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Alberta Chemistry 20
Chemistry 20 AP
Unit 4: Solutions
Definitions
Dissociation |
when highly soluble ionic compounds break apart/dissociate into their components in solutions |
Dissolving |
when the substance doesn't break apart into its components |
Ionization |
the process by which an atom or molecule acquires a charge by gaining or losing electrons |
Electrolyte |
the aqueous solution conducts electricity, highly soluble ionic hydroxides (bases) and acids (molecular) |
Non-Electrolyte |
the aqueous solutions doesn't conduct electricity, most molecular compounds (except acids) |
Bonds & Energy
Breaking bonds absorbs energy & forming new bonds releases energy |
Energy is absorbed to break ionic bonds and overcome the intermolecular forces among the water molecules |
Energy is released to form bonds between water and ions |
Types of Concentration
Percent volume by volume (%V/V) |
generally when a liquid is dissolved in a liquid |
Percent weight by volume (%W/V) |
generally when a solid is dissolved in a liquid |
Percent weight by weight (%W/W) |
generally a solid in solid |
Parts per million (ppm) |
1ppm = 1mg/kg (for dilute aqueous solutions, 1ppm = 1mg/1L) |
Amount concentration (M) |
moles/L |
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Ion Concentration
The dissociation or ionization equations for compounds allows you to determine the amount concentration of either the ions or the compounds in solution |
The ion concentration is always equal to a whole number multiple of the compound concentration (the coefficient in the chemical equation) |
Solubility
Saturated: maximum amount of solute dissolved in a solvent as a specific temperature |
Unsaturated: solution can dissolve more solute |
Super Saturated: can dissolve more with an increase in temperature |
Solubility Variables of Gases
Temperature |
as temperature increases, the solubility of a gas decreases |
Pressure |
the solubility of a gas increases as the partial pressure of the gas above a solution increase |
Solubility Variables of Liquids & Solids
Temperature |
solubility increases with temperature |
Pressure |
very little effect on the solubility of liquids and gases |
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Techniques to Separate Solutions
Chromatography: a technique that can be used to separate out, most commonly, different coloured solutes (pigments) in a solutions |
Distillation: a technique use to separate solutions of 2 or more liquids by using their differential boiling points |
Fractional Distillation: when multiple liquids (fractions) are mixed in a solution or the boiling points are very similar, they use many different condensation plates to condense and re-vaporize to allow a more pure solution to rise through the column |
Dynamic Equilibrium
Dynamic Equilibrium: both dissolving and crystallizing out of solution are occurring at the same rate which maintains a balance in the solution
Beer-Lambert Law
Beer-Lambert Law: a linear relationship between the absorbance and the concentration, molar absorption coefficient and optical coefficient of a solution
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