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Problem 22

Calculate each of the following: (a) Mass fraction of $\mathrm{C}$ in cesium acetate (b) Mass fraction of $\mathrm{O}$ in uranyl sulfate trihydrate (the uranyl ion is $\mathrm{UO}_{2}^{2+} )$

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Uranium can be isolated from its ores by dissolving it as UO $_{2}\left(\mathrm{NO}_{3}\right)_{2},$ then separating it as solid

$\mathrm{UO}_{2}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right) \cdot 3 \mathrm{H}_{2} \mathrm{O}$ . Addition of 0.4031 $\mathrm{g}$ of sodium oxalate, $\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4},$ to a soluting 1.481 $\mathrm{g}$ of uranyl nitrate, $\mathrm{UO}_{2}\left(\mathrm{NO}_{3}\right)_{2},$ yields 1.073 $\mathrm{g}$ of solid $\mathrm{UO}_{2}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right) \cdot 3 \mathrm{H}_{2} \mathrm{O}$ $\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}+\mathrm{UO}_{2}\left(\mathrm{NO}_{3}\right)_{2}+3 \mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{UO}_{2}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right) \cdot 3 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{NaNO}_{3}$

Determine the limiting reactant and the percent yield of this reaction.

A solution is made containing 14.6 $\mathrm{g}$ of $\mathrm{CH}_{3} \mathrm{OH}$ in 184 $\mathrm{g}$ of $\mathrm{H}_{2} \mathrm{O} .$ Calculate (a) the mole fraction of $\mathrm{CH}_{3} \mathrm{OH},$ (b) the mass percent of $\mathrm{CH}_{3} \mathrm{OH},(\mathbf{c})$ the molality of $\mathrm{CH}_{3} \mathrm{OH}$ .

A solution is prepared by dissolving 52.3 g cesium chloride in 60.0 g water. The volume of the solution is 63.3 $\mathrm{mL}$ . Calculate the mass percent, molarity, molality, and mole fraction of the CsCl solution.

An aqueous antifreeze solution is 40.0$\%$ ethylene glycol $\left(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}\right)$ by mass. The density of the solution is 1.05 $\mathrm{g} / \mathrm{cm}^{3}$ . Calculate the molality, molarity, and mole fraction of the ethylene glycol.