[Gabu]

Hi, guys. I'm sorry if this is too basic a question but I'm at a basic level and I'm having trouble solving it.

The question is

'One-tenth of a kg of an aqueous solution of HCl is poured into 0.2kg of an aqueous solution of NaOH. The mole fraction of the HCl solution was 0.1, whereas that of the NaOH solution was 0.25. What are the mole fractions of each of the components in the solution after the chemical reaction has come to completion?'

I have calculated the amount of each component before they are mixed together:

For the first solution:

M(HCl)=0.5035 mol
M(H₂O)=4.5315 mol

For the second solution

M(NaOH)=2.1267 mol
M(H₂O)=6.3801 mol

I know that

HCl+NaOH NaCl + H₂O

and given the amounts of components in the original solutions, my equation should be

0.5035 HCl + 2.1267 NaOH + 10.9116 H₂O  NaCl + H₂O

How can I balance this if I cannot change what's in the l.h.s. of the equation?

Thank you very much.

[Borek]

Reaction equation doesn't depend on the amounts of the substance. Find out what was the limiting reagent.