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Reactions in Aqueous Solutions

Reactions in Aqueous Solutions. Aqueous Solutions. Electrolyte: a substance whose water solution conducts an electric current Note: Organic substances are generally non-electrolytes (or at best weak electrolytes like acetic acid) Generally soluble ionic compounds are electrolytes

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Reactions in Aqueous Solutions

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  1. Reactions in Aqueous Solutions

  2. Aqueous Solutions • Electrolyte: a substance whose water solution conducts an electric current • Note: • Organic substances are generally non-electrolytes (or at best weak electrolytes like acetic acid) • Generally soluble ionic compounds are electrolytes • When an electrolyte dissolves in water it breaks apart into its component ions. • Examples: NaCl(s), K2SO4(s), HNO3, Ca(OH)2(s)

  3. NaCl(s)  Na+(aq) + Cl-(aq) • K2SO4(s) 2K+ (aq)+ SO42-(aq) • HNO3 H+ (aq)+ NO3-(aq) • Ca(OH)2(s)  Ca2+(aq)+ 2OH- (aq)

  4. The ions in solution makes it able to conduct electricity – the more ions present, the better the conduction • Strong Electrolyte: ionizes completely (many ions) • Weak Electrolyte: ionizes < 50% (few ions) • Non-Electrolyte: ionizes less than 0.01% (no ions)

  5. Reactions involving Ions In a solution, oppositely charged ions will attract each other and collide. If the +/- combination is only slightly soluble in water, it will form a solid in the liquid. This solid is called a precipitate. Example: A yellow precipitate forms when solutions of lead(II) nitrate and sodium iodide are mixed.

  6. Explanation: Each solution contributes two ions to the mixture: Pb(NO3) 2(s) Pb2+(aq) + 2NO3-(aq) NaI(s)  Na+(aq) + I-(aq) The yellow precipitate can only be PbI2 or NaNO3. Refer to the solubility table to determine which combination is insoluble.

  7. The solubility table shows that only PbI2 has low solubility, therefore it will be the yellow precipitate. The complete ionic equation is: Pb2+(aq) + 2NO3-(aq) + Na+(aq) + 2I-(aq) PbI2(s) + Na+(aq) + 2NO3-(aq) If spectator ions (ions that are not involved in the reaction) are cancelled on either side, the net equation can be written: Pb2+(aq) + 2I-(aq) PbI2(s)

  8. Examples: Write the complete ionic equation and net ionic equation for the following mixtures: • Potassium hydroxide and aluminum chloride • Iron(III)sulfate and sodium sulfide • Bismuth nitrate and ammonium hydroxide • Aluminum bromide and sodium carbonate

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