At 20°C, an aqueous solution that is 24.00% 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) 22.5 B) 4.79 C) 0.479 D) 5.90 E) 0.0445

Question

Quizplus · Accepted Answer

First, we need to calculate the mass of ammonium chloride in 100 g of solution:
Mass of ammonium chloride = 24.00 g/100 g of solution * 100 g = 24.00 g

Next, we can use the density to calculate the volume of the solution:
Density = mass/volume
Volume = mass/density = 24.00 g/1.0674 g/mL = 22.47 mL

Now we can calculate the number of moles of ammonium chloride:
moles = mass/fm
fm = 53.50 g/mol
moles = 24.00 g/53.50 g/mol = 0.4486 mol

Finally, we can use the volume to calculate the molarity:
Molarity = moles/volume = 0.4486 mol/0.02247 L = 19.95 M

We should note that this is a very concentrated solution, and it is unlikely that ammonium chloride could dissolve to such a high concentration without heating or using a concentrated solution. However, given the information provided in the question, B is the best choice.

At 20°C, an Aqueous Solution That Is 24