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Chemistry Forums for Students => Analytical Chemistry Forum => Topic started by: darknietzsche on September 01, 2008, 01:35:33 PM

Title: gravimetric analysis
Post by: darknietzsche on September 01, 2008, 01:35:33 PM

I have another question involving gravimetric analysis:

A 0.2795 g sample of an organic mixture containing only C₆H₆Cl₆ (290.83 g/mol) and C₁₄H₉Cl₅ (354.49g/mol) was burned in a stream of oxygen in a quartz tube. The products (CO₂, H₂, and HCl) were passed through a solution of NaHCO₃. After acidification, the chloride in this solution yielded 0.7161 g of AgCl (143.22g/mol). Calculate the percentage of each halogen compound in the sample.

Really I need to know where to begin. All I know to do to begin with is convert g of AgCl to moles:

moles of AgCl=.005 moles.

If you could explain where to begin in terms of the chemistry basis it would be greatly appreciated.

Title: Re: gravimetric analysis
Post by: Borek on September 01, 2008, 02:30:28 PM

Assume there were x moles and y moles of compounds, write equations for total mass of mixture and number of moles of chlorine.