1. The problem statement, all variables and given/known data 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 2. Relevant equations Molality= moles solute/kilograms solvent 3. 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.