Ch 13 | Ions in Aqueous Solutions and Colligative Properties

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17 Terms

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dissociation

separation of ions that occurs when an ionic compound dissolves

<p>separation of ions that occurs when an ionic compound dissolves</p>
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net ionic equation

Includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution

<p>Includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution</p>
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spectator ions

Ions that do not take part in a chemical reaction and are found in solution both before and after the reaction

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ionization

process in which ions are formed from solute molecules by the action of solvent; molecular/nonpolar in polar

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dissociation vs ionization

dissociation starts with an ionic compound and ionization starts with a molecular compound

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hydronium ion

hydrogen ion attracts other ions/molecule so strongly that is doesn't normally exist alone > bonds with a water molecule to form

<p>hydrogen ion attracts other ions/molecule so strongly that is doesn't normally exist alone &gt; bonds with a water molecule to form</p>
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electrolyte's strength depends on

how many dissolved ions it contains; related to their ability to form ions in solutions

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strong electrolyte

any compound whose dilute aqueous solutions conduct electricity well; this is due to the presence of all or almost all of the dissolved compound in the form of ions

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strong electrolyte examples

all soluble ionic compounds and HCl, HBr, HI, H2SO4, HNO3, HClO4, HClO3

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weak electrolyte

any compound whose dilute aqueous solutions conduct electricity poorly; this is due to the presence of a small amount of the dissolved compound in the form of ions

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colligative property

depends on the concentration of solute particles but not on the identity

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freezing point depression

the difference in temperature between the freezing point of a solution and the freezing point of the pure solvent

<p>the difference in temperature between the freezing point of a solution and the freezing point of the pure solvent</p>
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determining actual freezing point (solvent is water)

negative of ΔTf

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determining actual freezing point (solvent is not water)

Tf (solvent) - ΔTf

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boiling-point elevation

the difference in temperature between the boiling point of a solution and the boiling point of the pure solvent

<p>the difference in temperature between the boiling point of a solution and the boiling point of the pure solvent</p>
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determining actual boiling point

Tb (solvent) + ΔTb

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when solute is ionic/polar

multiply ΔT by # of solute ions

<p>multiply ΔT by # of solute ions</p>