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

Question

Quizplus · Accepted Answer

To find the molarity of ammonium chloride in the solution, we need to first calculate the mass of ammonium chloride present in 1 liter of the solution.

Let's assume we have 100g of the solution, which means that we have 24g of ammonium chloride and 76g of water.

Using the density of the solution, we can calculate the volume of 100g of the solution:

density = mass/volume

1.0674 g/mL = 100g/volume

volume = 93.7 mL = 0.0937 L

Now, we can use the mass of ammonium chloride and its formula weight to calculate the number of moles present in the solution:

moles of NH4Cl = mass of NH4Cl / formula weight of NH4Cl

moles of NH4Cl = 24g / 53.50 g/mol

moles of NH4Cl = 0.449 mol

Finally, we can calculate the molarity of the solution:

Molarity = moles of solute / volume of solution in liters

Molarity = 0.449 mol / 0.0937 L

Molarity = 4.79 M

Therefore, the answer is C) 4.79.

At 20°C, an Aqueous Solution That Is 24