What is the molality of a solution that contains 63.0 g #HNC_3# in 0.500 kg #H_2O#?

1 Answer
anor277
May 11, 2017

What do you mean by #HNC_3#, do you mean #H_2NCH_3#, i.e. #"methylamine"#?

Explanation:

If you mean #"methylamine"#, then the molality of the solution is given by:

#"Moles of solute"/"Kilograms of solvent"=((63.0*g)/(31.06*g*mol^-1))/(0.500*kg)=4.06*mol*kg^-1#.

I would not want to be downwind of such a solution. It would smell VILE! If you mean a different solute, you must specify the unambiguous chemical formula. The molarity of the solution would not be significantly different.

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