net ionic equations
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net ionic equations
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What are the rules you have to consider when determining the net ionic equation for a rxn?
Like how would it work in this example?
HCl (aq) + NaOH (aq) --> H2O (l) + NaCl (aq)
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You must consider the official "solubility rules" of ionic compounds, found in any GenChem textbook and all over the web. They're not too bad to memorize, and you MUST have them memorized to do well in chemistry.
Basically,
You write the reaction as you did, balance it, and then apply the solubility rules to see which (if any) compounds would dissociate into ions in an aqueous solution.
In your example, the NEXT step should be written next as H+(aq) + Cl-(aq) + Na+(aq) + OH-(aq) ---------> H20(l) + Na+(aq) + Cl-(aq)
The reason HCl and NaOH break into their ions is because based on solubility rules, they're soluble (anything that is soluble breaks up). If it were PbCl instead of NaCl, PbCl would have stayed PbCl since Pb+ is an exception to Cl's solubility. NOW THEN, once you've done this, you cancel out the common ions from both sides of the "----->" and you're left with
H+(aq) + OH-(aq) ---> H20 (l) ... this is the NET ionic equation because you cancelled out all common ions.
hope this helps.
DO LOOK UP SOLUBILITY RULES !!!
Neel.
--------------------------------------------------------------------------------
What are the rules you have to consider when determining the net ionic equation for a rxn?
Like how would it work in this example?
HCl (aq) + NaOH (aq) --> H2O (l) + NaCl (aq)
-----------------
You must consider the official "solubility rules" of ionic compounds, found in any GenChem textbook and all over the web. They're not too bad to memorize, and you MUST have them memorized to do well in chemistry.
Basically,
You write the reaction as you did, balance it, and then apply the solubility rules to see which (if any) compounds would dissociate into ions in an aqueous solution.
In your example, the NEXT step should be written next as H+(aq) + Cl-(aq) + Na+(aq) + OH-(aq) ---------> H20(l) + Na+(aq) + Cl-(aq)
The reason HCl and NaOH break into their ions is because based on solubility rules, they're soluble (anything that is soluble breaks up). If it were PbCl instead of NaCl, PbCl would have stayed PbCl since Pb+ is an exception to Cl's solubility. NOW THEN, once you've done this, you cancel out the common ions from both sides of the "----->" and you're left with
H+(aq) + OH-(aq) ---> H20 (l) ... this is the NET ionic equation because you cancelled out all common ions.
hope this helps.
DO LOOK UP SOLUBILITY RULES !!!
Neel.
thanks neel,
i always new my solubility rules should be memorized, just hadnt gotten around to it yet...guess i should do it soon. thanks for the help though
i always new my solubility rules should be memorized, just hadnt gotten around to it yet...guess i should do it soon. thanks for the help though
