$\overline{)\mathbf{molarity}\mathbf{}\mathbf{\text{(M)}}\mathbf{=}\frac{\mathbf{mol}}{\mathbf{L}}}$

(1) prepared by dissolving 21.0 g of NaF (0.500 mol) in enough water to make 500 mL

$\mathbf{molarity}\mathbf{=}\frac{\mathbf{0}\mathbf{.}\mathbf{500}\mathbf{}\mathbf{mol}\mathbf{}\mathbf{NaF}}{\mathbf{500}\mathbf{}\overline{)\mathbf{mL}}\mathbf{\times}{\displaystyle \frac{{\mathbf{10}}^{\mathbf{-}\mathbf{3}}\mathbf{}\mathbf{L}}{\mathbf{1}\mathbf{}\overline{)\mathbf{mL}}}}}\phantom{\rule{0ex}{0ex}}\mathbf{molarity}\mathbf{=}\frac{\mathbf{0}\mathbf{.}\mathbf{500}\mathbf{}\mathbf{mol}\mathbf{}\mathbf{NaF}}{\mathbf{0}\mathbf{.}\mathbf{500}\mathbf{}\mathbf{L}}\phantom{\rule{0ex}{0ex}}\mathbf{molarity}\mathbf{=}\mathbf{1}\mathbf{.}\mathbf{00}\frac{\mathbf{moL}\mathbf{}\mathbf{NaF}}{\mathbf{L}}$

Which is more concentrated, a solution (1) prepared by dissolving 21.0 g of NaF (0.500 mol) in enough water to make 500 mL of solution or a solution (2) prepared by dissolving 10.5 g (0.250 mol) of NaF in enough water to make 100 mL of solution?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Molarity concept. You can view video lessons to learn Molarity. Or if you need more Molarity practice, you can also practice Molarity practice problems.

What professor is this problem relevant for?

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