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Concept explainers
Equal numbers of moles of two soluble, substances, substance A and substance B, are placed into separate 1.0-L samples of water.
- a The water samples are cooled. Sample A freezes at −0.50°C, and Sample B freezes at −l.00°C. Explain how the solutions can have different freezing points.
- b You pour 500 mL of the solution containing substance B into a different beaker. How would the freezing point of this 500-mL portion of solution B compare to the freezing point of the 1.0-L sample of solution A?
- c Calculate the molality of the solutions of A and B. Assume that i = 1 for substance A.
- d If you were to add an additional 1.0 kg of water to solution B, what would be the new freezing point of the solution? Try to write an answer to this question without using a mathematical formula.
- e What concentration (molality) of substances A and B would result in both solutions having a freezing point of −0.25°C?
- f Compare the boiling points, vapor pressure, and osmotic pressure of the original solutions of A and B. Don’t perform the calculations; just state which is the greater in each ease.
(a)
![Check Mark](/static/check-mark.png)
Interpretation:
A and B are two substances having equal number of moles. They are placed into separate
Concept Introduction:
Freezing point of the substance is temperature at which liquid substance remains in equilibrium with solid substance.
Depression in freezing point of a substance can be determined by the formula,
Where,
Explanation of Solution
While dissolving in solvent the solute particles don't dissolve in same way always. This is why, even though the two sample solutions A and B are made of same type of solute and have equal number of moles has different freezing point.
(b)
![Check Mark](/static/check-mark.png)
Interpretation:
A and B are two substances having equal number of moles. They are placed into separate
Concept Introduction:
Freezing point of the substance is temperature at which liquid substance remains in equilibrium with solid substance.
Depression in freezing point of a substance can be determined by the formula,
Where,
Explanation of Solution
Freezing point of a solution is a colligative property which depends only on the concentration of the solute. Thus dividing the volume of solution of same concentration doesn't result in variation of freezing point. So there will be no change in difference between the boiling point of
Two different solutions made of same solute with same number of moles can have different freezing points. Freezing point of a solution doesn’t vary with volume and it varies only with concentration of the solute in the solution.
(c)
![Check Mark](/static/check-mark.png)
Interpretation:
A and B are two substances having equal number of moles. They are placed into separate
Molality of the solutions A and B has to be calculated by assuming
Concept Introduction:
Molality is one of the many parameters that is used to express concentration of a solution. It is expressed as,
Depression in freezing point of a substance can also be used to determine molality of the solution by rewriting the formula,
Answer to Problem 12.26QP
Molality of the solutions A and B are calculated to be
Explanation of Solution
Both the solutions A and B have same molality as both of them have same number of moles of solute. As given
Since depression in freezing point depends upon the concentration of the solute, this parameter can be used to determine the molal concentration of the solution.
(d)
![Check Mark](/static/check-mark.png)
Interpretation:
A and B are two substances having equal number of moles. They are placed into separate
Concept Introduction:
Molality is one of the many parameters that is used to express concentration of a solution. It is expressed as,
Depression in freezing point of a substance can also be used to determine molality of the solution by rewriting the formula,
Answer to Problem 12.26QP
The new freezing point will be half of the freezing point of solution B that is
Explanation of Solution
Adding
Addition of excess solvent varies the solute concentration. Varying the solute concentration varies the freezing point of the solution.
(e)
![Check Mark](/static/check-mark.png)
Interpretation:
A and B are two substances having equal number of moles. They are placed into separate
Concept Introduction:
Molality is one of the many parameters that is used to express concentration of a solution. It is expressed as,
Depression in freezing point of a substance can also be used to determine molality of the solution by rewriting the formula,
Answer to Problem 12.26QP
The two solutions A and B have same freezing point at molality of
Explanation of Solution
As given
Since depression in freezing point depends upon the concentration of the solute, this parameter can be used to determine the molal concentration of the solution.
(f)
![Check Mark](/static/check-mark.png)
Interpretation:
A and B are two substances having equal number of moles. They are placed into separate
Osmotic pressure, vapor pressure, boiling points of both the solutions A and B has to be compared by theoretical explanation.
Concept Introduction:
Boiling point of a liquid substance is defined as the temperature at which the vapor pressure of the liquid becomes equal to the atmospheric pressure.
Elevation in boiling point of a substance can be determined by the formula,
Where,
Vapor pressure of a substance is known as the pressure exerted by molecules on the vapor phase when they are in equilibrium with their actual phase which can be liquid or solid.
Vapor pressure of a volatile solvent can be lowered by addition of a non-volatile solute. Raoult’s law deals with the vapor pressure of pure solvents and solution which states –
Partial pressure of solvent is equivalent to the product of vapor pressure of the solvent in its pure state and mole fraction of solvent in the solution. It is expressed as,
Where,
When the solute is non-volatile, the vapor pressure of the whole solution is equal to
The lowering of vapor pressure of the solvent due to the addition of non-volatile solute is expressed as,
Where,
In the process of osmosis, the solvent molecules pass through a semi - permeable membrane from less concentrated solution to more concentrated solution. The pressure that has to be applied to prevent the flow of solvent molecules is called osmotic pressure. It is expressed as,
Where,
Answer to Problem 12.26QP
The solution A will have lower boiling point, lower osmotic pressure and higher vapor pressure than solution B.
Explanation of Solution
Vapor pressure and boiling point share inverse relationship. But decrease in vapor pressure leads to decrease in freezing point. Higher the vapor pressure of the solution lower will be the boiling point of the solution. Since solution A has lower freezing point than solution B, it indicates lower vapor pressure and higher boiling point than solution B. Solution A has lower freezing point that it has lower osmotic pressure than solution B.
Vapor pressure and boiling point of the solution are dependent on each other. Osmotic pressure of the solution can be determined on the basis of freezing point or depression in freezing point.
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Chapter 12 Solutions
General Chemistry - Standalone book (MindTap Course List)
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- Instead of using NaCl to melt the ice on your sidewalk you decide to use CaCl2. If you add 35.0 g of CaCl2 to 150. g of water, what is the freezing point of the solution? (Assume i = 2.7 for CaCl2.)arrow_forwardIn a mountainous location, the boiling point of pure water is found to be 95C. How many grams of sodium chloride must be added to 1 kg of water to bring the boiling point back to 100C? Assume that i = 2.arrow_forwardConsider the following aqueous solutions: (i) 0.20 m HOCH2CH2OH (nonvolatile, nonelectrolyte); (ii) 0.10 m CaCl2 (iii) 0.12 m KBr; and (iv) 0.12 m Na2SO4. (a) Which solution has the highest boiling point? (b) Which solution has the lowest freezing point? (c) Which solution has the highest water vapor pressure?arrow_forward
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