Chemistry Chapter: Solutions and Properties
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Questions and Answers

What is normality?

Normality is referred to as the equivalent concentration of a solution.

Normality is calculated by multiplying ______ by the number of protons performing units.

molarity

What is the normality of a 0.15 M solution of HCl?

0.15 N

What is the normality of a 1.4 M solution of H2SO4?

<p>2.8 N</p> Signup and view all the answers

What is the normality of a 2 M solution of NaOH?

<p>2 N</p> Signup and view all the answers

What is ppm?

<p>Parts per million</p> Signup and view all the answers

What is the concentration in ppm of a solution containing 4 mg of NaCl dissolved in 8 kg of water?

<p>0.5 ppm</p> Signup and view all the answers

What are Colligative Properties?

<p>Colligative properties are those that depend only on the number of solute particles in a solution, and not on the type of solute particles.</p> Signup and view all the answers

What are the three important colligative properties of solutions?

<p>Vapor-pressure lowering, boiling-point elevation, freezing-point depression (D)</p> Signup and view all the answers

Why do people spread salt on roads in the winter?

<p>Salt is spread on roads in the winter to lower the freezing point of water and prevent ice from forming.</p> Signup and view all the answers

The magnitude of the freezing-point depression is proportional to the number of solute particles dissolved in the solvent but does depend upon their identity.

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

What is the freezing point of a 1m solution of NaCl?

<p>-1.86 °C.</p> Signup and view all the answers

What is the boiling point elevation of a 1m solution of NaCl?

<p>1.02°C/m</p> Signup and view all the answers

Flashcards

Colligative Properties

The study of how the physical properties of a solution are affected by the concentration of dissolved particles.

Colligative Property

A property of a solution that depends only on the number of solute particles (concentration) and not their identity.

Vapor Pressure Lowering

A solution containing non-volatile solutes has a lower vapor pressure than the pure solvent.

Boiling Point Elevation

The difference in temperature between the boiling point of a solution and the boiling point of the pure solvent. The boiling point of a solution is always higher than that of the pure solvent.

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Freezing Point Depression

The difference in temperature between the freezing point of a solution and the freezing point of the pure solvent. The freezing point of a solution is always lower than that of the pure solvent.

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Molarity

A unit of concentration used to express the amount of a solute dissolved in a solvent. It represents the number of moles of solute per liter of solution.

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Normality

A unit of concentration used to express the amount of a solute dissolved in a solvent. It represents the number of equivalents of solute per liter of solution.

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Equivalent

The number of moles of a substance that can react with or provide one mole of hydrogen ions (H+) in a chemical reaction.

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Parts Per Million (ppm)

A unit of concentration used to express the amount of a dissolved substance in a solution. It represents the number of grams of solute per million grams of solution.

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Dissolving

The process by which a substance dissolves in a solvent to form a solution.

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Solute

The substance being dissolved in a solvent.

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Solvent

The substance that dissolves the solute to form a solution.

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Solution

A homogeneous mixture of two or more substances, where one substance (the solute) is dissolved in another substance (the solvent).

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Insoluble

A substance that does not dissolve in a particular solvent.

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Soluble

A substance that dissolves in a particular solvent.

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Solubility

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

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Dissociation

The process by which a substance breaks down into smaller particles when dissolved in a solvent.

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Electrolyte

A substance that dissociates into ions when dissolved in a solvent.

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Nonelectrolyte

A substance that does not dissociate into ions when dissolved in a solvent.

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Exothermic Dissolution

The process by which a substance increases in temperature when dissolved in a solvent.

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Endothermic Dissolution

The process by which a substance decreases in temperature when dissolved in a solvent.

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Molality

The number of moles of solute per kilogram of solvent.

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Van't Hoff Factor (i)

A factor that accounts for the number of particles a solute produces when dissolved in a solvent.

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Saturated Solution

The state of a solution where no more solute can dissolve at a specific temperature.

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Unsaturated Solution

The state of a solution where less solute is dissolved than the maximum solubility at a specific temperature.

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Supersaturated Solution

The state of a solution where more solute than the maximum solubility is dissolved at a specific temperature, usually achieved by increasing temperature or pressure.

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Precipitation

The process by which a dissolved substance comes out of solution, usually by changing temperature or pressure.

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Study Notes

Chemical Composition of Water

  • Water's chemical formula is H₂O.

Solution Concentrations

  • Normality (N): Normality is the equivalent concentration. N = Molarity (M) x n. n is the number of protons or hydrogen ions.

  • Molarity (M): Molarity is the number of moles of solute per liter of solution.

  • Parts Per Million (PPM): PPM = (grams of solute / grams of solution) x 10⁶

Colligative Properties of Solutions

  • Colligative Property: A property dependent on the number of solute particles in solution, not the identity of the solute.

  • Three Important Colligative Properties: Vapor-pressure lowering, Boiling-point elevation, and Freezing-point depression.

Vapor-Pressure Lowering

  • Vapor Pressure: The pressure exerted by a vapor in dynamic equilibrium with its liquid.

  • Solution Vapor Pressure: Solutions with solutes that do not easily vaporize have lower vapor pressure than pure solvents.

Freezing-Point Depression

  • Freezing-Point Depression: The magnitude of the freezing-point depression is proportional to the number of solute particles, regardless of the solute's identity.

  • Road Salt in Winter: People spread salt on roads in winter to lower the freezing point of water, preventing ice formation.

Boiling-Point Elevation

  • Boiling Point: The temperature at which the vapor pressure of the liquid equals atmospheric pressure.

  • Solution Boiling Point: The boiling point of a solution is always higher than the boiling point of the pure solvent.

  • Magnitude of Boiling-Point Elevation: The magnitude of boiling-point elevation is proportional to the number of solute particles.

  • Calculations: The change in boiling point (ΔT) is calculated using the formula: ΔT = Kb x m x i, where Kb is the boiling point elevation constant, m is the molality, and i is the van't Hoff factor.

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Description

This quiz explores the chemical composition of water and the various solution concentrations, including normality, molarity, and parts per million. Additionally, it covers colligative properties such as vapor-pressure lowering, boiling-point elevation, and freezing-point depression. Test your understanding of these fundamental concepts in chemistry!

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