How many moles of AgCl are contained in 244 mL of 0.135 m AgCl solution? The density of the solution is 1.22 g/mL. A) 4.31 × 10^-2 mol AgCl B) 4.02 × 10^-2 mol AgCl C) 3.29 × 10^-2 mol AgCl D) 2.32 × 10^-2 mol AgCl E) 1.85 × 10^-2 mol AgCl

Question

Quizplus · Accepted Answer

First, we need to calculate the number of moles of AgCl:
moles AgCl = (volume of solution in L) x (molarity of solution)
volume of solution = (mass of solution)/density = (244 mL)(1.22 g/mL) = 297.68 g = 0.29768 L
moles AgCl = (0.29768 L)(0.135 mol/L) = 0.0401828 mol

Therefore, the answer is B, which is 4.02 × 10-2 mol AgCl (in scientific notation with two significant figures).

How Many Moles of AgCl Are Contained in 244 ML