Solutions And Mixtures: Definition & Examples - StudySmarter

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Solutions and Mixtures

Solutions and Mixtures

What do maple syrup, saltwater, and a bowl containing cereal and milk have in common? There are different types of solutions and mixtures! These two are very similar expressions, but it can be important to understand the subtle differences between them. Let's take a closer look at Solutions and Mixtures!

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Dilution is the process of adding more solvent to a fixed amount of solute, increasing volume, and _____ the concentration of the solution.

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________ have a high amount of solute in the solution.

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________ are solutions that have less than the maximum amount of solute that can be dissolved in the solvent.

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Saturated solutions are solutions that have the ______ amount of solute dissolved.

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_______ are solutions that contain more than the maximum amount of solute that can be dissolved in the solvent

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Properties of solutions:

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Properties of Mixtures:

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A ______ is referred to as a homogeneous mixture that has a uniform composition

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True or false: A pure substance is referred to an element or compound that has a definite composition and distinct chemical properties.

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_____ can be considered pure substances, ______ cannot.

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A _____ is referred to as a heterogeneous mixture.

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Dilution is the process of adding more solvent to a fixed amount of solute, increasing volume, and _____ the concentration of the solution.

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________ have a high amount of solute in the solution.

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________ are solutions that have less than the maximum amount of solute that can be dissolved in the solvent.

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Saturated solutions are solutions that have the ______ amount of solute dissolved.

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_______ are solutions that contain more than the maximum amount of solute that can be dissolved in the solvent

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Properties of solutions:

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Properties of Mixtures:

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A ______ is referred to as a homogeneous mixture that has a uniform composition

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True or false: A pure substance is referred to an element or compound that has a definite composition and distinct chemical properties.

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_____ can be considered pure substances, ______ cannot.

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A _____ is referred to as a heterogeneous mixture.

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Last Updated: 30.11.2022
Published at: 16.05.2022
11 min reading time

Chemical Analysis
Chemical Reactions
Chemistry Branches
Inorganic Chemistry
Ionic and Molecular Compounds
Kinetics
Making Measurements
Nuclear Chemistry
Organic Chemistry
Physical Chemistry

Absolute Entropy And Entropy Change
Acid Dissociation Constant
Acid-Base Indicators
Acid-Base Reactions and Buffers
Acids and Bases
Alkali Metals
Allotropes of Carbon
Amorphous Polymer
Amount of Substance
Application of Le Chatelier's Principle
Arrhenius Equation
Arrhenius Theory
Atom Economy
Atomic Structure
Autoionization of Water
Avogadro Constant
Avogadro's Number and the Mole
Beer-Lambert Law
Bond Enthalpy
Bonding
Born Haber Cycles
Born-Haber Cycles Calculations
Boyle's Law
Brønsted-Lowry Acids and Bases
Buffer Capacity
Buffer Solutions
Buffers
Buffers Preparation
Calculating Enthalpy Change
Calculating Equilibrium Constant
Calorimetry
Carbon Structures
Cell Potential
Cell Potential and Free Energy
Chalcogens
Chemical Calculations
Chemical Equations
Chemical Equilibrium
Chemical Thermodynamics
Closed Systems
Colligative Properties
Collision Theory
Common-Ion Effect
Composite Materials
Composition of Mixture
Constant Pressure Calorimetry
Constant Volume Calorimetry
Coordination Compounds
Coupling Reactions
Covalent Bond
Covalent Network Solid
Crystalline Polymer
De Broglie Wavelength
Determining Rate Constant
Deviation From Ideal Gas Law
Diagonal Relationship
Diamond
Dilution
Dipole Chemistry
Dipole Moment
Dissociation Constant
Distillation
Dynamic Equilibrium
Electric Fields Chemistry
Electrochemical Cell
Electrochemical Series
Electrochemistry
Electrode Potential
Electrolysis
Electrolytes
Electromagnetic Spectrum
Electron Affinity
Electron Configuration
Electron Shells
Electronegativity
Electronic Transitions
Elemental Analysis
Elemental Composition of Pure Substances
Empirical and Molecular Formula
Endothermic and Exothermic Processes
Energetics
Energy Diagrams
Enthalpy Changes
Enthalpy For Phase Changes
Enthalpy of Formation
Enthalpy of Reaction
Enthalpy of Solution and Hydration
Entropy
Entropy Change
Equilibrium Concentrations
Equilibrium Constant Kp
Equilibrium Constants
Examples of Covalent Bonding
Factors Affecting Reaction Rates
Finding Ka
Free Energy
Free Energy Of Dissolution
Free Energy and Equilibrium
Free Energy of Formation
Fullerenes
Fundamental Particles
Galvanic and Electrolytic Cells
Gas Constant
Gas Solubility
Gay Lussacs Law
Giant Covalent Structures
Graham's Law
Graphite
Ground State
Group 3A
Group 4A
Group 5A
Half Equations
Heating Curve for Water
Heisenberg Uncertainty Principle
Henderson-Hasselbalch Equation
Hess' Law
Hybrid Orbitals
Hydrogen Bonds
Ideal Gas Law
Ideal and Real Gases
Intermolecular Forces
Introduction to Acids and Bases
Ion And Atom Photoelectron Spectroscopy
Ion dipole Forces
Ionic Bonding
Ionic Product of Water
Ionic Solids
Ionisation Energy
Ions: Anions and Cations
Isotopes
Kinetic Molecular Theory
Lattice Structures
Law of Definite Proportions
Le Chatelier's Principle
Lewis Acid and Bases
London Dispersion Forces
Magnitude Of Equilibrium Constant
Mass Spectrometry
Mass Spectrometry of Elements
Maxwell-Boltzmann Distribution
Measuring EMF
Mechanisms of Chemical Bonding
Melting and Boiling Point
Metallic Bonding
Metallic Solids
Metals Non-Metals and Metalloids
Mixtures and Solutions
Molar Mass Calculations
Molarity
Molecular Orbital Theory
Molecular Solid
Molecular Structures of Acids and Bases
Moles and Molar Mass
Nanoparticles
Neutralisation Reaction
Oxidation Number
Partial Pressure
Particulate Model
Partition Coefficient
Percentage Yield
Periodic Table Organization
Phase Changes
Phase Diagram of Water
Photoelectric Effect
Photoelectron Spectroscopy
Physical Properties
Polarity
Polyatomic Ions
Polyprotic Acid Titration
Prediction of Element Properties Based on Periodic Trends
Pressure and Density
Properties Of Equilibrium Constant
Properties of Buffers
Properties of Solids
Properties of Water
Quantitative Electrolysis
Quantum Energy
Quantum Numbers
RICE Tables
Rate Equations
Rate of Reaction and Temperature
Reacting Masses
Reaction Quotient
Reaction Quotient And Le Chateliers Principle
Real Gas
Redox
Relative Atomic Mass
Representations of Equilibrium
Reversible Reaction
SI units chemistry
Saturated Unsaturated and Supersaturated
Shapes of Molecules
Shielding Effect
Simple Molecules
Solids Liquids and Gases
Solubility
Solubility Curve
Solubility Equilibria
Solubility Product
Solubility Product Calculations
Solutes Solvents and Solutions
Solution Representations
Solutions and Mixtures
Specific Heat
Spectroscopy
Standard Potential
States of Matter
Stoichiometry In Reactions
Strength of Intermolecular Forces
The Laws of Thermodynamics
The Molar Volume of a Gas
Thermodynamically Favored
Trends in Ionic Charge
Trends in Ionisation Energy
Types of Mixtures
VSEPR Theory
Valence Electrons
Van der Waals Forces
Vapor Pressure
Water in Chemical Reactions
Wave Mechanical Model
Weak Acid and Base Equilibria
Weak Acids and Bases
Writing Chemical Formulae
pH
pH Change
pH Curves and Titrations
pH Scale
pH and Solubility
pH and pKa
pH and pOH

The Earths Atmosphere

Contents

Chemical Analysis
Chemical Reactions
Chemistry Branches
Inorganic Chemistry
Ionic and Molecular Compounds
Kinetics
Making Measurements
Nuclear Chemistry
Organic Chemistry
Physical Chemistry

Absolute Entropy And Entropy Change
Acid Dissociation Constant
Acid-Base Indicators
Acid-Base Reactions and Buffers
Acids and Bases
Alkali Metals
Allotropes of Carbon
Amorphous Polymer
Amount of Substance
Application of Le Chatelier's Principle
Arrhenius Equation
Arrhenius Theory
Atom Economy
Atomic Structure
Autoionization of Water
Avogadro Constant
Avogadro's Number and the Mole
Beer-Lambert Law
Bond Enthalpy
Bonding
Born Haber Cycles
Born-Haber Cycles Calculations
Boyle's Law
Brønsted-Lowry Acids and Bases
Buffer Capacity
Buffer Solutions
Buffers
Buffers Preparation
Calculating Enthalpy Change
Calculating Equilibrium Constant
Calorimetry
Carbon Structures
Cell Potential
Cell Potential and Free Energy
Chalcogens
Chemical Calculations
Chemical Equations
Chemical Equilibrium
Chemical Thermodynamics
Closed Systems
Colligative Properties
Collision Theory
Common-Ion Effect
Composite Materials
Composition of Mixture
Constant Pressure Calorimetry
Constant Volume Calorimetry
Coordination Compounds
Coupling Reactions
Covalent Bond
Covalent Network Solid
Crystalline Polymer
De Broglie Wavelength
Determining Rate Constant
Deviation From Ideal Gas Law
Diagonal Relationship
Diamond
Dilution
Dipole Chemistry
Dipole Moment
Dissociation Constant
Distillation
Dynamic Equilibrium
Electric Fields Chemistry
Electrochemical Cell
Electrochemical Series
Electrochemistry
Electrode Potential
Electrolysis
Electrolytes
Electromagnetic Spectrum
Electron Affinity
Electron Configuration
Electron Shells
Electronegativity
Electronic Transitions
Elemental Analysis
Elemental Composition of Pure Substances
Empirical and Molecular Formula
Endothermic and Exothermic Processes
Energetics
Energy Diagrams
Enthalpy Changes
Enthalpy For Phase Changes
Enthalpy of Formation
Enthalpy of Reaction
Enthalpy of Solution and Hydration
Entropy
Entropy Change
Equilibrium Concentrations
Equilibrium Constant Kp
Equilibrium Constants
Examples of Covalent Bonding
Factors Affecting Reaction Rates
Finding Ka
Free Energy
Free Energy Of Dissolution
Free Energy and Equilibrium
Free Energy of Formation
Fullerenes
Fundamental Particles
Galvanic and Electrolytic Cells
Gas Constant
Gas Solubility
Gay Lussacs Law
Giant Covalent Structures
Graham's Law
Graphite
Ground State
Group 3A
Group 4A
Group 5A
Half Equations
Heating Curve for Water
Heisenberg Uncertainty Principle
Henderson-Hasselbalch Equation
Hess' Law
Hybrid Orbitals
Hydrogen Bonds
Ideal Gas Law
Ideal and Real Gases
Intermolecular Forces
Introduction to Acids and Bases
Ion And Atom Photoelectron Spectroscopy
Ion dipole Forces
Ionic Bonding
Ionic Product of Water
Ionic Solids
Ionisation Energy
Ions: Anions and Cations
Isotopes
Kinetic Molecular Theory
Lattice Structures
Law of Definite Proportions
Le Chatelier's Principle
Lewis Acid and Bases
London Dispersion Forces
Magnitude Of Equilibrium Constant
Mass Spectrometry
Mass Spectrometry of Elements
Maxwell-Boltzmann Distribution
Measuring EMF
Mechanisms of Chemical Bonding
Melting and Boiling Point
Metallic Bonding
Metallic Solids
Metals Non-Metals and Metalloids
Mixtures and Solutions
Molar Mass Calculations
Molarity
Molecular Orbital Theory
Molecular Solid
Molecular Structures of Acids and Bases
Moles and Molar Mass
Nanoparticles
Neutralisation Reaction
Oxidation Number
Partial Pressure
Particulate Model
Partition Coefficient
Percentage Yield
Periodic Table Organization
Phase Changes
Phase Diagram of Water
Photoelectric Effect
Photoelectron Spectroscopy
Physical Properties
Polarity
Polyatomic Ions
Polyprotic Acid Titration
Prediction of Element Properties Based on Periodic Trends
Pressure and Density
Properties Of Equilibrium Constant
Properties of Buffers
Properties of Solids
Properties of Water
Quantitative Electrolysis
Quantum Energy
Quantum Numbers
RICE Tables
Rate Equations
Rate of Reaction and Temperature
Reacting Masses
Reaction Quotient
Reaction Quotient And Le Chateliers Principle
Real Gas
Redox
Relative Atomic Mass
Representations of Equilibrium
Reversible Reaction
SI units chemistry
Saturated Unsaturated and Supersaturated
Shapes of Molecules
Shielding Effect
Simple Molecules
Solids Liquids and Gases
Solubility
Solubility Curve
Solubility Equilibria
Solubility Product
Solubility Product Calculations
Solutes Solvents and Solutions
Solution Representations
Solutions and Mixtures
Specific Heat
Spectroscopy
Standard Potential
States of Matter
Stoichiometry In Reactions
Strength of Intermolecular Forces
The Laws of Thermodynamics
The Molar Volume of a Gas
Thermodynamically Favored
Trends in Ionic Charge
Trends in Ionisation Energy
Types of Mixtures
VSEPR Theory
Valence Electrons
Van der Waals Forces
Vapor Pressure
Water in Chemical Reactions
Wave Mechanical Model
Weak Acid and Base Equilibria
Weak Acids and Bases
Writing Chemical Formulae
pH
pH Change
pH Curves and Titrations
pH Scale
pH and Solubility
pH and pKa
pH and pOH

The Earths Atmosphere

Contents

Fact Checked Content
Last Updated: 30.11.2022
11 min reading time

Content creation process designed by Lily Hulatt
Content sources cross-checked by Gabriel Freitas
Content quality checked by Gabriel Freitas

Jump to a key chapter

First, we will talk about the difference between a mixture and a solution.
Then, we will look at the different types of mixtures and solutions.
Next, we will learn about their properties.
Lastly, we will talk about the meaning of pure substances.

Difference between a mixture and a solution

For your AP chemistry exam, you should know the following definitions regarding solutions and mixtures.

A solution is a mixture in which all the particles are evenly mixed. Solutions are considered homogeneous mixtures, and they can involve solids, liquids, and gases.

A solution is composed of a solute and a solvent. A solute is a substance that gets dissolved in a solvent. A solvent is a medium in which the solute gets dissolved. In solutions, the macroscopic properties do not vary throughout the sample.

In summary, a solution is referred to as a homogeneous mixture. Solutions have a uniform composition.

To form a solution, the intermolecular forces present in both the solute and the solvent must be broken, and then new intermolecular forces need to form between them.

Water is considered a universal solvent because of its capability of dissolving many substances! Water is able to dissolve ionic compounds, and also polar covalent compounds. When water dissociates ionic compounds, electrolyte solutions are formed. These solutions are capable of conducting electricity due to the presence of ions in the solution!

When water is used as a solvent, the solution is called an aqueous solution.

A mixture, on the other hand, consists of particles that cannot mix evenly and therefore are considered heterogeneous. In mixtures, the macroscopic properties vary depending on the location in the mixture.

A mixture is referred to as a heterogeneous mixture.

Before diving into the different types of mixtures and solutions, we need to remember the basics of solubility.

In solids, the solubility in water increases with an increase in temperature.
In gases, the solubility in water decreases with an increase in temperature.
Most ionic compounds that have Li+, Na+, K+, NH4+, NO3- or CH3CO2- are considered soluble in water.

The solubility of a solute is referred to as the maximum amount of solute that is able to dissolve in 100 grams of solvent at a given temperature.

Types of solutions and mixtures

Solutions can be formed from any combination of solid, liquid, or gas. In the table below, you can find some examples of solutions!

Examples of solutions

Primary solute	Solvent	Solution
Acetic acid (liquid)	Water (liquid)	Vinegar (liquid-liquid)
Zinc (solid)	Copper (solid)	Brass (solid-solid)
Oxygen (gas)	Nitrogen (gas)	Air (gas-gas)
Sodium chloride (solid)	Water (liquid)	Saltwater (solid-liquid)
Carbon dioxide (gas)	Water (liquid)	Soda water (gas-liquid)

Solutions can be categorized as:

Dilute solutions
Concentrated solutions
Saturated solutions
Supersaturated solutions
Unsaturated solutions

These days a super intensely researched area of chemistry is how to store hydrogen gas efficiently. One of the main problems with green energy production is the need to store this energy. Producing hydrogen from the energy (for example solar) is a very nice approach. However, what do you do with hydrogen? One idea is to dissolve it in metals like Palladium. Yes, that would be gas in a "solid solution". Many other elements are capable of dissolving hydrogen gas inside them these are called interstitial hydrides by the way. This is a very good solution for hydrogen transport but sadly very expensive.

Dilute vs concentration solutions

When you add a cup of concentrated orange juice to a jar containing three cups of water to make orange juice, you are actually making a dilution solution! Dilute solutions are solutions that have a low amount of solute in the solution.

Dilutions are usually performed by chemists to reduce the concentration of solutions. Concentration is a measurement of how much solute is dissolved in the solvent.

Dilution is the process of adding more solvent to a fixed amount of solute, increasing volume, and decreasing the concentration of the solution.

Concentrated solutions are the opposite of dilute solutions and they have a high amount of solute in the solution. Concentrated solutions can be further divided into unsaturated, saturated, and supersaturated solutions.

Did you know that dilute solutions of phenol (carbolic acid) were used in hospitals before as antiseptics to kill infectious microorganisms? Joseph Lister was actually the first person to ever sterilize surgical instruments with phenol and also use phenol to disinfect wounds!

Unsaturated Solutions

Unsaturated solutions are solutions that have less than the maximum amount of solute that can be dissolved in the solvent. So, if you decided to add more solute to an unsaturated solution, the solute would dissolve without a problem, leaving no traces of the solute!

For example, if you added salt to a cup of water and the salt completely dissolves, then you have an unsaturated solution.

Saturated solutions

Saturated solutions are solutions that have the maximum amount of solute dissolved. In other words, if you added more solute to it, the solute would not dissolve. Instead, it would sink to the bottom of the solution.

When a solution becomes saturated, it means that the rate at which the solute dissolves in the solvent is equal to the rate at which the saturated solution is formed. This is called crystallization.

Solutions and Mixtures Recrystallization Saturated Solutions StudySmarter Fig.1-Crystallization

Think about a time when you added sugar to your coffee or tea, and it got to a point where the sugar stopped dissolving. This is an example of a saturated solution!

If you mix two substances and they do not dissolve in one another (mixing oil and water or mixing salt and pepper), a saturated solution cannot be formed.

Supersaturated solutions

Supersaturated solutions are solutions that contain more than the maximum amount of solute that can be dissolved in the solvent. Supersaturated solutions are formed when a saturated solution gets heated to a high temperature and then more solute is added to it. When the solution cools down, no precipitate is formed.

Solutions and Mixtures Supersaturated Solution StudySmarter Fig.2-Formation of a supersaturated solution

Supersaturated solutions don't always have to be heated in order to be formed. Honey is a supersaturated solution made from more than 70% sugar added to very low water content. Supersaturated solutions are unstable and, as seen in honey, will crystallize over time to form a stable saturated solution.

Now, let's look at the different types of mixtures! Mixtures can be homogeneous and heterogeneous.

However, when dealing with AP exams, mixtures are the term used to refer to heterogeneous mixtures only! To make things simpler, let's focus on what heterogeneous mixtures are.

Heterogeneous Mixtures

When a mixture contains substances that are not uniform in composition, we give it the name heterogeneous mixture. This type of mixture can be separated by physical means. Your favorite pizza is a type of heterogeneous mixture!

Suspensions are a type of heterogeneous mixture. In order to mix the substances found in a suspension, an outside force is needed. But, after a while, the substances will separate again. A common example of a suspension is salad dressing, made up of oil and vinegar.

Try mixing oil and vinegar at home and watch how the two substances separate: oil on top and vinegar on the bottom!

Now that we learned about what mixtures and solutions are, and the types that exist, let's focus on the properties of mixtures and solutions!

Properties of Mixtures and Solutions

Solutions are a type of homogenous mixture consisting of particles with very small diameters that completely dissolve in the solution and cannot be seen with the naked eye. They are not capable of scattering beams of light, and they cannot be separated by filtration. Solutes are also stable at a given temperature.

Mixtures, on the other hand, are heterogeneous mixtures consisting of particles that can be separated. Mixtures do not have a uniform composition and the different parts may be seen with the naked eye. Mixtures are able to scatter light.

Molarity (Molar Concentration)

We can express the composition of a solution by using molarity. Molarity is the concentration of the solute.

Molarity, which is also known as molar concentration, indicates the number of moles of a solute in 1 L of solution.

The equation for molarity is as follows:

Molarity (M) = nsoluteLsolution

Let's look at an example!

How many moles of MgSO4 is found in 0.15 L of a 5.00 M solution?

The questions give us molarity and liters of solution. So, all we have to do is rearrange the equation and solve for moles of MgSO4.

nsolute = M × Lsolutionnsolute = 5.00 M × 0.15 L = 0.75 mol MgSO4

Dilution Calculation involving Molarity

We stated before that when more solvent is added to a sample, it becomes less concentrated (diluted). The dilution equation is:

M1V1 = M2V2

Where,

M1 is the molarity before dilution
M2 is the molarity after dilution
V1 is the volume of solution before dilution (in L)
V2is the volume of solution after dilution (in L)

Find the molarity of 0.07 L of a 4.00 M KCl solution when diluted to a volume of 0.3 L.

Notice that the question gives us M1, V1, and V2. So, we need to solve for M2 using the dilution equation above.

4.00 M × 0.07 L = M2 × 0.3 LM2 = 4.00 M × 0.07 L0.3 L = 0.9 M

Pure substances mixture and solution

Pure water is made up of hydrogen and oxygen molecules, and it is considered a pure substance. Some examples of pure substances include Iron, NaCl (table salt), sugar (sucrose), and ethanol.

A pure substance is referred to an element or compound that has a definite composition and distinct chemical properties.

If a solution has a constant composition, then it can also be considered a type of pure substance. For example, a solution containing salt dissolved in water is a pure substance because the composition of the solution stays the same throughout.

Mixtures (heterogeneous mixtures) are not considered pure substances due to the differences in composition.

Some substances are considered a gray area in terms of whether they are pure substances or not. Substances in this category as usually those that do not have a chemical formula, like milk, air, honey, and even coffee!

After reading this, I hope that you feel more confident about the difference between solutions and mixtures, and ready to tackle any problem that comes your way!

Solutions and Mixtures - Key takeaways

A solution is referred to as a homogeneous mixture composed of solute and solvent.
A mixture is referred to as a heterogeneous mixture, also composed of solute and solvent.
Solutions can be categorized as dilute, concentrated, unsaturated, saturated, and supersaturated.
A pure substance is referred to an element or compound that has a definite composition and distinct chemical properties. Solutions can be pure substances, mixtures cannot.

References

Brown, T. L. (2009). Chemistry: The Central Science. Pearson Education.
The Princeton Review. (2019). Cracking the AP Chemistry Exam 2020. Princeton Review.
AP Chemistry course and exam description ... - AP central. (n.d.). Retrieved April 29, 2022, from https://apcentral.collegeboard.org/pdf/ap-chemistry-course-and-exam-description.pdf?course=ap-chemistry
Swanson, J. W. (2020). Everything you need to Ace Chemistry in one big fat notebook. Workman Pub.
Timberlake, K. C., & Orgill, M. (2020). General, organic, and Biological Chemistry: Structures Of Life. Upper Saddle River: Pearson.

Flashcards in Solutions and Mixtures

20 Start learning

Dilution is the process of adding more solvent to a fixed amount of solute, increasing volume, and _____ the concentration of the solution.

decreasing

________ have a high amount of solute in the solution.

Concentrated solutions

________ are solutions that have less than the maximum amount of solute that can be dissolved in the solvent.

Unsaturated solutions

Saturated solutions are solutions that have the ______ amount of solute dissolved.

maximum

_______ are solutions that contain more than the maximum amount of solute that can be dissolved in the solvent

Supersaturated solutions

Properties of solutions:

They are homogenous mixtures

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Frequently Asked Questions about Solutions and Mixtures

What is the difference between a mixture and a solution?

A solution is a homogeneous mixture, while a mixture is a heterogeneous mixture.

What are mixtures and solutions?

Solutions are homogeneous mixtures, meaning that the solute completely dissolves in the solution/no different layers are formed. Mixtures are heterogeneous mixtures, so the solute does not mix with the solvent.

What are the types of mixtures?

Mixtures are referred to as heterogeneous mixtures or mixtures that do not have a uniform composition and separate into different regions/layers.

How to separate mixtures and solutions?

Solution and mixtures can be separated in various ways, including evaporation, filtration, distillation, and chromatography.

What are examples of the various types of mixtures?

Examples of mixtures include sand and water, salad dressing (oil-and-vinegar suspension), cereal in milk, and chocolate chip cookies.

Save Article Test your knowledge with multiple choice flashcards

Dilution is the process of adding more solvent to a fixed amount of solute, increasing volume, and _____ the concentration of the solution.

A. increasing B. decreasing

________ have a high amount of solute in the solution.

A. Dilute solutions B. Concentrated solutions

________ are solutions that have less than the maximum amount of solute that can be dissolved in the solvent.

A. Supersaturated Solutions B. Unsaturated solutions C. Saturated Solutions

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Tag » What Are Examples Of Solutions

Solutions And Mixtures: Definition & Examples - StudySmarter

Difference between a mixture and a solution

Types of solutions and mixtures

Examples of solutions

Dilute vs concentration solutions

Unsaturated Solutions

Saturated solutions

Supersaturated solutions

Heterogeneous Mixtures

Properties of Mixtures and Solutions

Molarity (Molar Concentration)

Dilution Calculation involving Molarity

Pure substances mixture and solution

Solutions and Mixtures - Key takeaways

References

Similar topics in Chemistry

Related topics to Physical Chemistry

Flashcards in Solutions and Mixtures

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Frequently Asked Questions about Solutions and Mixtures

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