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Registered Member #690
Joined: Tue May 08 2007, 03:47AM
Location: New Jersey, USA
Posts: 616
So I was at work the other day, and we were getting ready to mop up at the end of the night. The mop bucket has 2 cleaners added, bleach and something called G.P. Fresh (?). After the bleach is added to the hot water, the GP Fresh, which is dark green, turns clear instantly upon being added, up to a very specific point after which it remains green.
I know bleach's NaOCl is a weak acid, and on further inspection of the label on the GP Fresh, I see "It's slightly acidic pH will not harm floors..." and on the ingredients, citric acid is present.
What I'm wondering is, what causes the color change? Could the dye just be naturally pH sensitive?
Registered Member #8
Joined: Thu Feb 02 2006, 04:34AM
Location: Harlowton, MT, United States
Posts: 214
NaOCl is not an acid, as it has no H+. In fact typical bleach solutions contain a significant amount of sodium hydroxide left over from production. As a strong base, this likely caused the reaction. The dye could be an inadvertant pH indicator, or possibly the chemicals in the bleach just reacted with it regardless of pH, destroying the color.
Registered Member #193
Joined: Fri Feb 17 2006, 07:04AM
Location: sheffield
Posts: 1022
All the bottles of bleach I have seen (at least since I started reading that sort of thing) have warned that they shouldn't be mixed with other products. Does yours?
Registered Member #690
Joined: Tue May 08 2007, 03:47AM
Location: New Jersey, USA
Posts: 616
Well, yea, both bottles do say that, but my boss(es) are what you might call, well, chemically retarded. I saw no bubbles or foam forming (which I have seen with a mix of bleach and hand soap with bleach alternative), just the color change. I figure at the most it makes it clean worse by partially neutralizing the cleaning agents.
The possibility that the bleach simply destroys the dye makes a lot of sense to me now. That is what bleach is known for, right? Oxidizing away color?
Registered Member #530
Joined: Sat Feb 17 2007, 07:56AM
Location: Victoria BC, Canada
Posts: 178
Mixing strong Acids with NaOCl based products is a BIG no no! Its a fast way to wind yourself up in the ER with a serious case of Chlorine gas poisoning! I once saw a nasty accident with Industrial bleach and liquid drain remover - 95% H2SO4 --- VERY violent reaction and lots and lots of Chlorine gas....
Registered Member #690
Joined: Tue May 08 2007, 03:47AM
Location: New Jersey, USA
Posts: 616
Believe me, I know where you're coming from. I had a few nice whiffs of Cl2 during a chlorate electrolysis process. As I said, no bubbles were formed upon mixing. I know this doesn't neccesarily mean no gas is forming (see aqueous NaOH + NH4NO3 solution), but if anyone would recognize the scent of chlorine, it would be me, and there was none. A small amount probably did form initially, but there was so much water and so little reagent, that the gas should have just gone into solution, as it is fairly soluble.
I do my best to stay safe, really, but acids and gases tend to make you rethink your methods...
Registered Member #32
Joined: Sat Feb 04 2006, 08:58AM
Location: Australia
Posts: 549
Yes, bleach has a nasty habit of releasing chlorine gas (or worse) with a whole range of chemicals.
wrote ...
NaOCl is not an acid, as it has no H+.
On a technicality, an acid doesn't have to contain H+, depending on definition. The common high-school acid definition is centred on H+ (the Bronsted-Lowry definition, I think it is) but there are other kinds of acid.
FeCl3 (that etchant) is considered a kind of acid. Formally it is a Lewis acid. No H whatsoever.
Edit: Whoops! Thanks BC! Embarrassing... (I'm supposed to be a chem tutor, too...)
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