Writing Net Ionic Equation

[woox]

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I am having issues writing net ionic equation, for example this problem:
Net Ionic Equation for:
BaCO3 + HCl ->

Answer:
BaCO3 + 2H+ -> H2O + CO2 + Ba

Can anyone explain? I thought all you had to do was cross out the spectator ions?

 

[rockclock]

I am having issues writing net ionic equation, for example this problem:
Net Ionic Equation for:
BaCO3 + HCl ->

Answer:
BaCO3 + 2H+ -> H2O + CO2 + Ba

Can anyone explain? I thought all you had to do was cross out the spectator ions?

H2CO3 decomposes to H2O and CO2 gas...

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

Cl-(aq) is the only spectator ion...

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

Make it 2H+ to balance.

 

[needzmoar]

EDIT: ^^^^read answer above

 

[rah08e]

EDIT: ^^^^read answer above

What does "H2CO3 decomposes to H2O and CO2 gas..." have to do with this problem? I thought we were using BaCO3.. and even so, how does BaCO3 turn into H2O and CO2?

I just read on a website that for decomposition: XCO3(s) --> XO(s) + CO2(g)

So I would think that: BaCO3 --> BaO(s) + CO2(g)

 

[mh0000]

What does "H2CO3 decomposes to H2O and CO2 gas..." have to do with this problem? I thought we were using BaCO3.. and even so, how does BaCO3 turn into H2O and CO2?

I just read on a website that for decomposition: XCO3(s) --> XO(s) + CO2(g)

So I would think that: BaCO3 --> BaO(s) + CO2(g)

What you wrote is for a thermal decomposition, which is not the case here. As others have stated, there will be an acid-base reactions between CO3(2-) and H+ from HCl. Of course BaCO3 is only slightly soluble, but the acid-base reaction drives the equilibrium to the product side. One of the products is H2CO3 (carbonic acid). This is not very stable in water, and will spontaneously decompose (not to be confused with thermal decomp) into CO2 gas and water (if in a open system, the release of CO2 gas from the system (ie solution) further drives the equilibrium to the right). Therefore, write the acid-base reaction in ionic form, cancel out common species and in the last step, just change H2CO3(aq) into water and CO2(g).

 

[rah08e]

What you wrote is for a thermal decomposition, which is not the case here. As others have stated, there will be an acid-base reactions between CO3(2-) and H+ from HCl. Of course BaCO3 is only slightly soluble, but the acid-base reaction drives the equilibrium to the product side. One of the products is H2CO3 (carbonic acid). This is not very stable in water, and will spontaneously decompose (not to be confused with thermal decomp) into CO2 gas and water (if in a open system, the release of CO2 gas from the system (ie solution) further drives the equilibrium to the right). Therefore, write the acid-base reaction in ionic form, cancel out common species and in the last step, just change H2CO3(aq) into water and CO2(g).

Where does the 2nd "H" come from when you formed H2CO3?

-Thanks

 

[mh0000]

Where does the 2nd "H" come from when you formed H2CO3?

-Thanks

From two H+ (from HCl). CO3(-2) + H+ <--> HCO3(-1)
Bicarbonate is itself a weak base (which is why it serves as an important buffer component for the blood, amongst other buffer systems of course)
HCO3(-1) + H+ <--> H2CO3 [ -> CO2 + H2O]

 

[woox]

So this is a reaction you should already know? Because I would I thought this:
BaCO3 + HCl -> BaCl2 + HCO3