At 20 °C,an aqueous solution that is 24.0% by mass in ammonium chloride has a density of 1.0674 $\mathrm { g } \mathrm { mL } ^ { - 1 }$ What is the molarity of ammonium chloride in the solution? The formula weight of $\mathrm { NH } _ { 4 }$ Cl is $53.50 \mathrm {~g} \mathrm {~mol} ^ { - 1 }$ A)0.209 mol L^-1 B)0.0445 mol L^-1 C)22.5 mol L^-1 D)0.479 mol L^-1 E)4.79 mol L^-1

Question

Quizplus · Accepted Answer

To find the molarity, first calculate the mass of the solution in 1 liter using the density: 1.0674 g/mL * 1000 mL = 1067.4 g. Then, find the mass of NH4Cl in this solution: 24% of 1067.4 g = 256.176 g. Convert this mass to moles: 256.176 g / 53.50 g/mol = 4.79 mol. Therefore, the molarity is 4.79 mol/L.

At 20 °C,an Aqueous Solution That Is 24 gmL−1\mathrm { g } \mathrm { mL } ^ { - 1 }gmL−1

At 20 °C,an Aqueous Solution That Is 24 $\mathrm { g } \mathrm { mL } ^ { - 1 }$