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221. A 0.1539 molal aqueous solution of cane sugar (mol. mass = 342 g mol^–1) has a freezing point of 271 K while the freezing point of pure water is 273.15 K. What will be the freezing point of an aqueous solution containing 5 g of gluocose (mol. mass = 180 g mol^–1) per 100 g of solution?

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222.

An aqueous solution of 2 percent non-volatile solute exerts a pressure of 0.096 atm at the boiling poine of the solvent. What is the molecular mass of the solute ?

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223. The vapour pressure of water is 12.3 kPa at 300 K. Calculate the vapour pressure of a one molal solution of a non-volatile, non-ionic solute in water.

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224. Why is the vapour pressure of a solution of glucose in water lower than that of water?

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225. A 6.90 M solution of KOH in water contains 30% by mass of KOH. Calculate the density of the KOH solution. [Molar mass of KOH = 56 g mol^–1]

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226. Give reasons for the following:
When 30 ml of ethyl alcohol and 30 ml of water are mixed, the volume of resulting solution is more than 60 ml.

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227. Give reasons for the following:
Copper is conducting as such while copper sulphate is conducting only in molten state or in aqueous solution.

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228. Urea forms an ideal solution in water. Determine the vapour pressure of an aqueous solution containing 10% by mass of urea at 40⁰C. (Vapour pressure of water at 40⁰C = 55.3 mm of Hg)

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229. Why is freezing point depression of 0.1 M sodium chloride solution nearly twice that of 0.1 M glucose solution?

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230. A 6.90 M solution of KOH in water contains 30% by mass of KOH. Calculate the density of the KOH solution. (Molar mass of KOH = 56 g mol^–1)

Answer;

Let the mass of solution =100g

x_KOH = 30/56

volumeof solution = $\frac{mass of solution}{density of solution}$

$= \frac{100 g}{d g / {cm}^{3}} = \frac{100}{d} cm \times \frac{1}{1000} = \frac{1}{10 d} L Molarity = \frac{number of moles of solute}{volume of solution} 6.90 = \frac{30 / 56}{1 / 10 d} 6.90 = \frac{30}{56} \times \frac{10 d}{1} d = 1.288 g / cm$

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230. A 6.90 M solution of KOH in water contains 30% by mass of KOH. Calculate the density of the KOH solution. (Molar mass of KOH = 56 g mol–1)

230. A 6.90 M solution of KOH in water contains 30% by mass of KOH. Calculate the density of the KOH solution. (Molar mass of KOH = 56 g mol^–1)