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

Question

Quizplus · Accepted Answer

First, we need to find the mass of ammonium chloride in 1 L of the solution:

Density = mass/volume
1.0674 g/mL = mass/1000 mL
mass = 1067.4 g

The mass of ammonium chloride in the solution is:

24.0 g NH4Cl/100 g solution x 1067.4 g solution = 256.18 g NH4Cl

The number of moles of NH4Cl is:

256.18 g NH4Cl x (1 mol NH4Cl/53.50 g NH4Cl) = 4.79 mol NH4Cl

Finally, we find the molarity of the solution:

Molarity = moles of solute/liters of solution
Molarity = 4.79 mol NH4Cl/1 L solution = 4.79 M

Therefore, the answer is C (4.79 M).

At 20°C,an Aqueous Solution That Is 24