Chemistry Solutions and Colloids Quiz
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Questions and Answers

What characterizes a saturated solution?

  • It has less solute than a supersaturated solution.
  • It can dissolve any amount of solute regardless of temperature.
  • It contains the maximum amount of solute that can be dissolved by the solvent. (correct)
  • It is unstable and separates into phases.

    • What occurs during the seeding process in crystallization?

  • The solvent temperature is lowered to increase solubility.
  • The solute is completely removed from the solution.
  • A crystal of the solute is added to promote crystallization. (correct)
  • A supersaturated solution is diluted.

    • Which of the following best describes a semipermeable membrane?

  • It allows all types of molecules to pass through freely.
  • It is impermeable to both solvents and solutes.
  • It only permits solvent molecules to pass and retains solute particles. (correct)
  • It allows only solute particles to pass through.

    • What does the Tyndall Effect demonstrate?

    <p>Scattering of light as it passes through a colloid.</p> Signup and view all the answers

    Which statement is true about weak electrolytes?

    <p>They partially dissociate into ions and conduct electricity weakly.</p> Signup and view all the answers

    What term describes a liquid with a solute added that raises its boiling point?

    <p>Boiling-Point Elevation</p> Signup and view all the answers

    Which solution would cause red blood cells to swell and potentially burst?

    <p>Hypotonic Solution</p> Signup and view all the answers

    What process allows small molecules to pass through a semipermeable membrane while retaining larger molecules?

    <p>Dialysis</p> Signup and view all the answers

    Which term describes the phenomenon where water flows out of red blood cells causing them to shrivel?

    <p>Crenation</p> Signup and view all the answers

    Which term refers to a mixture that is not uniform throughout?

    <p>Heterogeneous Mixture</p> Signup and view all the answers

    What is the definition of colligative properties?

    <p>Properties that depend only on the number of solute particles</p> Signup and view all the answers

    What is the term for a solution that has the same salt concentration as red blood cells?

    <p>Isotonic Solution</p> Signup and view all the answers

    Which of the following describes the property of a substance that can absorb water vapor from the air?

    <p>Hygroscopic</p> Signup and view all the answers

    What is the relationship defined by Henry’s Law?

    <p>Solubility of a gas in liquid is directly proportional to pressure</p> Signup and view all the answers

    Which term indicates a mixture of two or more metals?

    <p>Alloy</p> Signup and view all the answers

    What characterizes a supersaturated solution?

    <p>It contains more solute than it should at a specific temperature.</p> Signup and view all the answers

    What is the primary function of a semipermeable membrane in a solution?

    <p>To allow only solvent molecules to pass through while retaining solute particles.</p> Signup and view all the answers

    How does solvation occur for an ionic compound in solution?

    <p>Solvent molecules surround the ions due to stronger attraction than ionic bonds.</p> Signup and view all the answers

    What effect does a strong electrolyte have in solution?

    <p>It completely dissociates into ions.</p> Signup and view all the answers

    What is a defining characteristic of a suspension?

    <p>It contains particles larger than 1000 nm that settle over time.</p> Signup and view all the answers

    What is the process called when water flows into red blood cells causing them to burst?

    <p>Hemolysis</p> Signup and view all the answers

    Which property describes a solution that only depends on the number of solute particles present?

    <p>Colligative Property</p> Signup and view all the answers

    Which term describes a crystal that has had all its water removed?

    <p>Anhydrous</p> Signup and view all the answers

    What occurs when a liquid's boiling point is increased due to the addition of a solute?

    <p>Boiling-Point Elevation</p> Signup and view all the answers

    Which solution would have a lower osmotic pressure than red blood cells?

    <p>Hypotonic Solution</p> Signup and view all the answers

    Which of the following describes a mixture that is uniform throughout?

    <p>Homogeneous Mixture</p> Signup and view all the answers

    What is the term for a solution that contains ions and can carry an electric current?

    <p>Electrolyte</p> Signup and view all the answers

    What is the process called when solvent molecules pass through a semipermeable membrane from a less concentrated solution to a more concentrated one?

    <p>Osmosis</p> Signup and view all the answers

    Which term describes a solution with the same osmotic pressure as red blood cells?

    <p>Isotonic Solution</p> Signup and view all the answers

    What is the effect called when solute particles in a solution disrupt the orderly arrangement of water molecules, causing the freezing point to decrease?

    <p>Freezing-Point Depression</p> Signup and view all the answers

    What is the characteristic of a hypertonic solution in relation to red blood cells?

    <p>It has a higher osmolarity than red blood cells.</p> Signup and view all the answers

    Which term describes two liquids that can mix in all proportions?

    <p>Miscible</p> Signup and view all the answers

    How does a hypotonic solution affect red blood cells?

    <p>It causes red blood cells to swell and potentially burst.</p> Signup and view all the answers

    What property describes a substance that readily absorbs water vapor from the air?

    <p>Hygroscopic</p> Signup and view all the answers

    What defines an isotonic solution in relation to blood cells?

    <p>It has the same osmolarity as blood cells.</p> Signup and view all the answers

    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.
    • 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.

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