chem question pls help

Question

A solution is prepared by mixing 605.0 mL of ethanol with 582.0 mL of water. The molarity of ethanol in the resulting solution is 9.096 M. The density of ethanol at this temperature is 0.7893 g/mL. Calculate the difference in volume between the total volume of water and ethanol that were mixed to prepare the solution and the actual volume of the solution.

Answer 1

Total volume mixed = 605 + 582 = 1187 ml or 1.187 liters

In order to find Volume of solution, start with amount of ethanol:

605ml eth (.7893 g/ml eth)(1 mole/ 46.07 g eth)( 1 liter of solution/9.096 moles eth) = liters of solution.