Evaluate the approximate freezing point of a solution

Reference no: EM13519807

1. If 26.4 g of nickel(II) bromide are dissolved in 224 g of water, what will be the freezing point of the resulting solution? Assume 100% dissociation and no interaction between ions.

2. How much glycol (1,2-ethandiol), C2H6O2, must be added to 1.00 L of water so the solution does not freeze above -20.0°C?

3. Calculate the approximate freezing point of a solution prepared by dissolving 10.0 g of naphthalene (C10H8) in 300. g of cyclohexane. Pure cyclohexane freezes at 6.6°C. Kf of cyclohexane = 20.0°C/m.

4. The freezing point of a solution that contains 1.00 g of an unknown compound, (A), dissolved in 10.0 g of benzene is found to be 2.07°C. The freezing point of pure benzene is 5.48°C. The molal freezing point depression constant of benzene is 5.12°C/molal. What is the molar mass of the unknown compound?

5. What is the molality of a solution composed of 38.0 g of cane sugar (C12H22O11) dissolved in 175 g of water?

Reference no: EM13519807

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