Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: zerofantasym on February 09, 2008, 11:31:51 AM
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What would be the vapor pressure of water at 70 C above a solution made by dissolving 57.980 g of Nickel nitrate Ni(NO3)2 in 288.26 g of water? The vapor pressure of pure water at this temperature is 233.70 mmHg? Assume complete dissociation of solute.
I got 233.68 mmHg. Is this right?
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No, it should be lower.
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hmm ok well this is actually an online homework and I don't know, maybe I'm not entering the answer in correctly. I tried it twice again and got 229.17 mmHg but it's still not correct apparently. What's wrong here?
mol fraction of Ni(NO3)2 = .0194
using Raoult's Law: PA = PA°XA
∆P = 233.70 mmHg x .0194 = 4.534 mmHg
PA = 233.70 - 4.534 = 229.17 mmHg
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mol fraction of Ni(NO3O)2 = .0194
Isn't it dissociated?
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It's what?
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Uh I copied it here wrong. I did it right on the paper though.