In the "reducing agent" article in Wikipedia it says
Good reducing agents are reagents that deliver $\ce{H2}$.
Wouldn't that make water unsafe to dissolve oxidizing agents?
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2$\begingroup$ I don't quite see how the statement about reducing agents is related to the safety of dissolving oxidising agents in water. Perhaps you could clarify this. $\endgroup$– bonCommented Jun 15, 2015 at 16:40
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$\begingroup$ @bon I think OP means that water may deliver $\ce{H2}$ and is as such unsafe to dissolve oxidizers in. $\endgroup$– tschoppiCommented Jun 15, 2015 at 16:50
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1$\begingroup$ Water doesn't deliver $\ce{H_2}$ though... $\endgroup$– Ali CaglayanCommented Jun 15, 2015 at 17:22
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2 Answers
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If the oxidizing agent is sufficiently strong, e.g. fluorine, yes. "[W]ater spontaneously combust[s] under a fluorine jet."
However, there are only a few oxidizers, such as fluorine, chlorine trifluoride, and dioxygen difluoride that can displace oxygen from water. More likely you'd encounter a strong reducing agent, such as Group I metals, that would attach to the oxygen in water, liberating hydrogen.
answered Jun 15, 2015 at 20:46
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$\begingroup$ A 3% solution of hydrogen peroxide bleaches hair pretty well, and it is a neutral solution. In the lab, you can get a 35% $\ce {H_2O_2}$ solution. $\endgroup$– LDC3Commented Jul 27, 2015 at 1:47
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The safety arises from the solution's characteristics. Some oxidizers produce highly alkali solutions which pose personnel risks from chemical burns. This nature occurs to a lesser extent when dry chemical contacts the skin or mucus membranes ext. as the agent acquires water from the body and in essence forms saturated solutions at the contact sites.
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