Concept explainers
(a)
Interpretation:
Which of the given aqueous solution has higher boiling point, higher freezing point and the lower vapor pressure have to be explained.
Concept introduction
Boiling point is the temperature at which liquid turns into a gas. Example: boiling point of water i
Where,
Boiling point elevation
Where,
m- molality of the solution
Freezing point is the temperature at which liquid turns into solid.
Freezing point depression
Where,
m- Molality of the solution
Vapor pressure is the pressure excreted by the molecules at the surface of the liquid in the closed container.
(a)
Answer to Problem 12.69QP
Explanation of Solution
Explanation of
(b)
Interpretation:
Which of the given aqueous solution has higher boiling point, higher freezing point and the lower vapor pressure have to be explained.
Concept introduction
Boiling point is the temperature at which liquid turns into a gas. Example: boiling point of water is
Where,
Boiling point elevation
Where,
m- molality of the solution
Freezing point is the temperature at which liquid turns into solid.
Freezing point depression
Where,
m- Molality of the solution
Vapor pressure is the pressure excreted by the molecules at the surface of the liquid in the closed container.
(b)
Answer to Problem 12.69QP
Explanation of Solution
Explanation of Urea has higher freezing point depression than
Freezing point depends on the molality and van’t Hoff factor of the solute. In this case,
(c)
Interpretation:
Which of the given aqueous solution has higher boiling point, higher freezing point and the lower vapor pressure have to be explained.
Concept introduction
Boiling point is the temperature at which liquid turns into a gas. Example: boiling point of water is
Where,
Boiling point elevation
Where,
m- molality of the solution
Freezing point is the temperature at which liquid turns into solid.
Freezing point depression
Where,
m- Molality of the solution
Vapor pressure is the pressure excreted by the molecules at the surface of the liquid in the closed container.
(c)
Answer to Problem 12.69QP
Explanation of Solution
Explanation of
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Chapter 12 Solutions
CHEMISTRY STUD.SOL.MANUAL >C<
- Urea, (NH2)2CO, has been used to melt ice from sidewalks, because the use of salt is harmful to plants. If the saturated aqueous solution contains 41% urea by mass, what is the freezing point? (The answer will be approximate, because the equation in the text applies accurately only to dilute solutions.)arrow_forwardThe freezing-point depression of a 0.091-m solution of CsCl is 0.320C. The freezing-point depression of a 0.091-m solution of CaCl2 is 0.440C. In which solution does ion association appear to be greater? Explain.arrow_forwardThe carbohydrate digitoxose contains 48.64% carbon and 8.16% hydrogen. The addition of 18.0 g of this compound to 100 g of water gives a solution that has a freezing point of 2.2C. a What is the molecular formula of the compound? b What is the molar mass of this compound to the nearest tenth of a gram?arrow_forward
- A 1.00 mol/kg aqueous sulfuric acid solution, H2SO4,freezes at 4.04 C. Calculate i, the vant Hoff factor,for sulfuric acid in this solution.arrow_forwardThe freezing point of a 0.031-m solution of copper(II) sulfate in water is 0.075 C. (a) Calculate the vant Hoff factor, i, for this solution. (b) Would the vant Hoff factor be larger, smaller, or the same for a 0.050-m solution of this compound?arrow_forward
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