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33 Cards in this Set
- Front
- Back
solution
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homogeneous mixture of two or more substances
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solvent
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has the greater number of moles and is generally considered the "vehicle" for the solute. Seen as less important (less note-worthy) than the solute.
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solute
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has fewer moles than the solvent and is normally the substance of interest. solutions are generally labeled with the solute.
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aqueous solution
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water is the solvent
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concentration
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ratio of solute to solvent (or to the entire solution).
uses molality and molarity for units |
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molarity
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moles of solute/liters of solution = mmol solute/mL solution.
used in problems involving osmotic pressure and stochiometry. |
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molality
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moles of solute/kg of solvent.
used in problems involving freezing point depression and boiling point elevation. |
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electrolyte
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any compound that can be dissolved into ions when placed in a solution.
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strong electrolyte
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completely dissolves into ions
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weak electrolyte
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partially dissolves into ions
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non-electrolytes
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do not dissolve into ions
(ex. ethanol) |
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osmosis
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when solvent passes through a semipermeable membrane to balance the solute on each side of the membrane
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semipermeable membrane
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allows only solvent passage through the membrane
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density of water
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1.00g/mL
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dilute solution
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contains less solute than a concentrated solution (well water)
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concentrated solution
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contains more solute than a dilute solution (sea-water)
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dilution
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when more solvent is added to a solution
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boiling point
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determined by amount of dissolved solute particles
the more solute dissolved, the higher the boiling point |
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Freezing Point Depression
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when solute is added, the freezing point lowers
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redox reactions
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oxidation/reduction reactions
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oxidation
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when electrons are lost
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reduction
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when electrons are gained
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oxidation number (ON)
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Charge that an atom possesses
halogens- ON= -1 alkali metals- ON= +1 alkaline earth metals- ON= +2 H- ON= +1 (sometimes -1) O- ON= -2 (sometimes -1 or -1/2) |
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oxidizing agents
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electron acceptors, they get reduced in a redox reaction
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reducing agents
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electron donors, they get oxidized
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acid-base
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neutralization (also an example of chemical equilibrium)
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acid
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donate H+ to the solution
(ex. HCl, HNO(3) |
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base
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accepts H+
(ex. NaOH, KOH, Ca(OH)(2)) |
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molecular equation
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chemical equation in which all reactants and products are written as molecules, when in reality, they are ions in water.
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Net Ionic Equation
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Chemical equation in which all soluble species are written in their aqueous ionic form
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Saturated Solution
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a solution with the maximum amount of solute for a given volume of solvent
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unsaturated solution
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a solution with less than the amount of solute per volume of solvent.
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supersaturated solution
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temporary condition in which the solution contains more than the saturated amount.
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