[rk_1993]

I had to find out the accurate concentration of sulphuric (VI) acid in a sample of the acid solution that is thought to have a concentration between 0.05 and 0.15 moldm^-3. I had to do this by titration with sodium carbonate.
what calculations do I have to carry out to find the accurate concentration of the sulphuric acid? Thanks in advance.
 (btw I have done the titration and I've got the results. I've also calculated the concentration of sodium carbonate in my standard solution)

[sjb]

What is the equation of the reaction you carried out?

[rk_1993]

H2SO4(aq) + Na2CO3(aq) --> Na2SO4(aq) + H2O(l) + CO2(g)

[sjb]

So how many moles of acid react with 1 mole of carbonate?

[rk_1993]

1:1?

[sjb]

Sounds good to me. How much carbonate did you use up in your titration?

[rk_1993]

Sorry, I'm not sure what you're asking for?

[sjb]

If you know the amount of carbonate you used up in the titration, you can work out how much acid you had

[rk_1993]

225cm^3

[sjb]

That's a volume, is it solid sodium carbonate? Or a solution?

[rk_1993]

I used 2.60g of solid sodium carbonate

[sjb]

2.60 g in 225 cm³? If so, how many moles of sodium carbonate is that?

[rk_1993]

sorry, 2.60g in 250cm^3

2.60/105.98
=0.0245329307 mol

[sjb]

OK, so how many moles of acid did you consume in your titration?

[rk_1993]

0.2406199021 mol