Ok, thanks, I thought I might be overthinking this, but I wanted to be sure.
Well the label says it is CaCl2. If you put 1 gram of that in 1 gal of water you will get 95.4 ppm Ca++ and 168.9 mg/L Cl-. If, OTOH, you put 1 gram of the dihydrate (CaCl2.2H2O) in 1 gal of water you would get the numbers on the label. So either the CaCl2 labeling is wrong or the concentrations are wrong.
Well the label says it is CaCl2. If you put 1 gram of that in 1 gal of water you will get 95.4 ppm Ca++ and 168.9 mg/L Cl-. If, OTOH, you put 1 gram of the dihydrate (CaCl2.2H2O) in 1 gal of water you would get the numbers on the label. So either the CaCl2 labeling is wrong or the concentrations are wrong.
When we buy it it's sealed in those little handy jars but somewhere along the line someone bought it in bulk and put it in those little jars and during that process there is a good possibility that it picked up water. Then, of course, we open the jar, take out a little and close it again. More exposure to air. OTOH if you look at specs for CaCl2 you see things like 77-80% with Dow bragging that theirs is 80 - 83%. I think this probably represents a mix of anhydride and dihydrate (though there are other impurities to like the calcium hydroxide I mentioned in an earlier post).Calcium chloride is highly hygroscopic, so isn't it possible that the stuff is coming from a supplier and over time picking up water?
Thanks for the compliment but it's probable that a lot of it is that I'm not familiar with the assay and am screwing it up.Maybe that's why your findings are inconclusive.
I guess we all need to be concerned with that.
As I recall, the temperature needed to move these various hydrates back toward an anhydrous state increase with each hydrate reduction.
Do I recall correctly that the best we could probably do in drying out these hydrates in a typical home oven is about the dihydrate version?
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