An aqueous solution of #H_2SO_4# (molecular weight=98) contains 10.78 #g# of acid per #dm^3# of solution. Density of solution is 1.123 #g#/#ml#. What is the molarity, molality, normality and mole fraction of the solution?
Here's how you can solve this problem.
The problem actually makes your life easier by telling you that you have that much sulfuric acid, 10.78 g to be precise, per
If you take into account that fact that
To do that, use the acid's moalr mass
This means that the solution's molarity is
This means that the mass of water will be
This molality of the solution will thus be
The solution's normality will take into account the number of protons the sulfuric acid will produce in solution.
Since sulfuric acid is a diprotic acid, every mole of the acid will produce two moles of
Since you have 0.11 moles, you'll get twice as many equivalents.
This means that the solution's normality will be twice as big as its molarity.
To get the mole fraction of the solution, you need to first determine how many moles of water you have.
The total number of moles will be
The mole fraction of sulfuric acid will thus be