Solubility Rules/ Precipitates!?!

Chemistry
Tutor: None Selected Time limit: 1 Day

Aug 4th, 2015

Thank you for the opportunity to help you with your question!

http://chemwiki.ucdavis.edu/Physical_Chemistry/Equilibria/Solubilty/Solubility_Rules

The above website lists the solubility rules, but they should also be found in your text.  The first thing that we want to do when looking at one of these problems is to first predict the products.

a.  Here we are combining barium hydroxide (Ba(OH)2 ) and ammonium phosphate ( (NH4)3PO4).  Reactions like this are always double displacement reactions meaning that the anions are switched to go with the opposite cation.

So,

Ba(OH)2 + (NH4)3PO4 <=====> Ba3(PO4)2 + NH4OH

Now we need to see if the products are soluble.  According to rule 1 (from the website above), all salts with NH4+ in them are soluble.  However, by rule 10, phosphates are usually insoluble. So the reaction given would produce a precipitate in the form of Ba3(PO4)2


b.  The rest ill follow a similar procedure.

AgNO3 + KCH3CO2 <=====> AgCH3CO2 + KNO3

By rule 4, AgCH3CO2 should be insoluble and form a precipitate since most silver salts are insoluble.  KNO3 would be soluble by both rules 1 and 2.


c.  

Cu2SO4 + NaCl <=====>  CuCl + Na2SO4

By rule 3, CuCl is soluble.  By rules 1 and 5, Na2SO4 is also soluble.  This means this reaction would not produce a precipitate.

Please let me know if you need any clarification. I'm always happy to answer your questions.
Aug 4th, 2015

Does it matter whether the reactants are soluble or insoluble? 

Aug 4th, 2015

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