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?

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

Which statement is true about weak electrolytes?

They partially dissociate into ions and conduct electricity weakly. Signup and view all the answers

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

Boiling-Point Elevation Signup and view all the answers

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

Hypotonic Solution Signup and view all the answers

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

Dialysis Signup and view all the answers

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

Crenation Signup and view all the answers

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

Heterogeneous Mixture Signup and view all the answers

What is the definition of colligative properties?

Properties that depend only on the number of solute particles Signup and view all the answers

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

Isotonic Solution Signup and view all the answers

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

Hygroscopic Signup and view all the answers

What is the relationship defined by Henry’s Law?

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

Which term indicates a mixture of two or more metals?

Alloy Signup and view all the answers

What characterizes a supersaturated solution?

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

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

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

How does solvation occur for an ionic compound in solution?

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

What effect does a strong electrolyte have in solution?

It completely dissociates into ions. Signup and view all the answers

What is a defining characteristic of a suspension?

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

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

Hemolysis Signup and view all the answers

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

Colligative Property Signup and view all the answers

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

Anhydrous Signup and view all the answers

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

Boiling-Point Elevation Signup and view all the answers

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

Hypotonic Solution Signup and view all the answers

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

Homogeneous Mixture Signup and view all the answers

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

Electrolyte 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?

Osmosis Signup and view all the answers

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

Isotonic Solution 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?

Freezing-Point Depression Signup and view all the answers

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

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

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

Miscible Signup and view all the answers

How does a hypotonic solution affect red blood cells?

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

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

Hygroscopic Signup and view all the answers

What defines an isotonic solution in relation to blood cells?

It has the same osmolarity as blood cells. 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.