An aqueous solution of a compound with a molar mass of 34.02 g/mol is 25.5% by mass and has a density of 1.19 g/cm³. What is the molarity of the solution? A) 8.92 M B) 7.50 M C) 1.37 M D) 0.000892 M E) 6.30 M

Question

Quizplus · Accepted Answer

To calculate the molarity of the solution, we first need to find the mass of the solute present in the solution.

Let's assume we have 100 g of the solution, which means 25.5 g of the solution is the solute, and the rest is water.

Now, we need to find the moles of the solute present in the solution.

Moles = Mass/Molar mass = 25.5 g/34.02 g/mol = 0.75 mol

The volume of the solution can be calculated as:

Volume = Mass/Density = 100 g/1.19 g/cm³ = 84.03 cm³

Now, we can calculate the molarity of the solution as:

Molarity = Moles/Volume (in liters) = 0.75 mol/0.08403 L = 8.92 M

Therefore, the answer is A) 8.92 M.

An Aqueous Solution of a Compound with a Molar Mass