# Redox problem involving Na2S and HSO4- [on hold]

I'm trying to complete a question on an assignment that says

Show all steps in determining the number of electrons an atom of sulfur loses when it changes from sodium sulfide to hydrogen sulfate ions in a reaction.

I can't come up with a chemical equation for this scenario. I'm assuming I need one more reactant and one more product to go from

$$\ce{Na2S -> HSO4-}$$

but I have no idea what.

Would it be 8e- lost since the oxidation number of S in $$\ce{Na2S}$$ is -2, and the oxidation number of S in $$\ce{HSO4-}$$ is +6?

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## put on hold as off-topic by Todd Minehardt, user55119, Karsten Theis, Poutnik, Jon CusterJun 13 at 13:02

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• Are you familiar with the concept of oxidation numbers? That would be a key tool to write down this oxidation half reaction (loss of electrons is oxidation). – Karsten Theis Jun 13 at 3:32
• The assignment doesn't ask you to provide the complete reaction; all you have to do is to determine oxidation numbers of sulfur and make a conclusion regarding the number of electrons based on that. – andselisk Jun 13 at 6:23
• @andelisk so would it be 8e- lost since the oxidation number of S in Na2S is -2, and the oxidation number of S in HSO4- is +6? – Insanit Jun 13 at 11:53