We’re being asked to **calculate the mass of potassium chloride, KCl**** **in a **100.0 mL of a 2.0 M KCl solution**.

Recall that ** molarity** is the ratio of the moles of solute and the volume of solution (in liters).

In other words:

$\overline{){\mathbf{Molarity}}{\mathbf{\left(}}{\mathbf{M}}{\mathbf{\right)}}{\mathbf{=}}\frac{\mathbf{moles}\mathbf{}\mathbf{of}\mathbf{}\mathbf{solute}}{\mathbf{Liters}\mathbf{}\mathbf{of}\mathbf{}\mathbf{solution}}}$

How many mass of potassium chloride, KCl, are needed to make 100.0 mL of a 2.0 M KCl solution?

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