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sseebeck Group Title

Is the equation NaCl(s) + H2O -> Na+(aq) + Cl-(aq) considered balanced? I said that it was as the aq on the product side accounts for the H2O on the reactant side but the textbook uses the same equation and omits the H20 on the reactant side. Is the H20 necessary?

  • one year ago
  • one year ago

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  1. abb0t Group Title
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    No. NaOH and HCl are both strong acid/ base and would not exist together. They merely dissociate the Saodium and Chlorine into ions. In some cases, I think H+ and OH- ions might be there, but when the salt concentration is high. Sodium and Chlorine ions are able to be with water. I think its just assumed that you have the ions floating in the system with water.

    • one year ago
  2. sseebeck Group Title
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    I must be missing something still. When sodium chloride dissociates into its respective Ions Those Ions are then surrounded by the polar ends of water molecules. But is it necessary to account for the H2O with the reactants because while it does not react with the NaCl it is still present and does not get dropped from the product side of the equation (it remains part of the equation as aq indicates that water is present as the solvent)

    • one year ago
  3. abb0t Group Title
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    yes.

    • one year ago
  4. sseebeck Group Title
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    Thanks

    • one year ago
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