Does this problem require knowing the density of water?

[JeweliaHeart]

Homework Statement

What is the molality of an aqueous solution of a compound with a molar mass of 120. g/mol that has a density of 1.56 g/mL and a molarity of 5.78 M?

(A) 6.67 m
(B) 5.78 m
(C) 120. m
(D) 1.56 m
(E) None of the Above

Homework Equations

Molality= moles solute/kilograms solvent

The Attempt at a Solution

I assumed a volume of 1 L of solution, leaving me with 5.78 moles solute.

5.78 moles solute x 120 g/mole solute = 693.6 g solute

693.6 g solute x 1 mL/ 1.56 g solute =444.615 mL (the space taken up by the solute)

1000 ml(b/c I assumed 1 L solution)- 444.615= 555.385 ml (volume of solvent, water)

I don't know where to go from here b/c I don't know what the density of water is at whatever temperature the solution is at.

 

[Borek]

I believe you are misreading the question. 1.56 g/mL is density of the solution, not of the solute. If so, what is mass of the 1L of the solution? How much of this mass is water?

If 1.56 g/mL is intended to be density of the solute, there is not enough information to solve the problem.

 

[JeweliaHeart]

Thanks so much Borek.

Yes, I was misreading the problem. I tried solving it again using 1.56 g/mL as the density of the entire solution and I got the right answer, which is a) 6.67 molality.

I got to start reading these problems more carefully.

 

[Borek]

I am not surprised you misread the problem, it is lousy worded and confusing. For me it was obvious as I have seen zillions of such questions.