🤓 Based on our data, we think this question is relevant for Professor Halasyamani's class at UH.

We’re being asked to **calculate the molarity (M)** of **an aqueous solution that is 22.3% by mass calcium chloride**. Recall that ** molarity** is the ratio of the moles of solute and the volume of solution (in liters). In other words:

$\overline{){\mathbf{molarity}}{\mathbf{}}{\mathbf{\left(}}{\mathbf{M}}{\mathbf{\right)}}{\mathbf{=}}\frac{\mathbf{moles}\mathbf{}\mathbf{solute}}{\mathbf{L}\mathbf{}\mathbf{solution}}}$

We first need to determine the number of moles of** calcium chloride (CaCl _{2})**. We’re given the mass percent of calcium chloride in the solution water,

$\overline{){\mathbf{\%}}{\mathbf{}}{\mathbf{Mass}}{\mathbf{=}}\frac{\mathbf{mass}\mathbf{}\mathbf{of}\mathbf{}{\mathbf{CaCl}}_{\mathbf{2}}}{\mathbf{mass}\mathbf{}\mathbf{of}\mathbf{}\mathbf{solution}}}$

Calculate the molarity of an aqueous solution that is 22.3% by mass calcium chloride. You might need to know that the density is 1.20 g/mL.

A. 0.96

B. 2.41

C. 0.0024

D. 3.54

E. 0.035

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Based on our data, we think this problem is relevant for Professor Halasyamani's class at UH.