The freezing point of a solution that contains 1.1 g of an unknown compound, (A), dissolved in 12 g of benzene is found to be 2.97 °C. The freezing point of pure benzene is 5.48 °C. The freezing point depression constant of benzene is 5.12 °C/molal. What is the molecular weight of the unknown compound?

A chemist is studying the properties of a small organic compound. One of the properties under study is the effect on osmotic pressure. (A) When 0.517 g of the compound are dissolved in enough water to make a total volume of 50.0 mL, the resulting solution has an osmotic pressure of 4.18 atm at 23.0°C. What is the molar mass of the organic compound? Assume the compound does not dissociate in water and is nonvolatile. (B) Analysis shows that the compound is 59.96% C, 13.42% H, and the rest O by mass. Determine the empirical formula of the compound. (Hint: See Chapter 4.) (C) Draw two potential Lewis structures for the compound based on the formula from (B). One of the Lewis structures should be able to form H-bonds, while the other should not. Clearly identify which structure is which.

A certain liquid X has a normal freezing point of -4.00 °C and a freezing point depression constant K = 6.25 °C-kg-mol some iron(III) chloride (FeCl3) in 600. g of X. This solution freezes at -5.2 °C. Calculate the mass of FeCl3 that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. g . A solution is prepared by dissolv 0 || cue X

Identify the following statements about the principles of solubility. Each statement refers to the solubility of the solute mentioned.     Increasing the temperature of a solution of a salt that has an enthalpy of solution of 0.0 kJ/mol.     Increasing the overall pressure on a solution of NaCl dissolved in water.     Reducing the partial pressure of nitrogen gas over a solution of nitrogen dissolved in hexane.     Changing the solvent for a solution of C5H12 from methanol (CH3OH) to pentanol (C5H11OH).     Changing the solvent for a solution of CH3OH from pentanol(C5H11OH) to ethanol(C2H5OH)     Increasing the temperature of a solution of KOH dissolved in water. This salt has an exothermic enthalpy of solution.     Raising the partial pressure of CO2 gas on a solution of CO2 dissolved in water.