Dissolving an Ionic Electrolyte

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Presentation transcript:

Dissolving an Ionic Electrolyte

Stationary ions can NOT Dissolving an Ionic Electrolyte The dissolving of an ionic electrolyte. All salts are ionic electrolytes! Hydroxide bases are ionic electrolytes! + ― + ― Stationary ions can NOT conduct electricity Free moving ions can conduct electricity

Dissolving an Ionic Electrolyte Ex. (1) Write the dissolving reaction for each of the following ionic electrolytes. NaCl(s) → _____________________________ BaCl2(s) → ____________________________ Sr(OH)2(s) → __________________________ +1 -1 1+ 1- 1 H2O 1 Na + 1 Cl (aq) (aq) +2 -1 2+ H2O 1- 1 1 Ba + 2 Cl (aq) (aq) +2 -1 H2O 2+ 1- 1 1 Sr + 2 OH (aq) (aq)

Dissolving an Ionic Electrolyte Mg(NO3)2(s) → __________________________ Na2CO3(s) → ___________________________ KOH(s) → ______________________________ +2 -1 2+ H2O 1- 1 1 Mg + 2 NO3 (aq) (aq) +1 -2 2- H2O 1+ 2 Na + 1 1 CO3 (aq) (aq) +1 -1 1- H2O 1+ 1 1 K + 1 OH (aq) (aq)

Dissolving an Ionic Electrolyte Ex. (2) Which of the following sodium chloride samples is incapable of conducting electricity? (1) NaCl(s) (3) NaCl(aq) (2) NaCl(l) (4) NaCl(g) Ionic electrolytes will conduct electricity NOT only in the aqueous phase BUT also in the liquid and gases phases because the ions are free to move around!