Saccharin (C7H5NO3S) is sometimes dispensed in tablet form. Ten tablets with total mass of 0.5369 g were dissolved in water. They were oxidized to convert all the sulfphur to sulphate ion, which was precipitated by adding an excess of barium chloride solution. The mass of BaSO4 obtained was 0.5118 g.
What is the average mass of saccharin per tablet in mg?
What is the average mass percent of saccharin in the tablets?
I'm not sure if I'm on the right track:
.5032gBaSO4 / 233.33g =.001085mol BaSO4
.001085mol * 32.07gS=.03480gS
Not sure where to go from there. Can anyone help?
2007-10-02 12:08:45 · 1 answers · asked by Nhat t 1 in Science & Mathematics ➔ Chemistry
Where did you get the data of .5032gBaSO4 in the problem?
Anyway, BaSO4 contains one atomic sulpher. Saccharin (C7H5NO3S) contains one atomic sulpher. Thus one mole of Saccharin (C7H5NO3S) may generate one mole of BaSO4. Your second step is not necessary. When you find the CORRECT number of moles of BaSO4, that is the number of moles of initial Saccharin (C7H5NO3S).
Good Luck!
2007-10-02 13:45:26 · answer #1 · answered by Hahaha 7 · 0⤊ 0⤋