine in the solution, which is a good thing, while not affecting the chlorine dioxide and other oxychlorines. However, if you have a strong mms2 solution, it will be very acidic and they are saying it could be enough to oxidize the DMSO, and I don't know how good or bad that could be.
I went to that link and you can't tell what that article is about. I don't think they are doing this in human bodies, it sounds like it is reactions under lab conditions.
If you are going to test it, I would do it on your skin first. Start out with low dilutions and use it on a healthy person's skin.
What you should do Gary is go here
genesis2forum.org/index.php?option=com_kunena&func=showcat&catid=2&Itemid=66 and ask Bruce (brtanner) this question, about using DMSO with mms2. Just start a new topic in the questions re mms section. He went through Jim's training and he'll answer by tomorrow morning.
Michael Harrah
Original Message
From: Gary Stauffer
To:
This email address is being protected from spambots. You need JavaScript enabled to view it.
Sent: Monday, January 10, 2011 7:56 PM
Subject: [Humble_MMS] Research?
Let us figure out with this is saying no mix dmso for use with mm2 water or yes mix dmso with mms2 water?
pubs.rsc.org/en/Content/ArticleLanding/1995/AN/an9952001983
The aim of this work was to demonstrate that dimethylsulfoxide (DMSO) is an excellent masking agent for aqueous chlorine in the determination of other oxychlorines. By the addition of excess DMSO, specific absorbance of free chlorine disappeared, and the oxidation of iodide to iodine by chlorine was completely prevented. Chlorine dioxide, chlorite and chlorate were not affected by the co-existence of excess DMSO, but chlorosulfamic acid, showed results comparable to free chlorine. By using ion chromatographic analysis of the mixed solution of free chlorine and DMSO, chloride was recovered as the only anionic species and its molar concentration was approximately twice the initial chlorine concentration. DMSO seems to reduce and mask chlorine completely, without affecting other oxychlorines. Chlorine and DMSO reacted in the molar ratio of 1:1 The reaction seemed to be second-order. The rate constant was larger at a lower pH, and it was dependent not on a concentration of total chlorine, but on that of hypochlorous acid. The redox potential of DMSO was higher at a lower pH, and only hypochlorous acid would have a redox potential high enough to oxidize DMSO in acidic conditions. These results suggest that DMSO reacts with hypochlorous acid stoichiometrically. In practical use, DMSO may be successfully used as a masking agent for aqueous chlorine.
The use of DMSO as a masking agent for Cl2 was investigated. Under neutral and acidic conditions, DMSO selectively reacted with free and combined Cl2 and did not affect oxychlorines such as chlorine dioxide (ClO2), chlorite and chlorate. The utility of DMSO as a masking agent for Cl2 was demonstrated by the titrimetric, voltammetric and spectrophotometric determination of various oxychlorines (mainly ClO2) in the presence of Cl2. The mechanism of the reaction between DMSO and Cl2 is also discussed.
