At 20 °C, an aqueous solution that is 12.0% by mass in ammonium chloride has a density of 1.0344 g/mL. What is the molarity of ammonium chloride in the solution? The formula weight of NH₄Cl is 53.50 g/mol. A)2.55 B)0.232 C)2.32 D)0.0862 E)11.6

Question

Quizplus · Accepted Answer

First, we need to calculate the mass of ammonium chloride in 100 grams of solution:
mass of NH4Cl = 12.0 g/100 g solution x 100 g solution = 12.0 g

Next, we can use the density to calculate the volume of 12.0 g of solution:
volume of solution = mass of solution/density = 12.0 g/1.0344 g/mL = 11.59 mL

Now, we can use the formula weight and the mass of ammonium chloride to calculate the number of moles:
moles of NH4Cl = mass of NH4Cl/formula weight of NH4Cl = 12.0 g/53.50 g/mol = 0.224 mol

Finally, we can use the volume of solution to calculate the molarity:
molarity = moles of solute (NH4Cl)/volume of solution (L) x 1000 mL/L = 0.224 mol/ 11.59 mL x 1 L/1000 mL = 2.32 M

Therefore, the answer is C) 2.32.

At 20 °C, an Aqueous Solution That Is 12