$\overline{)\mathbf{Molarity}\mathbf{}\mathbf{\text{(M)}}\mathbf{}\mathbf{=}\mathbf{}\frac{\mathbf{mol}\mathbf{}\mathbf{solute}}{\mathbf{L}\mathbf{}\mathbf{solution}}}$

**Step 1:** Calculate moles KMnO_{4}

molar mass KMnO_{4} = 158.034 g/mol

$\mathbf{moles}\mathbf{}{\mathbf{KMnO}}_{\mathbf{4}}\mathbf{=}\mathbf{0}\mathbf{.}\mathbf{0908}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{KMnO}}_{\mathbf{4}}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{KMnO}}_{\mathbf{4}}}{\mathbf{158}\mathbf{.}\mathbf{034}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{KMnO}}_{\mathbf{4}}}}$

moles KMnO_{4} = 5.7456×10^{‒4} mol KMnO_{4}

**Step 2:** Calculate molarity

Consider this question: What is the molarity of KMnO_{4} in a solution of 0.0908 g of KMnO_{4} in 0.500 L of solution? (a) Outline the steps necessary to answer the question. (b) Answer the question.

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