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What property of all ionic compounds make them electrolytes? they dissociate into ions
What would you do to reduce the solubility of gas solute in a gas/liquid solution? reduce the partial pressure of the gas above the solution
Tyndall Effect separation of light as it passes through colloid or suspension
Solute substance in lesser quantity that is dissolved
Emulsion a colloid of a liquid in a liquid
Electrolyte ionic compounds that dissolve into solution and conducts electricity
Alloy homogeneous mixtures of metals
Immiscible describes liquids that are insoluble in one another
Saturated Solution solution containing maximum amount of solute
Supersaturated Solution solution containing more solute than can theoretically dissolve at a given temperature
Colloid heterogeneous mixture in which particles cannot be separated by filtration
Polar molecules with uneven distribution of charge
Solvent dissolving medium, the substance in greater quantity
Aqueous Solution homogeneous mixture of water and dissolved substances
Solvation solute ions or molecules are surrounded by solvent molecules
Tincture homogeneous mixture of dissolved particles in alcohol
Solution homogeneous mixture of solute and solvent
Solute + Solvent = solution
Solvent-Solvent energy absorbed
Solute-Solute energy absorbed
Solvent-Solute energy released
Dissociation separation of an ionic solid into aqueous ions
Ionization breaking apart of some polar molecules into aqueous ions
Dispersion molecules stay intact
Two substances with similar IMF are likely to be soluble in one another
Non-Polar molecules are soluble in non-polar solvents
Ionic compounds are more soluble in polar solvents
How do we know ions are present in aqueous solutions? electrolytes
Non-electrolytes some compounds dissolve in water but do not conduct electricity
Unsaturated Solution when the solvent holds less solute than it normally can at a given temperature
Solubility the maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature
Concentration the amount of solute in a solution
More solute, constant amount of solvent more concentrated
Less solute less concentrated
More solvent less concentrated
Less solvent more concentrated
Dilution the procedure for preparing a less concentrated solution from a more concentrated solution
3 Factors Affecting Solubility the size of the solute/crystals the temperature of the solvent the vigor and duration of stirring
Henry's Law States That the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution
Henry's Law c=kP
c concentration(M) of the dissolved gas
k a constant for each gas (mol/L x atm) that depends only on temperature
P pressure of the gas over the solution
The solubility of gases decreases at higher temperatures
Colligative Properties are properties of solutions that depend on the ratio of the number of solute particles to the number of solvent molecules in a solution, and not on the nature of the chemical species present
Created by: jordinlevy