# neutralization of a strong acid with a strong base [closed]

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

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

This question appears to be off-topic. The users who voted to close gave this specific reason:

If this question can be reworded to fit the rules in the help center, please edit the question.

• Welcome to Chemistry.SE! Please note that formulas can be better expressed with \$\ce{}\$ for chemical formulas/equations, \$\mathrm{}\$ for math term/equations, and \$\pu\$ for units. More information is available in this meta post Also, take a minute to look over the help center and tour page to better understand our guidelines and question policies. – A.K. Aug 24 '18 at 1:42

## 1 Answer

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.

• Balance sodium hydroxide :$\ce{2NaOH}$ – Adnan AL-Amleh Aug 24 '18 at 4:56
• 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;- $$\ce{H2SO4 + NaOH -> NaHSO4 + H2O}$$ – Adnan AL-Amleh Aug 24 '18 at 7:30