H+ and OH-

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If you just have an aqueous electrolyte with virtually no H+ or OH- ions (neutral), will water spontaneously produce them if required? e.g.

[TrueTears]

How would it produce the ?

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?

[TrueTears]

I see but where is that in the original equation?

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It was just an example. You could use a few other half equations to balance, i think, e.g.

[TrueTears]

It was just an example. You could use a few other half equations to balance, i think, e.g.

Hmm I see but where would the be in that equation?

[Collin Li]

If you just have an aqueous electrolyte with virtually no H+ or OH- ions (neutral), will water spontaneously produce them if required? e.g.

Yes, but not nearly enough for any significant rate of reaction. (Around ~)

This half-equation needs an acidified conditions in order to operate functionally (and 1M for electrochemical series to work)

P.S.: Excited to be unveiling a great and free solution to these kind of short (but important and conceptual) questions soon!

[NE2000]

It was just an example. You could use a few other half equations to balance, i think, e.g.

Hmm I see but where would the be in that equation?

Combine with the previous half equation with the H+