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Chapter 11: Q11.2-10E (page 646)
Explain why solutions of HBr in benzene (a nonpolar solvent) are nonconductive, while solutions in water (a polar solvent) are conductive.
Conductive means to produce electricity
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A 12.0-g sample of a nonelectrolyte is dissolved in 80.0 g of water. The solution freezes at 鈭�1.94 掳C. Calculate the molar mass of the substance. The Vapour Pressure of the Solution is 23.35 Tor.
Question: The vapor pressure of methanol, \({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH}}\) , is 94 tor at 20 掳C. The vapor pressure of ethanol,\({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH}}\) , is 44 tor at the same temperature.
(a) Calculate the mole fraction of methanol and of ethanol in a solution of 50.0 g of methanol and 50.0 g of ethanol.
(b) Ethanol and methanol form a solution that behaves like an ideal solution. Calculate the vapor pressure of methanol and of ethanol above the solution at 20 掳C.
(c) Calculate the mole fraction of methanol and of ethanol in the vapor above the solution.
The triple point of air-free water is defined as 273.15 K. Why is it important that the water be free of air?
Which of the following gases is expected to be most soluble in water? Explain your reasoning.
(a) \({\bf{CH}}_4\)
(b) \({\bf{CCl}}_4\)
(c)\({\bf{CHCl}}_3\)
How do colloids differ from solutions with regard to dispersed particle size and homogeneity?
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