At 20 °C, an aqueous solution that is 24.0% by mass in ammonium chloride has a density of 1.0674 g mL^-1. What is the molarity of ammonium chloride in the solution? The formula weight of NH₄Cl is 53.50 g mol^-1. A)5.90 B)0.479 C)4.79 D)0.0445 E)22.5

Question

Quizplus · Accepted Answer

First, we need to calculate the mass of ammonium chloride in 100 g of the solution:

Mass of ammonium chloride = 24.0 g/100 g solution = 24.0 g/100 g × 100 mL/1.0674 g = 224.8 g/L

Next, we can calculate the moles of ammonium chloride in the solution using its formula weight:

Moles of NH4Cl = Mass of NH4Cl/Formula weight of NH4Cl = 224.8 g/L / 53.50 g/mol = 4.20 mol/L

Finally, we can express the concentration in terms of molarity:

Molarity = Moles of solute / Volume of solution in liters = 4.20 mol/L

Therefore, the molarity of ammonium chloride in the solution is 4.79 M (rounded to two significant figures). The correct answer is C).

At 20 °C, an Aqueous Solution That Is 24