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Alberta Chemistry 20
Chemistry 20 AP
Unit 4: Solutions
DefinitionsDissociation | 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 & EnergyBreaking 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 ConcentrationPercent 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 |
| | Ion ConcentrationThe 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) |
SolubilitySaturated: 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 GasesTemperature | 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 & SolidsTemperature | solubility increases with temperature | Pressure | very little effect on the solubility of liquids and gases |
| | Techniques to Separate SolutionsChromatography: 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 EquilibriumDynamic Equilibrium: both dissolving and crystallizing out of solution are occurring at the same rate which maintains a balance in the solution Beer-Lambert LawBeer-Lambert Law: a linear relationship between the absorbance and the concentration, molar absorption coefficient and optical coefficient of a solution |
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