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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: needhelpplz on September 10, 2007, 08:01:22 PM

Title: Mass Percent Problem~
Post by: needhelpplz on September 10, 2007, 08:01:22 PM

Douglasite is a mineral with the formula 2 KCl·FeCl2·2 H2O. Calculate the mass percent of douglasite in a 578.0 mg sample if it took 37.20 mL of a 0.1000 M AgNO3 solution to precipitate all of the Cl- as AgCl. Assume the douglasite is the only source of chloride ion.


First I got mole for AgNO3, which is 0.00372mol.  Then, what I did was I counted number of chlorids in Douglasite, which is 4, and according to that I wrote following equation:   

2 KCl·FeCl2·2H2O + 4AgNO3 --> 4AgCl + ????(we don't really need this part rite?)

then, I did 0.00372 X mole ratio X MM of Douglasite(which is 311.88416)

and I ended up with weird number...  I have no clue with this problem.. can somebody help me??^^ thx

Title: Re: Mass Percent Problem~
Post by: AWK on September 11, 2007, 02:45:07 AM

 Note:
1 mole of douglasite ==> 4 mole of chloride anions
It means mass of pure douglasite is equal to MMxmoles_of_chloride/4
(this mass is in grams!)