One gram of caffeine dissolves in 55 ml of water, 7 ml of dichloromethane (DCM), 530 ml of diethyl ether, and 100 ml of benzene. Covert the solubility of caffeine in these four solvents into units of mg/ml. Which is the optimal solvent to extract caffeine from an aqueous solution? Why?
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Given: 1 g of caffeine in 55 ml of water. Convert 1 g to mg: 1 g = 1000 mg. Calculate solubility: 1000 mg / 55 ml = 18.18 mg/ml. ** Show more…
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Consider a 0.015 L aqueous solution that contains 1.4 g of caffeine. The solubility of caffeine in water is 2.2 g/100 mL and the solubility in methylene chloride is 10.2 g/100 mL. a) How much caffeine can be extracted with 15 mL of methylene chloride? b) How much caffeine will be extracted if the aqueous solution is extracted twice with 7.5 mL of methylene chloride? Which is more effective, a or b?
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Questions: Based on what happened in this experiment, is caffeine more soluble in water or more soluble in dichloromethane? Explain your reasoning. Methanol is miscible with water. Assuming that caffeine is soluble in methanol, could you use methanol as a solvent to extract caffeine from tea (rather than using dichloromethane as the extraction solvent)? Explain why or why not. Go through the procedure thoroughly and list all the places where you definitely lost caffeine.
The solubility of benzoic acid, is 0.34 $\mathrm{g} / 100 \mathrm{mL}$ in water at $25^{\circ} \mathrm{C}$ and 10.0 $\mathrm{g} / 100 \mathrm{mL}$ in benzene $\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)$ at $25^{\circ} \mathrm{C} .$ Rationalize this solubility behavior. For a $1.0-\mathrm{m}$ solution of benzoic acid in benzene, would the measured freezing point depression be equal to, greater than, or less than $5.12^{\circ} \mathrm{C} ?\left(K_{\mathrm{f}}=5.12^{\circ} \mathrm{C} \cdot \mathrm{kg} / \mathrm{mol} \text { for benzene.) }\right.$
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