ionic equation Q?

Question

1)If you have solid sodium carbonate(Na2CO3) reacting with aqueous HF acid should the overall ionic equation show sodium carbonate as ions since they dissociated in the water of the aqueous HF or should they be an ionic compound since the question says it is solid? Why? Here's what I think it is but I'm not sure.

Molecular Equation
Na2CO3(s)+2HF(aq)===>2NaF+H2O+CO2

Overall ionic equation
2Na(+)+CO3(2-)+2HF===>2Na(+)+2F(-)+H2O+CO2
could someone please elaborate, I'm not sure why or why not sodium carbonate or the sodium fluoride should be written as ions. So if a soluble solid is added to something dissolved in water will it dissociate into ions too.

2)Can something covalent dissociate in water? How do you write the overall ionic equation for SO2+H2O===>H2SO3? Will the SO2 dissociate into ions? Will the H2SO# dissociate into ions??

Thank you for checking my work and helping me with #2

Answer 1

It sounds like a trick philosophical question to me. I'll go for the overall ionic equation, because Na2CO3(s) dissolves in water in any case. If you put solid Na2CO3 into a water solution of any thing, it is not going to sit there. "Pardon: I don't have teacher's permission to dissolve."

2) This is a reversible process. SO2 cannot dissociate into ions. SO2 + H2O <===> H2SO3 <===> 2H+ + SO3=