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Questions and Answers
What happens to the vapor pressure of a solution when a non-volatile solute is added?
What happens to the vapor pressure of a solution when a non-volatile solute is added?
- It increases.
- It decreases. (correct)
- It remains the same.
- It doubles.
Raoult's Law states that the vapor pressure of a solution is dependent on the nature of the solute.
Raoult's Law states that the vapor pressure of a solution is dependent on the nature of the solute.
False (B)
What defines colligative properties?
What defines colligative properties?
Colligative properties depend on the number of solute particles, not their nature.
The relative lowering of vapor pressure of a solution is equal to the mole fraction of the ______.
The relative lowering of vapor pressure of a solution is equal to the mole fraction of the ______.
Which of the following represents a colligative property?
Which of the following represents a colligative property?
Match the following terms with their definitions:
Match the following terms with their definitions:
A volatile solute will contribute to the total vapor pressure of a solution.
A volatile solute will contribute to the total vapor pressure of a solution.
What is the normality of a solution containing 0.248 moles of sulfuric acid dissolved in 250mL of solution?
What is the normality of a solution containing 0.248 moles of sulfuric acid dissolved in 250mL of solution?
Molar solutions are more concentrated than molal solutions.
Molar solutions are more concentrated than molal solutions.
What is the effect of adding a non-volatile solute on the escaping tendency of solvent molecules?
What is the effect of adding a non-volatile solute on the escaping tendency of solvent molecules?
What is the molality of a solution containing 18 g of urea in 1.5 kg of solvent?
What is the molality of a solution containing 18 g of urea in 1.5 kg of solvent?
The mole fraction is a __________ quantity because it is a ratio of two numbers representing moles.
The mole fraction is a __________ quantity because it is a ratio of two numbers representing moles.
If 100g of sucrose is dissolved, how many grams of water are needed to prepare a 0.2 molal solution?
If 100g of sucrose is dissolved, how many grams of water are needed to prepare a 0.2 molal solution?
Raoult's law applies only to solutions containing volatile solutes.
Raoult's law applies only to solutions containing volatile solutes.
Calculate the mole fraction of water in a solution prepared by mixing 25g of water and 25g of ethanol.
Calculate the mole fraction of water in a solution prepared by mixing 25g of water and 25g of ethanol.
What is the definition of normality (N)?
What is the definition of normality (N)?
The molarity of a solution is calculated as the number of moles of solute per volume of solution in liters.
The molarity of a solution is calculated as the number of moles of solute per volume of solution in liters.
Calculate the normality of a solution containing 1.5 g of calcium hydroxide dissolved in 850 mL.
Calculate the normality of a solution containing 1.5 g of calcium hydroxide dissolved in 850 mL.
The equivalent weight of calcium is ______.
The equivalent weight of calcium is ______.
Match the following concentration units with their definitions:
Match the following concentration units with their definitions:
Which statement correctly describes the relationship between normality and molarity?
Which statement correctly describes the relationship between normality and molarity?
A dilute solution contains a higher concentration of solute than a concentrated solution.
A dilute solution contains a higher concentration of solute than a concentrated solution.
What is the mole fraction of solute if 2 moles of solute are dissolved in 8 moles of solvent?
What is the mole fraction of solute if 2 moles of solute are dissolved in 8 moles of solvent?
Flashcards
Normality
Normality
A measure of concentration, expressing the number of gram-equivalent weights of solute per liter of solution.
Molality (m)
Molality (m)
The number of moles of solute per kilogram of solvent.
Mole Fraction
Mole Fraction
The ratio of the moles of a component to the total moles of all components in a mixture.
Molarity
Molarity
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Temperature Dependence of Concentration
Temperature Dependence of Concentration
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Raoult's Law
Raoult's Law
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Mole Fraction of Solvent
Mole Fraction of Solvent
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Mole Fraction
Mole Fraction
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Mole (n)
Mole (n)
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Normality (N)
Normality (N)
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Equivalent weight
Equivalent weight
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Solution
Solution
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Concentrated solution
Concentrated solution
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Dilute solution
Dilute solution
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Relation between Normality and Molarity
Relation between Normality and Molarity
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Relative Lowering of Vapor Pressure
Relative Lowering of Vapor Pressure
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Colligative Properties
Colligative Properties
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Non-volatile Solute
Non-volatile Solute
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Vapor Pressure of Solution
Vapor Pressure of Solution
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Ebullioscopy
Ebullioscopy
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Cryoscopy
Cryoscopy
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Study Notes
Colligative Properties
- Colligative properties depend on the number of solute particles, not their nature.
- Key colligative properties include relative lowering of vapor pressure, elevation of boiling point, depression of freezing point, and osmotic pressure.
Solution Concentration Units
- Mole (n): The mass of a substance containing Avogadro's number (6.023 x 1023) of particles.
- Mole (n) = (Weight in grams) / (Molecular mass)
- Normality (N): Number of gram equivalents of solute per liter of solution.
- Gram equivalent weight of element = (Atomic weight)/(Valency)
- Gram equivalent weight of acid = (Molecular weight)/(Acidity)
- Gram equivalent weight of base = (Molecular weight)/(Basicity)
- Gram equivalent weight of salt= (Molecular weight)/(Total charge on cation or anion)
- Normality (N) = (No. of gram equivalents of solute) / (Volume of solution in liters)
- Molarity (M): Number of moles of solute per liter of solution.
- Molarity (M) = (No. of moles of solute)/(Volume of solution in liters)
- Molality (m): Number of moles of solute per kilogram of solvent.
- Molality (m) = (No. of moles of solute) / (Mass of solvent in kg)
- Mole Fraction (x): Ratio of moles of a component to the total moles of all components in a mixture.
- Mole fraction (x) = (Number of moles of a component) / (Total number of moles of all components)
Raoult's Law
- The vapor pressure of a solution containing a non-volatile solute is directly proportional to the mole fraction of the solvent.
- Psolution = Xsolvent × P°solvent
- Psolution = vapor pressure of the solution
- Xsolvent = mole fraction of the solvent
- P°solvent = vapor pressure of the pure solvent
Additional Notes
- Concentration units that vary with temperature are molarity and normality.
- Concentration units that are independent of temperature are molality and mole fraction.
- The vapor pressure of a solution is the pressure exerted by the vapor in equilibrium with the liquid at a given temperature.
- In a solution with a non-volatile solute, the vapor pressure is solely determined by the solvent.
Questions (Examples)
- Provided are example questions to calculate the normality, molarity, and molality of solutions.
- Calculations involve finding equivalent weights, molecular weights, and mole fractions of various substances. Solutions may contain calcium hydroxide, sulphuric acid.
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