Question

1. Which of these aqueous solutions has the highest boiling point? [Kb= 0.512]

(a) 1.25 M C6H12O6 (b) 1.25 M KNO3 (c) 1.25 M Ca(NO3)2 (d) they all have the same boiling point

2. Which of these aqueous solutions has the highest boiling point? [Kb= 0.512]

(a) 1.25 M C6H12O6 (b) 1.25 M KNO3 (c) 1.25 M Ca(NO3)2 (d) they all have the same boiling point

3. A solution contains a mixture of substance A and substance B, both of which are volatile. The mole fraction of substance A is 0.35. At 32°C the vapor pressure of pure A is 87 mm Hg and the vapor pressure of pure B is 122 mmHg. What is the total vapor pressure of the solution at this temperature?
(a) 110 mmHg (b) 209 mmHg (c) 99.3 mmHg (d) 73.2 mmHg

4. To equalize the pressure

(a) solvent moves from a low concentration to a higher concentration

(b) solvent moves from a high concentration to a lower concentration

(c) solute moves from a low concentration to a higher concentration

(d) solute moves from a higher concentration to a lower concentration.

5. What is the molality of a solution produced by dissolving 14.40 g of LiCl (42.39 g/n) in water to make 0.104 L of solution with a density of 1.102 g/mL?
(a) 0.340m (b)3.39m (c)3.27m (d)3.74m (e)2.96m

6. A 0.86% by mass solution of NaCl is called “physiological saline” because its osmotic pressure is equal to that of the solution in blood cells. Calculate the osmotic pressure of this solution at normal body temperature (37°C). Note that the density of “physiological saline” solution is 1.005 g/mL.
[R = 0.0821 L.atm/n.K; MM of NaCl = 58.45]

7. Determine the vapor pressure of an aqueous ethylene glycol (C2H6O2) solution that is 17.2% C2H6O2 by mass. The vapor pressure of pure water at 25°C is 23.8 torr.

Answer 1

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