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

molar mass sucrose = 342.3 g/mol

$\mathbf{moles}\mathbf{}\mathbf{sucrose}\mathbf{=}\mathbf{35}\mathbf{.}\mathbf{0}\mathbf{}\overline{)\mathbf{g}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\mathbf{mol}}{\mathbf{342}\mathbf{.}\mathbf{3}\mathbf{}\overline{)\mathbf{g}}}$

You may want to reference (Pages 145 - 148) Section 4.5 while completing this problem.

You make 1.000 L of an aqueous solution that contains 35.0 g of sucrose (C_{12}H_{22}O_{11}). What is the molarity of sucrose in this solution?

Express your answer to three significant figures

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