How many milliliters of 2.00 M #H_2SO_4# will react with 28.0 g of #NaOH#?

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Answer 1 · 2016-06-11T05:19:04

#175*mL# of the given sulfuric acid.

We need (i) a balanced chemical equation:

#H_2SO_4(aq) + 2NaOH(aq) rarr Na_2SO_4(aq) + 2H_2O(l)#

And (ii) equivalent molar quantitites:

#"Moles of NaOH"# #=# #(28.0*g)/(40.0*g*mol^-1)# #=# #0.70*mol#

Given the stoichiometry of the reaction, we require a half equivalent of sulfuric acid, i.e. #0.35*mol#.

So we divide this molar quantity by the concentration to get an answer in #mL#.

#"Volume"# #=# #(0.35*mol)/(2.0*mol*L^-1)xx1000*mL*L^-1# #=# #175*mL#.