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Questions and Answers
According to Henry's Law, how does gas solubility (S) change with partial pressure (P) at a constant temperature?
According to Henry's Law, how does gas solubility (S) change with partial pressure (P) at a constant temperature?
Which of the following factors directly influences colligative properties of a solution?
Which of the following factors directly influences colligative properties of a solution?
A solution containing two volatile liquids, A and B, has a vapor pressure of $P$. If the mole fraction of A is $X_A$ and of B is $X_B$, and the vapor pressures of pure A and B are $P°A$ and $P°B$ respectively, what does Raoult's Law state about $P$?
A solution containing two volatile liquids, A and B, has a vapor pressure of $P$. If the mole fraction of A is $X_A$ and of B is $X_B$, and the vapor pressures of pure A and B are $P°A$ and $P°B$ respectively, what does Raoult's Law state about $P$?
What would suggest a negative deviation from Raoult's Law in a non-ideal solution?
What would suggest a negative deviation from Raoult's Law in a non-ideal solution?
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How does the presence of a common ion affect the solubility of a sparingly soluble salt in a solution?
How does the presence of a common ion affect the solubility of a sparingly soluble salt in a solution?
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Which concentration unit is defined as the number of moles of solute per kilogram of solvent?
Which concentration unit is defined as the number of moles of solute per kilogram of solvent?
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If the temperature of a solution increases, how is the solubility of most solid solutes generally affected?
If the temperature of a solution increases, how is the solubility of most solid solutes generally affected?
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According to Henry's Law, what is the relationship between the solubility of a gas in a liquid and the partial pressure of the gas above the liquid?
According to Henry's Law, what is the relationship between the solubility of a gas in a liquid and the partial pressure of the gas above the liquid?
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Which concentration unit is most suitable for expressing the concentration of a very dilute solution?
Which concentration unit is most suitable for expressing the concentration of a very dilute solution?
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If the mass of a solute is 10 grams and the mass of the solution is 100 grams, what is the mass percent of the solute in the solution?
If the mass of a solute is 10 grams and the mass of the solution is 100 grams, what is the mass percent of the solute in the solution?
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Which concentration unit is affected by changes in temperature?
Which concentration unit is affected by changes in temperature?
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What is the effect of increasing pressure on the solubility of a gas in a liquid?
What is the effect of increasing pressure on the solubility of a gas in a liquid?
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Which of the following is a homogeneous mixture of two or more components?
Which of the following is a homogeneous mixture of two or more components?
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Study Notes
Solutions - Class 12 Chemistry
- A solution is a homogeneous mixture of two or more components.
- The component present in the larger amount is called the solvent, and the other component(s) are called the solute(s).
- Solutions can exist in various states: solid (e.g., alloys), liquid (e.g., saltwater), or gas (e.g., air).
- The concentration of a solution is a measure of the amount of solute present in a given amount of solvent or solution.
- Various concentration units exist, including molarity (mol/L), molality (mol/kg), mass percent, volume percent, and parts per million (ppm).
Molarity
- Molarity (M) is defined as the number of moles of solute per liter of solution.
- It is a measure of the concentration of solute in a solution.
- Formula: Molarity = (moles of solute) / (liters of solution)
- Molarity changes with temperature due to the change in volume.
Molality
- Molality (m) is the number of moles of solute per kilogram of solvent.
- It is independent of temperature.
- Formula: Molality = (moles of solute) / (kilograms of solvent)
- Molality is preferred over molarity when dealing with temperature variations.
Mass Percent
- Mass percent is the mass of the solute divided by the mass of the solution, multiplied by 100.
- Formula: Mass percent = (mass of solute / mass of solution) x 100
- Useful for expressing the concentration of solid solutes in solid solvents.
Volume Percent
- Volume percent expresses the volume of solute in 100 units of volume of solution.
- Formula: Volume percent = (volume of solute / volume of solution) x 100
- Commonly used for liquid solutions.
Parts per Million (ppm)
- Parts per million (ppm) is a measure of the concentration of a very dilute solution.
- It represents the number of parts of solute per one million parts of solution.
- Formula: ppm = (mass of solute / mass of solution) x 10^6
- Used for extremely dilute solutions.
Factors Affecting Solubility
- Temperature generally increases the solubility of solids and gases.
- For solids, solubility typically increases with temperature.
- For gases, solubility typically decreases with temperature.
- Pressure significantly affects the solubility of gases, with higher pressure leading to greater solubility, as described by Henry's Law.
Henry's Law
- Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid.
- Mathematically represented as: S = kH P
- Where S is the solubility of the gas, kH is Henry's Law constant, and P is the partial pressure of the gas.
Colligative Properties of Solutions
- Colligative properties depend on the number of solute particles, not the nature of the solute.
- These properties include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
- The extent of the colligative properties changes correlates directly with the number of solute particles.
Raoult's Law
- For a solution of volatile liquids, the vapor pressure of the solution is equal to the sum of the vapor pressures of each component in the solution.
- Formula: P = P°A × X_A + P°B × X_B (where P°A and P°B are the vapor pressures of pure components A and B, and X_A and X_B are their mole fractions).
- This principle helps understand the behavior of volatile solutions.
Ideal and Non-Ideal Solutions
- Ideal solutions obey Raoult's Law perfectly.
- Non-ideal solutions do not obey Raoult's Law.
- The deviation from Raoult's Law can be positive or negative.
- Positive deviations indicate solute–solute or solvent–solvent interactions are weaker than solute–solvent interactions.
- Negative deviations indicate solute–solute or solvent–solvent interactions are stronger than solute–solvent interactions.
Solubility of Ionic Compounds
- The solubility of ionic compounds in water depends on the balance between the lattice energy of the solid and the hydration energy of the ions.
- Common Ion Effect: The solubility of a sparingly soluble salt is decreased in a solution containing a common ion.
- Precipitation of ionic compounds can be predicted based on solubility rules.
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Description
Explore the concepts of solutions and their properties in this quiz designed for Class 12 Chemistry. You'll learn about the definitions of solvents and solutes, different types of solutions, and important concentration units like molarity and molality. Test your knowledge and enhance your understanding of these fundamental concepts!
