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Mixtures vs. solutions vs. suspensions.
mixture is a combination of substances which are not chemically joined together.
Mixtures have the same properties as their components
There is no fixed proportion between the components
The components can be separated from the mixture
sugar and salt
air with nitrogen and oxygen
is a solution homogeneous mixture in which one substance (solute) is dissolved in another substance (solvent).
The components in a solution may
not be separated from the solution by leaving it to stand, or by filtration
If a material dissolves in a liquid the material is said to be
soluble. A solution is saturated if no more solute can be dissolved with temperature remaining constant. Examples
suspension is a mixture of liquids with particles of a solid which may not dissolve in the liquid.
The solid may be separated from the liquid by leaving it to stand, or by filtration
The SI-system, unit converters, physical constants, drawing scales and more.
The study of fluids - liquids and gases. Involving velocity, pressure, density and temperature as functions of space and time.
Calculator and formulas for conversion between different units of concentration: Molarity, molality, mole fraction, weight percent of solute and grams of solute per liter of solution - descriptive terms for solubility.
Guidelines or solubility rules to predict whether or not a given ionic compound is soluble in water at room temperature.
It is possible to estimate the density of a liquid-liquid solution from the density of the solute and the solvent. However, due to shrinkage, the estimate will be a bit too low.
Final mass and temperature when mixing fluids.
Rules for naming inorganic ionic and covalent types of chemical compounds.
The amount of a solute that can be dissolved in a solvent.
The equilibrium constant, Ksp, for aqueous solutions of ionic compounds at 25°C.
Definitions and examples of how to calculate wt%, molarity and how to prepare dilutions.
Dynamic viscosities of sucrose water solutions vs. temperature.
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