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When a 1M H2SO4 is mixed with an equal volume of 1M NaOH, is the mixture acidic, basic, or neutral?

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closed as off-topic by a-cyclohexane-molecule, DrMoishe Pippik, A.K., Tyberius, Waylander Aug 24 '18 at 10:29

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Since the sulfuric acid is diprotic, the reaction of sulfuric acid with sodium hydroxide has a 1:2 ratio, with twice as much sodium hydroxide being used up in the reaction. The neutralization reaction would be:

$\ce{H2SO4 + 2NaOH -> Na2SO4 + 2H2O}$

After that reaction is complete, approximately half of the sulfuric acid remains, and you would be left with an acidic solution.

Edit: As was pointed out below, I failed to balance my sodium hydroxide.

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    $\begingroup$ Balance sodium hydroxide :$\ce{2NaOH}$ $\endgroup$ – Adnan AL-Amleh Aug 24 '18 at 4:56
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    $\begingroup$ Since hydroxide ion is a monoprotic base and sulphuric acid is a diprotic acid , there are actually two equations involved. Because we have an equimolar amount of acid and base, the products of the first reaction are sodium bisulfate and water;- $$\ce{H2SO4 + NaOH -> NaHSO4 + H2O}$$ $\endgroup$ – Adnan AL-Amleh Aug 24 '18 at 7:30

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