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I´m not a chemist - far away from that but can´t this be explained by looking att the reaction as a disproportionation reaction there the reduction (forming of H2O) will be happen faster than the oxidation (forming of O2 or oxidation of some other substances with help o the free oxygen radicals). In my no chemical brain I see it like the following scenario. - The reduction process (forming of H2O) happens directly when the O atom leave the H2O2 molecule but in order to fulfil the oxidation process the free O atom has to find another O atom or another molecule. It will be a time lap between the two processes – therefor we see it as a lower ORP (due to H2O forming) followed of a rise in ORP (forming of O2 or other oxidized molecules)
I will not argue with you about it – its only a suggestion that can give an explanation to the observed measurements.
@DangerDave
I think that you got a to fast reaction in the plastic chamber and that to much H2O2 was pressed out in the water column in a speed that the secondary catalyst did not managed and therefore you get a situation rather alike dosing H2O2 directly into the water column. Not so many catalyst or lower concentration of H2O2 in the plastic chamber will probably be the best way to go.
Sincerely Lasse
My thought is the way the oxygen ions in peroxides are charged, -1, instead of -2 for o2. So when the h2o2 is added to the water it's hitting the orp probe with a lower charge along the the normal o2 and O radicals in suspention. Thus pulling down the orp reading. As the h2o2 decays and releases the 2nd oxygen atom the charge rises, as seen by the probe, until the h2o2 is depleted. Then it will slowly equalize to norm for the tank.
Is this, even remotely, the correct way of looking at it?
One thing I did notice is how it dropped my PH at times. When I fill it and replace, I have to do some creative maneuvering to get it back into the holder. It also bangs around a bit as I put the strap back on. When this happens my PH drops to the low 200's very quickly. I'm assuming that i'm releasing some h202 directly when this happens. I also get a PH drop whenever my return pump turns off and back on, which is mostly when I feed. It goes up much faster in this example, but not as fast as it goes down.
Dave
Thanks for the suggestion. I'm still trying to understand the typical drop that is seen.
The disproportion reaction certainly can happen, and there are many different species that form from hydrogen peroxide (HO2-, OH., O2, - OOH, HO+, ertc.).
I just don't see any of those being likely to reduce ORP. A free O atom, ifit formed, is not an ORP reducing species. It is highly oxidizing.
You mean the ORP - not the pH - I suppose
Sincerely Lasse
Go for it, what water volume tank?
If you can accommodate it I would go for the W model with that volume of water.200 gallons.
If you can accommodate it I would go for the W model with that volume of water.
Yes that seems about right. I use 2 oxydator As. In 100 gallons using 9% peroxide and 2 catalysts but my tank is very full and I feed a lot.Do you know the dimensions of it off the top of your head? I only had time for a quick search but I came up with 18 cm x 15 cm. Does that seem right?