Dissolution, Electrolytes, and Solubility
The Dissolution Process
A solution forms when two or more substances combine physically to yield a mixture that is homogeneous at the
molecular level. The solvent is the most concentrated component and determines the physical state of the solution.
The solutes are the other components typically present at concentrations less than that of the solvent. Solutions may
form endothermically or exothermically, depending upon the relative magnitudes of solute and solvent intermolecular
attractive forces. Ideal solutions form with no appreciable change in energy.
Electrolytes
Substances that dissolve in water to yield ions are called electrolytes. Electrolytes may be covalent compounds
that chemically react with water to produce ions (for example, acids and bases), or they may be ionic compounds
that dissociate to yield their constituent cations and anions, when dissolved. Dissolution of an ionic compound is
facilitated by ion-dipole attractions between the ions of the compound and the polar water molecules. Soluble ionic
substances and strong acids ionize completely and are strong electrolytes, while weak acids and bases ionize to only
a small extent and are weak electrolytes. Nonelectrolytes are substances that do not produce ions when dissolved in
water.
(From Chemistry by OpenStax - Download for free at http://cnx.org/content/col11760/latest/)
A solution forms when two or more substances combine physically to yield a mixture that is homogeneous at the
molecular level. The solvent is the most concentrated component and determines the physical state of the solution.
The solutes are the other components typically present at concentrations less than that of the solvent. Solutions may
form endothermically or exothermically, depending upon the relative magnitudes of solute and solvent intermolecular
attractive forces. Ideal solutions form with no appreciable change in energy.
Electrolytes
Substances that dissolve in water to yield ions are called electrolytes. Electrolytes may be covalent compounds
that chemically react with water to produce ions (for example, acids and bases), or they may be ionic compounds
that dissociate to yield their constituent cations and anions, when dissolved. Dissolution of an ionic compound is
facilitated by ion-dipole attractions between the ions of the compound and the polar water molecules. Soluble ionic
substances and strong acids ionize completely and are strong electrolytes, while weak acids and bases ionize to only
a small extent and are weak electrolytes. Nonelectrolytes are substances that do not produce ions when dissolved in
water.
(From Chemistry by OpenStax - Download for free at http://cnx.org/content/col11760/latest/)
Text Resources
Properties of Solutes in Aqueous Solutions CHM1046 Tutorials by Dr. Michael Blaber at Florida State
Acids, Bases and Salts CHM1046 Tutorials by Dr. Michael Blaber at Florida State
Videos
What Happens when Stuff Dissolves? Tyler DeWitt [4:09]
We'll look at what happens when you dissolve ionic and covalent compounds in water. Ionic compounds break apart into the ions that make them up, a process called dissociation, while covalent compounds only break into the molecules, not the individual atoms.
Biggest Mistakes in Chemistry: Dissolving Tyler DeWitt [4:10
What is a Solution? Ben's Chem Videos [7:31]
Review of making solutions.
Electrolytes Ben's Chem Videos [10:37]
Definition of an electrolyte, plus the three dissolution processes--molecular dissolution, ionic dissolution, and molecular ionization--that give rise to strong electrolytes, weak electrolytes, and nonelectrolytes.
Solutions, Acids, and Bases Chemistry Matters video playlist by Georgia Public Broadcasting
Solutions web-based tutorials for GenChem at The University of Texas
Solutions Bozeman Science [9:46] with Concept Map
Chemistry of Solutions Unit 9 playlist by IsaacsTEACH
Suggested Videos:
Properties of Solutes in Aqueous Solutions CHM1046 Tutorials by Dr. Michael Blaber at Florida State
Acids, Bases and Salts CHM1046 Tutorials by Dr. Michael Blaber at Florida State
Videos
What Happens when Stuff Dissolves? Tyler DeWitt [4:09]
We'll look at what happens when you dissolve ionic and covalent compounds in water. Ionic compounds break apart into the ions that make them up, a process called dissociation, while covalent compounds only break into the molecules, not the individual atoms.
Biggest Mistakes in Chemistry: Dissolving Tyler DeWitt [4:10
What is a Solution? Ben's Chem Videos [7:31]
Review of making solutions.
Electrolytes Ben's Chem Videos [10:37]
Definition of an electrolyte, plus the three dissolution processes--molecular dissolution, ionic dissolution, and molecular ionization--that give rise to strong electrolytes, weak electrolytes, and nonelectrolytes.
Solutions, Acids, and Bases Chemistry Matters video playlist by Georgia Public Broadcasting
Solutions web-based tutorials for GenChem at The University of Texas
Solutions Bozeman Science [9:46] with Concept Map
Chemistry of Solutions Unit 9 playlist by IsaacsTEACH
Suggested Videos:
- Chemistry 9.1 Properties of Water from Hydrogen Bonding
- Chemistry 9.2 What are Electrolytes?
- Chemistry 9.2b More on Electrolytes
Solubility
The extent to which one substance will dissolve in another is determined by several factors, including the types
and relative strengths of intermolecular attractive forces that may exist between the substances’ atoms, ions, or
molecules. This tendency to dissolve is quantified as substance’s solubility, its maximum concentration in a solution
at equilibrium under specified conditions. A saturated solution contains solute at a concentration equal to its solubility.
A supersaturated solution is one in which a solute’s concentration exceeds its solubility—a nonequilibrium (unstable)
condition that will result in solute precipitation when the solution is appropriately perturbed. Miscible liquids are
soluble in all proportions, and immiscible liquids exhibit very low mutual solubility. Solubilities for gaseous solutes
decrease with increasing temperature, while those for most, but not all, solid solutes increase with temperature. The
concentration of a gaseous solute in a solution is proportional to the partial pressure of the gas to which the solution
is exposed, a relation known as Henry’s law.
(From Chemistry by OpenStax - Download for free at http://cnx.org/content/col11760/latest/)
Tutorials in Chem1 General Chemistry Virtual Textbook by Dr. Lower
Factors Affecting Solubility CHM1046 Tutorials by Dr. Michael Blaber at Florida State
Video
Polar & Non-Polar Molecules: Crash Course Chemistry #23 CrashCourse Chemistry [10:45]
Chemistry of Solutions Unit 9 playlist by IsaacsTEACH
Suggested Video:
Properties of Solutions: Part 2 of 11 Mike Christiansen [9:54]
In this video I’ll talk about how solutions form. I’ll explain further how to determine if a solute is miscible or immiscible in a particular solvent; I’ll introduce you to crystallization of saturated solutions; and I’ll introduce you to Henry’s Law, which allows us to interrelate the concentration of a gas in solution to its pressure.
The extent to which one substance will dissolve in another is determined by several factors, including the types
and relative strengths of intermolecular attractive forces that may exist between the substances’ atoms, ions, or
molecules. This tendency to dissolve is quantified as substance’s solubility, its maximum concentration in a solution
at equilibrium under specified conditions. A saturated solution contains solute at a concentration equal to its solubility.
A supersaturated solution is one in which a solute’s concentration exceeds its solubility—a nonequilibrium (unstable)
condition that will result in solute precipitation when the solution is appropriately perturbed. Miscible liquids are
soluble in all proportions, and immiscible liquids exhibit very low mutual solubility. Solubilities for gaseous solutes
decrease with increasing temperature, while those for most, but not all, solid solutes increase with temperature. The
concentration of a gaseous solute in a solution is proportional to the partial pressure of the gas to which the solution
is exposed, a relation known as Henry’s law.
(From Chemistry by OpenStax - Download for free at http://cnx.org/content/col11760/latest/)
Tutorials in Chem1 General Chemistry Virtual Textbook by Dr. Lower
- Solubility: the dissolution of salts in water
- Solutions of gases in liquids
- Solubility of gases in water
- Solubility of gases increases with pressure: Henry's Law
- The Solution Process
Factors Affecting Solubility CHM1046 Tutorials by Dr. Michael Blaber at Florida State
Video
Polar & Non-Polar Molecules: Crash Course Chemistry #23 CrashCourse Chemistry [10:45]
Chemistry of Solutions Unit 9 playlist by IsaacsTEACH
Suggested Video:
- Chemistry 9.5a Dissolving Solids and Liquids
Properties of Solutions: Part 2 of 11 Mike Christiansen [9:54]
In this video I’ll talk about how solutions form. I’ll explain further how to determine if a solute is miscible or immiscible in a particular solvent; I’ll introduce you to crystallization of saturated solutions; and I’ll introduce you to Henry’s Law, which allows us to interrelate the concentration of a gas in solution to its pressure.