Osmotic Pressure & Mass Percent

[kuahji]

[SOLVED] Osmotic Pressure & Mass Percent

A solid mixture of KCL, KNO3, and Ba(NO3)2 is 20.92 mass percent chlorine, and a 1.000g sample of the mixture in 500.0 mL of aqueous solution at 25 C has an osmotic pressure of 744.7 mm Hg. What are the mass percents of KCl, KNO3, and Ba(NO3)2 in the mixture?

First I started out using osmotic pressure equation after I converted 744.7 mm Hg to atm.

.9799atm=7x(.08206 L*atm*K^{-1}*mol^{-1})(298K)

x=.0057 mol of ions/liter (I chose 7x because it appears there would be 7 ions, assuming they'd all dissociate completely)

Here however is where I'm stuck already. Any advice on where to go from here?

 

[chemisttree]

A solid mixture of KCL, KNO3, and Ba(NO3)2 is 20.92 mass percent chlorine, and a 1.000g sample of the mixture in 500.0 mL of aqueous solution at 25 C has an osmotic pressure of 744.7 mm Hg. What are the mass percents of KCl, KNO3, and Ba(NO3)2 in the mixture?

First I started out using osmotic pressure equation after I converted 744.7 mm Hg to atm.

.9799atm=7x(.08206 L*atm*K^{-1}*mol^{-1})(298K)

x=.0057 mol of ions/liter (I chose 7x because it appears there would be 7 ions, assuming they'd all dissociate completely)

Here however is where I'm stuck already. Any advice on where to go from here?

From here determine how many moles of ions are in half a liter.

 

[kuahji]

I was able to figure it out from here, though it wasn't pretty. I ended up having to make two equations with two different variables. Thanks.