If 12.3g of H2SO4 is neutralized by 0.25M NaOH, what volume of NaOH solution is required?

Question

H2SO4 + 2NaOH -> Na2SO4 + 2H2O

Help!
How to I even begin to solve this?!

Answer 1

Find the molar mass of the NaOH. Then do a conversion to the units of volume you are suppesed to answer the question in.

Answer 2

The molar mass of H2SO4 equals Mr = 98, so the 12.3 g of H2SO4 are:

n = m/Mr = 12.3/98 = 0.125 mol approx.

Now from the chem. equation:

H2SO4 + 2NaOH -> Na2SO4 + 2H2O

we see that 1 mol of H2SO4 requires 2 mol of NaOH, so the 0.1255 mol require 2*0.1255 = 0.25 mol of NaOH, approx. But:

n = C*V, so V = n/C, V = 0.25/0.25, V = 1 L.

Answer 3

You need 2 moles of NaOH to neutralize 1 mole of H2SO4.
You need to find out how many moles H2SO4 you have.
You can find the atomic masses of H, S, and O per mole in the periodic table. In H2SO4 you have 2 moles of H, 1 mole of S, and 4 moles of O. Just do simple multiplication and addition to find the weight of 1 mole of H2SO4.
Divide 12.3g by the weight of 1 mole to get the number of moles of H2SO4 that you have.
You will need twice that many moles of NaOH.
You know you have .25 moles of NaOH per litre of NaOH solution, so it's simple math after that.

Answer 4

you must have some information about the molarity of the acid, then it is a simple matter of algebra:

molarity of acid X volume of acid = molarity of base X volume of base.