I have a feeling I've done the last part of this wrong- can you please check this for me:
Ammonia sample was dissolved in water to produce 100cm3 of a solution, X. 10cm3 of this was made up to volume of 250cm3. 25cm3 of this diluted ammonia solution was titrated with hydrochloric acid of concentration 0.11moldm-3. 37.1cm3 of acid was required to neutralise.
1) Find number of moles of ammonia in solution X
Moles HCl = 37.1/1000 x 0.11 = 0.00408mol
Moles in 250cm3 = 0.0408mol
Moles in 10cm3 = 0.0408/25 = 0.00163mol
Moles in 100cm3 = 0.0163mol
2) Calculate concentration of solution X
Conc. = 0.0163/ (100/1000) = 0.163moldm-3
Does this look right? Please correct me if it isn't! Thanks
Brilliant- thanks thanks thanks!