[onesikgypo]

alright just a little help on questions where they start off like

"Balance the equation for the precipitation reaction between copper sulfate and barium chloride"

Now i know how to balance equations i just dont know about the "precipitation" part.

lol give use a lil head start   - copper sulfate = CuSO₄
                                        -  barium chloride = BaCl (if im not mistaken)

[Blueshawk]

alright just a little help on questions where they start off like

"Balance the equation for the precipitation reaction between copper sulfate and barium chloride"

Now i know how to balance equations i just dont know about the "precipitation" part.

lol give use a lil head start   - copper sulfate = CuSO₄
                                        -  barium chloride = BaCl (if im not mistaken)

All they want you to know is that a solid will be formed.  that is what precipitating means...to form a solid from liquids.  I am not sure whether the BaSO₄ or the CuCl₂ is the precipitate though.

CuSO₄ + BaCl₂ --->  CuCl₂ + BaSO₄.

I think BaSO₄ is slighlty soluble...so CuCl might be the precipitate.

[onesikgypo]

so do you like just swap the endings around for the right part of the equation?

[xiankai]

BaSO4 is the precipitate. CuCl is dissolvable.

this kind of reactions are in general what u said, but this is only the case when a less soluble salt than the two regeants can be formed. likewise, BaSO4 + CuCl will give u nothing because BaSO4 is less soluble than the possible products.

[Donaldson Tan]

CuCl is dissolvable.

It's CuCl₂, not CuCl.

Now i know how to balance equations i just dont know about the "precipitation" part.

Precipitation occurs because at least one of the products is insoluble in the solvent. In this case, the insoluble product is BaSO₄.

[charco]

All reactions are fundamentally reversible but when two types of ion bond together more 'tightly' than the ions bond to the solvent then these ions are removed from the mix as a solid precipitate. This pulls the reaction to the right hand side (the side of the precipitate).