Madison Boss
Chapter 15 Review
Solutions
Solution- a homogenous mixture
Solvent- substance that is in the larger amount
Solute- substances that are in lesser amounts
Aqueous Solutions- solutions where water is the solvent
15.1

Polar compounds dissolve in water because the polar bonds attract the water
molecules

Ionic compounds dissolve in water because they break apart into a positively
charged ion and a negatively charged ion when put into water (NaCl)

When the electronegativity of the atoms in a molecule are similar this leads
to the electrons being evenly shared and the molecule does not dissolve in
water (these molecules are considered non-polar)

Substances dissolve when they have similar polarities

In order for a molecule to dissolve, the atoms of that molecule must bond
with the water molecules
15.2
Saturated- solution that contains as much solute as will dissolve at a given
temperature
Unsaturated- a solution that has not reached the limit of solute that will dissolve
Supersaturated- a solution that contains more solute than will dissolve at that
temperature (heating and then cooling of the solution is required)
Concentrated- a relatively large amount of solute is dissolved (strong coffee)
Dilute- a relatively small amount of solute is dissolved (weak coffee)

There is always a limit to how much of a solute can be dissolved in a solvent
15.3

There are three factors that affect the rate at which something dissolves
Madison Boss
Chapter 15 Review
1. Surface area- the greater amount of surface area of the solid being
dissolved that is exposed to the solvent, the greater rate at which
dissolution (dissolving) takes place
2. Stirring- stirring causes newly dissolved particles to be moved away from
the surface of the solid which allows the solid surface area to always be
exposed to the solvent
3. Temperature- increase in temperature causes the solvent molecules to
move much faster and this increases the dissolving process (tea dissolves
much faster in hot water then it does in cold water)

Higher temperatures usually also cause substances to become more soluble
(increased saturation point)
15.4
Mass Percent- a solutions composition (how much mass of solute is there for how
much mass of solution)

Mass percent= (the mass of solute) / (mass of solution) x 100
*Mass of solution= sum of the masses of solute and solvent
15.5
Molarity (M)- expression of concentration
Standard Solution- a solution whose concentration is accurately known

M= (moles of solute) / (liters of solution)

Be careful to convert units of solution into liters (usually expressed as ml)
15.6
Dilution- the process of adding more solvent to a solution

Solutions are often purchased or prepared in concentrated form (stock
solution). This allows you to create any concentration of the solution by
adding measured quantities of water (or other solvent)
Madison Boss

Chapter 15 Review
M1 (molarity before dilution) x V1 (volume before dilution) =
M2 (molarity after dilution) x V2 (volume after dilution)
15.7
Steps
1. Write the balanced equation. For reactions involving ions, write the
net ionic equation.
2. Calculate the moles of reactants
3. Determine which reactant is the limiting reagent
4. Calculate the moles of other reactants or products, as required
5. Convert to grams or other units
15.8
Neutralizing Reaction- when the same moles of base are added to the same
moles of acid.

As in all acid-base reactions, an H+ from the acid and the OH- form the
base are synthesized to form H2O
15.9
Equivalent of an acid- the amount of that acid that can furnish 1 mole of H+
Equivalent of a base- the amount of that base that can furnish 1 mole of OHEquivalent weight- the mass in grams of 1 equivalent of an acid or a base
Normality- the number of equivalents of solute per liter of solution

Equivalent (acid) = Equivalent (base) in a neutralizing reaction
15.10
Colligative Property- a solution property that depends on the number of solute
particles present.

Solutes can change the properties of the solvent (salt in water causes the
water to boil faster)