Is this net ionic equation correct? (#2!)
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Is this net ionic equation correct? (#2!)

[From: ] [author: ] [Date: 11-04-22] [Hit: ]
and am not sure which way to go.If I dont break it up,If I break it up,and removing 2Cl,My question is, apart from which way is correct,......
I have a molecular equation of:

CaCo3 (s) + 2HCl (aq) ---> CaCl2 (aq) + CO2 (g) + H2O (l)

I'm not sure if when writing the net ionic equation, I break down the CaCO3 or not, as it's a solid. I've seen both answers on here, and am not sure which way to go.

If I don't break it up, I get:

CaCO3 (s) + 2H+ (g) + 2Cl- (aq) ---> Ca2+ (aq) + 2Cl (aq) + CO2 (g) + H2O (l)
and removing 2Cl as the spectator ions to get:
CaCO3 (s) + 2H+ (g) ---> Ca2+ (aq) + CO2 (g) + H2O (l)

If I break it up, I get:

Ca2+ (s) + (CO3)2- (s) + 2H+ (g) + 2Cl- (aq) ---> Ca2+ (aq) + 2Cl (aq) + CO2 (g) + H2O (l)
and removing 2Cl, Ca2 as the spectator ions to get:
(CO3)2- (s) + 2H+ (g) ---> CO2 (g) + H2O (l)

My question is, apart from which way is correct, is WHY is that way correct, and how do I tell how far to split the molecules into ions?

This chemistry is killing me...

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Your first method is the correct one. You should never break up the solid, like CaCO3(s), it should remain in that form in any of the equations you write.

CaCO3(s) + 2 H^+(aq) --> Ca^2+(aq) + H2O(l) + CO2(g) represents the correct net ionic equation.

This is correct because the CaCO3 does not break apart into ions on the reactant side of the equation. The solid CaCO3 is attacked by the H^+ ions which breaks down the structure into its ions. That will be generally true for any reaction that contains a solid and an acid.

Hope this is helpful. JIL HIR

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As CaCO3 is insoluble in wtr, ionization of CaCO3 in not possible.It reacts directly with HCL(aqu)
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