Ionic Equation Question

[Golfguy]

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What is the net ionic equation?

BaCO3 + HCl ----> ?


BaCO3 + 2H+ ----> Ba+ (aq) + CO2 (g) + H20(l)


Why does Ba+ get included in the net equation, but Cl doesn't? Shouldn't both drop out? Plus, I thought Group II carbonates are insoluble.

 

[rpatel8]

I also don't understand how CO2 is formed. If someone could explain, that would be great. Thanks

 

[Golfguy]

I also don't understand how CO2 is formed. If someone could explain, that would be great. Thanks

H2CO3 -----> CO2 + H20

Carbonic acid decomposes like this. Think of how your blood carries CO2 gas.

 

[PooyaH]

If you right out the ionic form of the reaction you'd get:

BaCO3(s) + 2HCl ->BaCl2(aq) + CO2(g) + H2O(l)

BaCO3(s) + 2H+ + 2Cl- -> Ba2+ + 2Cl- + CO2(g) + H2O(l) ....... (2Cl-'s cancel)

BaCO3(s) + 2H+ -> Ba2(aq) + CO2(g) + H2O(l)

There are so many exceptions with solubility. BaCl2 is one of them. Anything with Cl- is soluble except AgCl, PbCl2, and HgCl.

 

[rockclock]

What is the net ionic equation?

BaCO3 + HCl ----> ?


BaCO3 + 2H+ ----> Ba+ (aq) + CO2 (g) + H20(l)


Why does Ba+ get included in the net equation, but Cl doesn't? Shouldn't both drop out? Plus, I thought Group II carbonates are insoluble.

you basically answered your own question, Golf...

BaCO3 is essentially insoluble, which is why it appears as a solid in the reactants and not as dissociated aqueous ions (like HCl). CO2 and H2O dropping out of equilibrium drives the reaction, though, which pulls the balance in favor of products.