There are several terms used
to describe solutions and their properties. Here are some of the most common terms:
Solvent
The substance that dissolves
the solute, typically the liquid component of a solution.
Solute
The substance that is
dissolved in the solvent to form a solution.
Solution
A homogeneous mixture of a
solvent and one or more solutes.
Concentration
The amount of solute
dissolved in a given amount of solvent or solution, usually expressed as
mass/volume, molarity, or molality.
Solubility
The maximum amount of solute
that can be dissolved in a given amount of solvent at a specific temperature and
pressure.
Saturation
The state of a solution in
which no more solute can be dissolved in the solvent at a given temperature and
pressure.
Molar
Solution
A molar solution is a type
of solution where one mole of a solute is dissolved in one liter of solvent. It
is a measure of the concentration of the solute in the solution. The unit of
molarity is moles per liter (mol/L) and is denoted as M. For example, a 1 M
solution of sodium chloride (NaCl) contains one mole of NaCl in one liter of
water.
Molarity
Molarity is a measure of the
concentration of a solute in a solution. It is defined as the number of moles
of solute present in one liter of the solution. The unit of molarity is moles
per liter (mol/L) and is denoted as M. For example, a 0.5 M solution of
sulfuric acid (H2SO4) contains 0.5 moles of H2SO4 in one liter of water.
True
Solution
A true solution is a type of
homogeneous mixture where the solute particles are molecular in size and
uniformly distributed in the solvent. The solute particles are too small to be
seen by the naked eye or even a microscope. The solution is stable, and the
solute does not settle down over time. Examples of true solutions include
saltwater, sugar solution, and alcohol-water mixture.
Colloidal
Solution
A colloidal solution is a
type of heterogeneous mixture where the solute particles are larger than
molecular but smaller than those of a suspension. The solute particles in a
colloidal solution are dispersed throughout the solvent by Brownian motion. The
particles are not visible to the naked eye but can be seen under a microscope.
The solute particles do not settle down over time and are stabilized by
electrostatic forces. Examples of colloidal solutions include milk, blood, and
ink.
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