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Equations for the dissolution of salts of strong bases and weak acids

Submitted by chrisf on Sun, 06/29/2008 - 08:58

With Spectator Ion(s)

CH3COONa.3H2O + H2O -> CH3COOH + Na+ + OH-

Na2HPO4.7H2O + H2O -> H2PO4 + Na+ + OH-

Without Spectator Ion(s)

CH3COO.3H2O + H2O -> CH3COOH + OH-

HPO4.7H2O + H2O -> H2PO4 + OH-

Would these be correct?


Just have to know your solubility rules & Strong Acids and Bases for this.

I never understood what .xH2O meant, so I'm not quite sure myself.  I do know that Na will become an ion, so it shouldn't appear in your net ionic. 


SchoolBoyDJ wrote:

Just have to know your solubility rules & Strong Acids and Bases for this.

I never understood what .xH2O meant, so I'm not quite sure myself.  I do know that Na will become an ion, so it shouldn't appear in your net ionic. 

The .xH2O indicates a hydrated ionic compound. The H2O isn't chemically bonded, but it exists inside the crystal lattice. I believe they're usually hygroscopic.


The water of hydration should not appear in a net ionic equation:

  CH3COO-  +  H2O  -->  CH3COOH  +  OH-

  HPO4-2    +  H2O  -->  H2PO4-  +  OH-


spock wrote:

The water of hydration should not appear in a net ionic equation:

I was wondering about that, since they're not really chemically bonded...

Thanks!