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

Answer 1

Naomi Aronson

#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#.

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Answer 2

Ellie Andrews

To find the number of milliliters of 2.00 M H2SO4 needed to react with 28.0 g of NaOH, you first need to calculate the number of moles of NaOH using its molar mass, then use the balanced chemical equation to determine the stoichiometric ratio between NaOH and H2SO4, and finally use the concentration of H2SO4 to find the volume required.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.