Oops… when working with hazardous materials, I suppose it is evidently often a good idea to read the label first 
9% but dilute 1:8 before use. Thanks for that, mbakron!
At milder strengths, peroxides are bleaches. At higher strengths, peroxides are literally, fire in a bottle – the ability to oxidize is what fire does, but which peroxide does chemically instead of via heat/energy exchange physics.
The milder peroxide mouthwash is excellent for getting gums back into shape, heh… an old person observation, no doubt …
Well, the reactions of peroxide or hypochlorite, (bleach,) on pheromones at room temperature are a bit more predictable than “fire in a bottle.” But nevertheless, they do a good job of tearing pheromones to pieces. And what they don’t tear up, they make easier for other things to tear up. If you’re a chemist, think epoxidation, Baeyer-Villiger reactions, oxidations of vicinal diols, etc. You’re not getting “fire in a bottle” unless it’s quite concentrated and you mix it with a strong reducing agent, which would also have to be quite concentrated.
Fortunately, the skin is much more resistant to these oxidation reactions than pheromones are… but I wouldn’t pour concentrated peroxide on my skin!
For those that don’t care about the science, just know that peroxide and bleach work, and there’s solid science out there saying they do. And they’re safe as long as they’re reasonably dilute.