I did an experiment in class, where I was given 2.00g of an acidic solid 'H3X'. I made a 250cm3 solution of water and the acid and titrated it against 25cm3 of 0.100 mol dm^-3 of NaOH.
The equation is H3X(aq) + 3NaOH(aq) = Na3X(aq) + 3H2O.
I have been given these questions to complete.
1. My average titre. This question was fairly simple, I calculated a mean of all my titres to get an average of 21.54cm^3.
2. Moles of NaOH. For this I did (25/1000)*0.100 to get 2.5*10^-3.
3. Calculate the amount of moles of H3X in your mean titre. For this I simply divided my moles of NaOH by 3 since it is in a 1:3 molar ratio, to get 8.3*10^-4.
4. Calculate the amount, in mol, of H3X present in the 250cm^3 solution that you prepared. For this do I just have to multiply the moles I calculated previously by (250/21.54) since it is the mean titre I got and I multiply it by the factor.
5. Calculate the molar mass, in g mol-1 of H3X (dot) nH2O. This part I am slightly confused on. For this, all I assumed is to use the formula n=m/Mr but this must be wrong since it is a dot formula with water so I obviously can't just use the mass of H3X by itself, so I am unsure about this.
Any help is appreciated, thank you very much.