At 20 °C,a 0.389 mol L^-1 aqueous solution of ammonium chloride has a density of 1.0064 $\mathrm { g } \mathrm { mL } ^ { - 1 }$ What is the mass % of ammonium chloride in the solution? The formula weight of $\mathrm { NH } _ { 4 }$ Cl is $53.50 \mathrm {~g} \mathrm {~mol} ^ { - 1 }$

Question

Quizplus · Accepted Answer

To find the mass %, calculate the mass of NH4Cl in 1 L of solution: 0.389 mol/L * 53.50 g/mol = 20.8155 g. The mass of 1 L of solution is 1006.4 g (since density is 1.0064 g/mL). Mass % = (20.8155 g / 1006.4 g) * 100% = 2.07%.

At 20 °C,a 0 gmL−1\mathrm { g } \mathrm { mL } ^ { - 1 }gmL−1

At 20 °C,a 0 $\mathrm { g } \mathrm { mL } ^ { - 1 }$