The solvent is water. Pure water has a freezing point of 0 degrees Celsius. How come, in this problem, the addition of solute results in an elevation of the freezing point from 0 to 0.46 degrees C? Is this possible? Or is this question just flawed?
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1If you'd see "Buffalo" written on an elephant's cage in a zoo, would you suspect a mistake, or suppose that you didn't know something? – Ivan Neretin Feb 24 '17 at 15:27
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1I would assume that this is supposed to be $-0.46\ ^{\circ}\mathrm{C}$... – Zhe Feb 24 '17 at 16:06
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My thought as well. – Ivan Neretin Feb 24 '17 at 16:07
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Adding deuterium oxide would raise the freezing point. – MaxW Feb 24 '17 at 16:47
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I see no problem here. It's not a salt and it doesn't lower melting point but on contrary... – Mithoron Feb 24 '17 at 16:48
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Truthfully it is very unlikely, but possible. – MaxW Feb 24 '17 at 16:51
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Ha, found it! http://chemistry.stackexchange.com/questions/57686/are-melting-points-for-mixtures-of-solids-always-below-the-melting-points-of-the – Mithoron Feb 24 '17 at 17:30
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The solute does not need to be ionic but just be involatile relative to the solvent. – porphyrin Feb 24 '17 at 22:37