A 9.50 % by mass solution of acetone (C₃H₆O) in water has a density of 0.9849 g/mL at 20^$\circ$C. What is the molarity of this solution A) 0.621 M B) 1.61 M C) 1.66 M D) 1.71 M E) 16.9 M

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To find the molarity of the solution, we first need to calculate the mass of acetone and water in a given volume of solution, then convert the mass of acetone to moles, and finally divide by the volume of the solution in liters.Given:- 9.50% by mass solution of acetone means 9.50 g of acetone in 100 g of solution.- The density of the solution is 0.9849 g/mL, which means 1 mL of the solution weighs 0.9849 g.Steps:1. Calculate the mass of the solution that contains 1 mole of acetone:   Acetone's molar mass = 12(3) + 1(6) + 16 = 58 g/mol.   2. For 100 g of solution, the mass of acetone is 9.50 g. So, the mass of water is 100 g - 9.50 g = 90.5 g.3. To find the volume of this solution, we use the density:   Volume = mass / density = 100 g / 0.9849 g/mL = 101.53 mL = 0.10153 L.4. The moles of acetone in 9.50 g:   Moles = mass / molar mass = 9.50 g / 58 g/mol = 0.1638 mol.5. Finally, the molarity (M) is moles of solute per liter of solution:   Molarity = moles / volume = 0.1638 mol / 0.10153 L ≈ 1.61 M.

A 950 % by Mass Solution of Acetone (C3H6O) in Water

A 950 % by Mass Solution of Acetone (C₃H₆O) in Water