Identify the precipitate formed when solutions of these compounds are mixed.

Question

H2SO4 + BaCl2 ==>

So when you do the double replacement reaction, would the products of this chemical equation be HCl + BaSO4? or H2Cl2 + BaSO4 ? (not balanced)

also would both of the products be solids?

Answer 1

H2SO4(aq) + BaCl2(aq) ==> BaSO4(s) + 2HCl(aq)
Your response to your question makes me think you are trying an old student trick of "trying to make the equation balance by changing the subscripts." How else would you explain getting H2Cl2. HCl is hydrochloric acid and you balance ONLY (repeat ONLY) by changing the coefficients. Rule number one in balancing equation is what not to do. You may NOT change any of the subscripts. You also need to know the solubility tables when problems like this come along. Here is a simplified set of rules.
http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html
The way you do these questions is to write the double displacement (double replacement) reaction, then go through three questions you ask yourself.
a. Is one of the products a gas? If so the reaction will go as written.
b. Is one of the products insoluble? If so the reaction will go as written.
c. Is one of the products a weak electrolyte? If so the reaction will go as written.

Answer 2

What precipitate is formed when solutions of these ionic compounds are mixed?

H2SO4 + BaCl2