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Electrolytes

Electrolytes. Chemistry in Aqueous Solution. Types of Electrolytes. Strong : Completely dissociated (break into ions) Weak : Partially dissociate Non : No dissociation occurs. Examples of Electrolytes. Strong: Soluble Ionic Compounds NaNO 3 (s)  Na + + NO 3 - (these are ( aq ))

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Electrolytes

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  1. Electrolytes Chemistry in Aqueous Solution

  2. Types of Electrolytes • Strong : Completely dissociated (break into ions) • Weak : Partially dissociate • Non : No dissociation occurs

  3. Examples of Electrolytes • Strong: Soluble Ionic Compounds • NaNO3 (s)  Na+ + NO3- (these are (aq)) • Weak: Molecular Acids • HC2H3O2 (l)  H+ + C2H3O2- • Non: Molecular Non-acids (alcohols) • CH3OH (l)  does not dissociate

  4. Say what you mean! • Three types of equations: • Molecular • Ionic • Net ionic • Each is more specific… • Does not specify if they dissociate or not • Specifies which ones dissociate • Specify if an ion changes its dissociation

  5. Examples of Equations • Molecular: • NaCl(aq)+AgNO3(aq)AgCl(s)+NaNO3(aq) • Ionic: which are dissociated? • Na+ + Cl- + Ag+ + NO3- AgCl(s)+ Na+ + NO3- • Net Ionic: which ones changed? • Cl- + Ag+ AgCl(s) Spectator ions are removed since they don’t change

  6. Dissolve vs. Dissociate • Dissolve means to mix together to become homogenous. • Dissociate means to break apart upon dissolving. • You can dissolve without dissociating (non electrolyte) but… • You CANNOT dissociate without dissolving.

  7. Dissolving • Non-electrolyte (no ions)

  8. Dissociation • Strong electrolyte (all as ions)

  9. Weak Dissociation • Weak electrolyte (few ions in solution) Photos courtesy Hal Bender, Clackamas Community College http://dl.clackamas.edu/ch105-03/examples.htm

  10. Conductivity • More ions = more conductivity • Non electrolytes = no conductivity • Weak electrolytes = small conductivity • Strong Electrolytes = large conductivity

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