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Questions and Answers
What characterizes a saturated solution?
What characterizes a saturated solution?
What occurs during the seeding process in crystallization?
What occurs during the seeding process in crystallization?
Which of the following best describes a semipermeable membrane?
Which of the following best describes a semipermeable membrane?
What does the Tyndall Effect demonstrate?
What does the Tyndall Effect demonstrate?
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Which statement is true about weak electrolytes?
Which statement is true about weak electrolytes?
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What term describes a liquid with a solute added that raises its boiling point?
What term describes a liquid with a solute added that raises its boiling point?
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Which solution would cause red blood cells to swell and potentially burst?
Which solution would cause red blood cells to swell and potentially burst?
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What process allows small molecules to pass through a semipermeable membrane while retaining larger molecules?
What process allows small molecules to pass through a semipermeable membrane while retaining larger molecules?
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Which term describes the phenomenon where water flows out of red blood cells causing them to shrivel?
Which term describes the phenomenon where water flows out of red blood cells causing them to shrivel?
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Which term refers to a mixture that is not uniform throughout?
Which term refers to a mixture that is not uniform throughout?
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What is the definition of colligative properties?
What is the definition of colligative properties?
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What is the term for a solution that has the same salt concentration as red blood cells?
What is the term for a solution that has the same salt concentration as red blood cells?
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Which of the following describes the property of a substance that can absorb water vapor from the air?
Which of the following describes the property of a substance that can absorb water vapor from the air?
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What is the relationship defined by Henry’s Law?
What is the relationship defined by Henry’s Law?
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Which term indicates a mixture of two or more metals?
Which term indicates a mixture of two or more metals?
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What characterizes a supersaturated solution?
What characterizes a supersaturated solution?
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What is the primary function of a semipermeable membrane in a solution?
What is the primary function of a semipermeable membrane in a solution?
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How does solvation occur for an ionic compound in solution?
How does solvation occur for an ionic compound in solution?
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What effect does a strong electrolyte have in solution?
What effect does a strong electrolyte have in solution?
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What is a defining characteristic of a suspension?
What is a defining characteristic of a suspension?
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What is the process called when water flows into red blood cells causing them to burst?
What is the process called when water flows into red blood cells causing them to burst?
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Which property describes a solution that only depends on the number of solute particles present?
Which property describes a solution that only depends on the number of solute particles present?
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Which term describes a crystal that has had all its water removed?
Which term describes a crystal that has had all its water removed?
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What occurs when a liquid's boiling point is increased due to the addition of a solute?
What occurs when a liquid's boiling point is increased due to the addition of a solute?
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Which solution would have a lower osmotic pressure than red blood cells?
Which solution would have a lower osmotic pressure than red blood cells?
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Which of the following describes a mixture that is uniform throughout?
Which of the following describes a mixture that is uniform throughout?
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What is the term for a solution that contains ions and can carry an electric current?
What is the term for a solution that contains ions and can carry an electric current?
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What is the process called when solvent molecules pass through a semipermeable membrane from a less concentrated solution to a more concentrated one?
What is the process called when solvent molecules pass through a semipermeable membrane from a less concentrated solution to a more concentrated one?
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Which term describes a solution with the same osmotic pressure as red blood cells?
Which term describes a solution with the same osmotic pressure as red blood cells?
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What is the effect called when solute particles in a solution disrupt the orderly arrangement of water molecules, causing the freezing point to decrease?
What is the effect called when solute particles in a solution disrupt the orderly arrangement of water molecules, causing the freezing point to decrease?
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What is the characteristic of a hypertonic solution in relation to red blood cells?
What is the characteristic of a hypertonic solution in relation to red blood cells?
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Which term describes two liquids that can mix in all proportions?
Which term describes two liquids that can mix in all proportions?
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How does a hypotonic solution affect red blood cells?
How does a hypotonic solution affect red blood cells?
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What property describes a substance that readily absorbs water vapor from the air?
What property describes a substance that readily absorbs water vapor from the air?
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What defines an isotonic solution in relation to blood cells?
What defines an isotonic solution in relation to blood cells?
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Study Notes
Solutions and Colloids
- Solutions: Homogeneous mixtures of two or more substances, where the solute dissolves in the solvent.
- Colloids: Heterogeneous mixtures with solute particles ranging from 1 to 1000 nm; exhibit the Tyndall Effect.
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Types of Colloids:
- Emulsions: Liquids dispersed in liquids.
- Suspensions: Particles larger than 1000 nm, unstable and separate into phases.
Solution Concentration
- Concentration: The amount of solute dissolved in a specific amount of solvent.
- Molarity (M): Moles of solute per liter of solution.
- Percent Concentration (%w/v): Grams of solute per 100 mL of solution.
- Parts per million (ppm): Grams of solute per million grams of solution.
- Parts per billion (ppb): Grams of solute per billion grams of solution.
Solution Properties
- Colligative Properties: Depend only on the number of solute particles, not their identity.
- Boiling-Point Elevation: The increase in boiling point of a liquid caused by a solute.
- Freezing-Point Depression: The decrease in freezing point of a liquid caused by a solute.
- Osmosis: The movement of solvent molecules across a semipermeable membrane from a less concentrated solution to a more concentrated one.
- Osmotic Pressure: The external pressure required to stop osmosis.
- Isotonic Solutions: Solutions with the same osmolarity.
- Hypotonic Solutions: Solutions with lower osmolarity than red blood cells, causing hemolysis.
- Hypertonic Solutions: Solutions with higher osmolarity than red blood cells, causing crenation.
Electrolytes
- Electrolyte: A solution that conducts electricity due to the presence of ions.
- Nonelectrolyte: A solution that does not conduct electricity.
- Strong Electrolyte: Dissociates completely into ions in solution.
- Weak Electrolyte: Dissociates only partially into ions in solution.
Solubility
- Solubility: The maximum amount of solute that can dissolve in a given solvent at a specific temperature.
- Saturated Solution: Contains the maximum amount of dissolved solute.
- Unsaturated Solution: Contains less than the maximum amount of dissolved solute.
- Supersaturated Solution: Contains more solute than it should at a given temperature, unstable.
Hydrates
- Hydrates: Compounds containing water molecules in their crystal structure.
- Anhydrous: A crystal with water removed.
- Water of Hydration: The water molecules in a hydrate.
- Hygroscopic: Substances that absorb water vapor from the air.
Other Terms
- Anode: Positive electrode, attracts anions.
- Cathode: Negative electrode, attracts cations.
- Dialysis: Separation of solutes based on size using a semipermeable membrane.
- Seeding: Adding a crystal of solute to a supersaturated solution to induce crystallization
- Henry's Law: The solubility of a gas in a liquid is directly proportional to its partial pressure.
- Solvated: When a solute molecule is surrounded by solvent molecules.
Alloys
- Homogeneous mixtures of two or more metals
Anhydrous
- A crystal that has had the water removed
Anode
- The positive electrode
- Anions migrate to the positive electrode
Boiling-Point Elevation
- Occurs when a solute is added to a liquid, increasing its boiling point
Brownian Motion
- Random, chaotic motion of any colloidal particle
Cathode
- The negative electrode
- Cations migrate to the negative electrode
Colligative Property
- Property of a solution dependent on the number of solute particles, not the chemical identity of the solute
Colloid
- Two-part system where solute particles range from 1 to 1000 nm
Concentration
- Amount of solute dissolved in a given quantity of solvent
Crenation
- Osmotic process where water flows out of red blood cells through a semipermeable membrane, causing the cells to shrivel
Dialysis
- Process where a solution containing particles of different sizes is placed in a semipermeable membrane bag
- The bag is placed in a solvent or solution containing only small molecules
- The solution in the bag reaches equilibrium with the solvent outside, allowing small molecules to diffuse across the membrane, retaining large molecules
Electrolyte
- Solution containing ions capable of carrying an electric current
Emulsions
- Systems where a liquid, with or without an emulsifying agent, is in an immiscible liquid, usually as droplets larger than colloidal size
Freezing-Point Depression
- Decrease in the freezing point of a liquid caused by adding a solute
Hemolysis
- Osmotic process where water flows into red blood cells through the semipermeable membrane, causing the cells to burst
Henry's Law
- Solubility of a gas in a liquid is directly proportional to the pressure
Heterogeneous Mixture
- Mixture that is not uniform throughout
Homogeneous Mixture
- Mixture that is uniform throughout
Hydrated
- Occurs when a solid ionic compound is dissolved in water, and the water molecules surround the ions when the combined force of attraction of the water molecules is greater than the force of attraction of the ionic bonds
Hydrates
- Substances that contain water in their crystals
Hygroscopic
- A substance that absorbs water vapor from the air
Hypertonic Solution
- Solutions where the osmolarity and osmotic pressure are greater than red blood cells
Hypotonic Solution
- Solutions where the osmolarity and osmotic pressure are lower than red blood cells
Immiscible
- Liquids that don't mix
Isotonic
- Two solutions with the same osmolarity
Isotonic Solution
- Solution that has the same salt concentration as cells and blood
Miscible
- Liquids that mix in all proportions
Molarity (M)
- Moles per liter, a unit of concentration
Nonelectrolyte
- Solution that does not contain ions and cannot carry an electric current
Osmolarity
- Molarity multiplied by the number of particles in solution in each formula unit of solute
Osmosis
- The passage of solvent molecules from a less concentrated solution across a semipermeable membrane into a more concentrated solution
Osmotic Pressure
- Amount of external pressure needed to stop the passage of solvent molecules across a semipermeable membrane
Parts per Billion (ppb)
- Concentration of a solution in grams of solute per billion grams of solution
Parts per Million (ppm)
- Concentration of a solution in grams of solute per million grams of solution
Percent Concentration (%w/v)
- Number of grams of solute in 100 mL of solution
Saturated Solution
- Solution containing the maximum amount of solute that can be dissolved by that solvent at a given temperature
Seeding
- Process used to crystallize excess solute of a supersaturated solution by adding a crystal of the solute
Semipermeable Membrane
- Substance containing tiny pores that only allow solvent molecules to pass through while retaining solvated solute particles
Solubility
- Amount of solute, in grams, that can be dissolved in 100 mL of solvent at a given temperature
Solute
- Substance dissolved to make a solution
Solvated
- When a solid ionic compound is dissolved in a solvent, the solvent molecules surround the ions when the combined force of attraction to the solvent molecules is greater than the force of attraction of the ionic bond
Solvent
- Chemical that dissolves the solute
Strong Electrolyte
- Compound that dissociates completely into ions
Supersaturated Solution
- Solution containing more solute than it should
Suspension
- System where colloidal particles are larger than 1000 nm, although unstable and separates into phases
Tyndall Effect
- Light passing through and scattered by a colloid viewed at a right angle
Unsaturated Solution
- Solution containing less than the maximum amount of solvent dissolved in it.
Water of Hydration
- Water molecules in a crystal
Weak Electrolyte
- Compound that dissociates only partially into ions
Solutions and Properties
- Hydrates are substances containing water molecules within their crystal structures.
- Hygroscopic substances readily absorb water vapor from the air.
- Hypertonic solutions have a higher osmolarity and osmotic pressure than red blood cells, leading to water movement out of the cells.
- Hypotonic solutions have a lower osmolarity and osmotic pressure than red blood cells, causing water to move into the cells.
- Immiscible liquids do not mix, forming distinct layers.
- Isotonic solutions have the same osmolarity, meaning they exert the same osmotic pressure.
- Isotonic solutions have the same salt concentration as cells and blood, maintaining cellular equilibrium.
- Miscible liquids mix in all proportions, forming a homogeneous solution.
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Description
Test your knowledge on solutions and colloids, including their properties, types, and concentration measures. Understand the differences between homogeneous and heterogeneous mixtures, as well as important concepts like molarity and colligative properties. This quiz will help reinforce key concepts from your chemistry studies.
