Identify the precipitate formed when solutions of these compounds are mixed.
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?
What precipitate is formed when solutions of these ionic compounds are mixed?
H2SO4 + BaCl2
To determine the precipitate formed when solutions of H2SO4 and BaCl2 are mixed, we need to consider the solubility of the products.
The double replacement reaction between H2SO4 (sulfuric acid) and BaCl2 (barium chloride) can be represented as follows:
H2SO4 + BaCl2 -> BaSO4 + 2HCl
According to the solubility rules, barium sulfate (BaSO4) is insoluble in water and forms a solid precipitate. Hydrochloric acid (HCl), on the other hand, is soluble and remains in solution.
So, the precipitate formed when H2SO4 and BaCl2 are mixed is BaSO4 (barium sulfate), and it will form a solid, while HCl will remain in solution as an aqueous compound.
To identify the precipitate formed when solutions of H2SO4 and BaCl2 are mixed, we need to understand the solubility rules of common compounds.
First, let's write the balanced chemical equation for the reaction:
H2SO4 + BaCl2 → BaSO4 + 2HCl
According to the solubility rules, most sulfates (like BaSO4) are insoluble, meaning they form solid precipitates. Chlorides (like HCl) are usually soluble and remain in solution. Thus, the precipitate formed in this reaction is BaSO4.
To answer your second question, yes, BaSO4 is a solid precipitate, while HCl remains in its ionic form as an aqueous solution.
It's important to note that this explanation is based on general solubility rules, and there might be exceptions or specific conditions that can influence the solubility of certain compounds.
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.