Chemistry: Solubility Concepts
35 Questions
0 Views

Choose a study mode

Play Quiz
Study Flashcards
Spaced Repetition
Chat to Lesson

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

What term describes the process when a solute's particles separate from the solution?

  • Crystallisation (correct)
  • Dissolution
  • Saturation
  • Solvation

Which statement correctly describes a saturated solution?

  • It is unstable and will always precipitate.
  • It loses solute particles to the environment.
  • It has reached a point where no more solute can dissolve. (correct)
  • It contains less solute than can be dissolved.

What key factor influences whether a solid solute will dissolve in a liquid solvent?

  • The polarity of both solute and solvent. (correct)
  • The pressure applied.
  • Only temperature.
  • The color of the solute.

Which of the following combinations correctly follows the 'like dissolves like' principle?

<p>Sugar in water. (B)</p> Signup and view all the answers

What happens at equilibrium in a saturated solution?

<p>Dissolution and crystallisation occur at equal rates. (A)</p> Signup and view all the answers

How does temperature generally affect the solubility of solid solutes in liquids?

<p>Higher temperatures generally increase solubility. (C)</p> Signup and view all the answers

What characterizes an unsaturated solution?

<p>It can still dissolve more solute at the same temperature. (D)</p> Signup and view all the answers

What defines solubility in a given solvent?

<p>The maximum amount that can dissolve at specific conditions. (C)</p> Signup and view all the answers

What happens to the solubility of an endothermic dissolution process as temperature increases?

<p>Solubility increases (C)</p> Signup and view all the answers

Which of the following accurately describes an ideal solution?

<p>Has zero enthalpy and volume of mixing (C)</p> Signup and view all the answers

What characterizes a solution exhibiting positive deviation from Raoult's law?

<p>Higher vapor pressure than predicted (B)</p> Signup and view all the answers

Which of the following is an example of a binary mixture that exhibits a negative deviation from Raoult's law?

<p>Phenol and aniline (C)</p> Signup and view all the answers

What is a characteristic property of non-ideal solutions?

<p>Vapor pressure deviates from Raoult's law (C)</p> Signup and view all the answers

In the formation of an azeotrope, what occurs at the azeotropic composition?

<p>Liquid and vapor phases have the same composition (A)</p> Signup and view all the answers

What type of azeotrope results from a solution showing a significant positive deviation from Raoult’s law?

<p>Minimum boiling azeotrope (A)</p> Signup and view all the answers

Which of the following factors does NOT significantly affect the solubility of solids in liquids?

<p>Pressure changes (C)</p> Signup and view all the answers

Increasing the boiling point of a solvent when a non-volatile solute is added is known as:

<p>Elevation of boiling point (A)</p> Signup and view all the answers

What effect does adding a non-volatile solute have on the vapor pressure of a solution?

<p>Reduces vapor pressure (A)</p> Signup and view all the answers

What kind of interactions lead to negative deviations from Raoult’s law?

<p>Stronger intermolecular forces among A-B than A-A and B-B (D)</p> Signup and view all the answers

Which of the following is true regarding the relation of pressure and solubility of liquids?

<p>Solubility of gases increases significantly with pressure (C)</p> Signup and view all the answers

Which of the following properties is NOT affected by the addition of a non-volatile solute to a volatile solvent?

<p>Molecular weight of solute (B)</p> Signup and view all the answers

What are colligative properties dependent on?

<p>The total number of particles in the solution (C)</p> Signup and view all the answers

In which type of solution does no osmosis occur when separated by a semipermeable membrane?

<p>Isotonic solution (B)</p> Signup and view all the answers

What is the effect of placing blood cells in a hypertonic solution?

<p>Cells shrink and water flows out (C)</p> Signup and view all the answers

What happens to bacteria on salted meat due to osmosis?

<p>They lose water, shrivel, and die (C)</p> Signup and view all the answers

What effect does a higher concentration of sodium chloride have on blood cells?

<p>Stops water from entering the cells (A)</p> Signup and view all the answers

What type of solution has a salt concentration less than 0.9% (mass/volume)?

<p>Hypotonic solution (B)</p> Signup and view all the answers

When one mole of KCl is dissolved in water, how many moles of particles are expected in the solution?

<p>Two moles (C)</p> Signup and view all the answers

Why would the experimentally determined molar mass of an ionic compound be lower than the true value?

<p>Because of the degree of dissociation (C)</p> Signup and view all the answers

What is an abnormal molar mass in the context of association of molecules?

<p>Both A and B are correct (A)</p> Signup and view all the answers

What does Henry's law explain regarding the solubility of gases?

<p>It increases with high pressure (C)</p> Signup and view all the answers

What medical condition can arise for scuba divers due to dissolved gases when ascending?

<p>Decompression sickness (bends) (A)</p> Signup and view all the answers

How does temperature affect the solubility of gases in liquids?

<p>Decreases with temperature rise (D)</p> Signup and view all the answers

What is one consequence of placing high concentration gas mixtures in scuba tanks?

<p>Prevents nitrogen narcosis (A)</p> Signup and view all the answers

What process can be partly attributed to osmosis in plants?

<p>Water movement from soil into roots (B)</p> Signup and view all the answers

Flashcards

Solubility

The maximum amount of a substance that can dissolve in a given amount of solvent at a specific temperature and pressure.

Dissolution

The process of a solid dissolving in a liquid, increasing the concentration of the solute in the solution.

Crystallisation

The process of solute particles in a solution separating out and returning to the solid state.

Dynamic equilibrium

A state where the rate of dissolution is equal to the rate of crystallisation, resulting in a constant concentration of solute in the solution.

Signup and view all the flashcards

Saturated solution

A solution where no more solute can be dissolved at a given temperature and pressure.

Signup and view all the flashcards

Unsaturated solution

A solution where more solute can be dissolved at a given temperature.

Signup and view all the flashcards

Like dissolves like principle

Substances with similar intermolecular forces tend to dissolve in each other.

Signup and view all the flashcards

Effect of temperature on solubility

The solubility of a solid in a liquid is generally increased at higher temperatures.

Signup and view all the flashcards

Solubility and Temperature

In a nearly saturated solution, the solubility of a solid increases with temperature if the dissolution process is endothermic (heat is absorbed).

Signup and view all the flashcards

Solubility and Temperature (Exothermic)

In a nearly saturated solution, the solubility of a solid decreases with temperature if the dissolution process is exothermic (heat is released).

Signup and view all the flashcards

Pressure and Solubility

Pressure has no significant effect on the solubility of solids in liquids.

Signup and view all the flashcards

Ideal Solution

A solution is ideal when it obeys Raoult's law for all concentrations. This means the vapor pressure of each component is directly proportional to its mole fraction in the solution.

Signup and view all the flashcards

Enthalpy of Mixing (Ideal)

The enthalpy of mixing (heat change) for an ideal solution is zero, meaning no heat is absorbed or released when components are mixed.

Signup and view all the flashcards

Volume of Mixing (Ideal)

The volume of mixing for an ideal solution is zero, meaning the final volume is simply the sum of the initial volumes of the components.

Signup and view all the flashcards

Ideal Solution (Molecular)

The intermolecular forces between solute-solute and solvent-solvent molecules are similar to those between solute-solvent molecules.

Signup and view all the flashcards

Non-ideal Solution

A solution that does not follow Raoult's law over the entire range of concentrations.

Signup and view all the flashcards

Positive Deviation (Raoult's Law)

A non-ideal solution where the vapor pressure is higher than predicted by Raoult's law. This happens when solute-solvent interactions are weaker than solute-solute or solvent-solvent interactions.

Signup and view all the flashcards

Negative Deviation (Raoult's Law)

A non-ideal solution where the vapor pressure is lower than predicted by Raoult's law. This happens when solute-solvent interactions are stronger than solute-solute or solvent-solvent interactions.

Signup and view all the flashcards

Azeotrope

A mixture of two liquids with a fixed composition that boils at a constant temperature. The vapor phase has the same composition as the liquid phase.

Signup and view all the flashcards

Minimum Boiling Azeotrope

An azeotrope where the boiling point is lower than the boiling points of either pure component. This occurs due to strong positive deviations from Raoult's law.

Signup and view all the flashcards

Maximum Boiling Azeotrope

An azeotrope where the boiling point is higher than the boiling points of either pure component. This occurs due to strong negative deviations from Raoult's law.

Signup and view all the flashcards

Relative Lowering of Vapor Pressure

The relative lowering of vapor pressure of a solvent is directly proportional to the mole fraction of the non-volatile solute.

Signup and view all the flashcards

Solution Definition

A solution is a homogeneous mixture of two or more components.

Signup and view all the flashcards

Colligative Properties

Properties of solutions that depend only on the number of solute particles, regardless of their nature, relative to the total number of particles in the solution.

Signup and view all the flashcards

Semipermeable Membrane

A membrane that allows the passage of solvent molecules but restricts the passage of larger solute molecules.

Signup and view all the flashcards

Osmosis

The movement of solvent molecules from a region of higher solvent concentration to a region of lower solvent concentration across a semipermeable membrane.

Signup and view all the flashcards

Osmotic Pressure

The pressure that must be applied to a solution to prevent the inward flow of water across a semipermeable membrane.

Signup and view all the flashcards

Isotonic Solutions

Solutions having the same osmotic pressure at a given temperature, resulting in no net movement of water across a semipermeable membrane.

Signup and view all the flashcards

Hypertonic Solution

A solution with a higher osmotic pressure than another solution, causing water to flow out of the other solution.

Signup and view all the flashcards

Hypotonic Solution

A solution with a lower osmotic pressure than another solution, causing water to flow into the other solution.

Signup and view all the flashcards

Edema

The swelling or puffiness caused by the accumulation of fluid in tissues, often due to osmosis.

Signup and view all the flashcards

Henry's Law

The process by which the solubility of a gas in a liquid increases with increasing pressure.

Signup and view all the flashcards

Bends

A condition caused by the formation of nitrogen bubbles in the blood due to a rapid decrease in pressure, often experienced by scuba divers.

Signup and view all the flashcards

Anoxia

A medical condition caused by low blood oxygen levels, often occurring at high altitudes due to lower oxygen pressure.

Signup and view all the flashcards

Abnormal Molar Mass

The phenomenon where the experimentally determined molar mass of a substance differs from the true value due to dissociation or association of solute particles in solution.

Signup and view all the flashcards

Association

The process where molecules of a substance join together in solution, forming larger units.

Signup and view all the flashcards

Study Notes

Solubility of Substances

  • Solubility is the maximum amount of solute that dissolves in a given amount of solvent at a specific temperature and pressure.
  • Solubility depends on the nature of both the solute and solvent. Polar solutes dissolve in polar solvents, and nonpolar solutes dissolve in nonpolar solvents ("like dissolves like").
  • Dissolution is the process where a solute dissolves in a solvent.
  • Crystallization is the process where solute particles separate from the solution.
  • A saturated solution contains the maximum amount of solute dissolved at a given temperature and pressure.
  • Unsaturated solutions can dissolve more solute at the same temperature.

Temperature Effects on Solubility

  • The solubility of a solid in a liquid is significantly affected by temperature.
  • If the dissolution process is endothermic (ΔHsol > 0), solubility increases with temperature.
  • If the dissolution process is exothermic (ΔHsol < 0), solubility decreases with temperature.
  • These trends are observed experimentally.

Pressure Effects on Solubility

  • Pressure has a negligible effect on the solubility of solids in liquids because they are practically incompressible.

Ideal Solutions

  • Ideal solutions obey Raoult's Law at all concentrations.
  • Enthalpy of mixing (ΔmixH) and volume of mixing (ΔmixV) are both zero for ideal solutions.
  • In ideal solutions, intermolecular attractive forces between A-A, B-B, and A-B are similar.
  • Examples include n-hexane and n-heptane, bromoethane and chloroethane, benzene and toluene.

Non-Ideal Solutions

  • Non-ideal solutions do not obey Raoult's Law throughout all concentrations.
  • Solutions can show positive or negative deviations from Raoult's Law.
  • Positive deviations occur when A-B interactions are weaker than A-A or B-B interactions (e.g., ethanol and acetone). Vapor pressure is higher than predicted by Raoult's Law.
  • Negative deviations occur when A-B interactions are stronger than A-A or B-B interactions (e.g., phenol and aniline). Vapor pressure is lower than predicted by Raoult's Law.

Azeotropes

  • Azeotropes are binary mixtures with identical compositions in liquid and vapor phases.
  • They boil at constant temperatures and cannot be separated by fractional distillation.
  • Minimum boiling azeotropes form when solutions show large positive deviations from Raoult's Law.
  • Maximum boiling azeotropes form when solutions show large negative deviations from Raoult's Law.

Colligative Properties

  • Colligative properties depend on the** number** of solute particles, not their nature.
  • Examples include: relative lowering of vapor pressure, depression of freezing point, elevation of boiling point, and osmotic pressure.
  • These properties are useful in understanding phenomena like pickling food or water movement in plants.

Osmosis and Isotonic Solutions

  • Isotonic solutions have the same osmotic pressure at a given temperature.
  • No osmosis occurs between such solutions separated by a semipermeable membrane.
  • Normal saline (0.9% sodium chloride) is isotonic with blood.
  • Hypertonic solutions have a higher solute concentration than isotonic ones, causing water to flow out of cells.
  • Hypotonic solutions have a lower solute concentration, and water flows into cells, causing swelling.

Ionic Compounds and Molar Mass

  • Ionic compounds dissociate into ions when dissolved in water; this affects experimentally determined molar mass.
  • Abnormal molar mass occurs when molecules associate or dissociate in solution. This affects colligative properties.

Henry's Law and Applications

  • Henry's law describes the solubility of gases in liquids.
  • Increased pressure increases gas solubility.
  • Scuba diving (bends) and high-altitude effects are examples related to Henry's Law.
  • Soft drinks (increased CO2 solubility due to pressure) is also an example.

Effect of Temperature on Gas Solubility

  • Gas solubility decreases with increasing temperature.
  • Gas dissolution is an exothermic process, meaning heat is evolved during dissolution; hence, solubility decreases with increasing temperature.

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

Quiz Team

Description

This quiz explores the principles of solubility, including how temperature affects the solubility of substances. Learn about saturated and unsaturated solutions, and the relationship between polar and nonpolar solutes and solvents. Test your understanding of these critical chemistry concepts.

More Like This

Use Quizgecko on...
Browser
Open
Browser
Browser