Certainly! Let's determine the correct products of the reaction between barium chloride ([tex]\( \text{BaCl}_2 \)[/tex]) and magnesium sulfate ([tex]\( \text{MgSO}_4 \)[/tex]).
### Step-by-Step Solution
1. Write the reactants:
- [tex]\( \text{BaCl}_2 \)[/tex] (barium chloride)
- [tex]\( \text{MgSO}_4 \)[/tex] (magnesium sulfate)
2. Identify the possible products:
- [tex]\( \text{BaSO}_4 \)[/tex] (barium sulfate) and [tex]\( \text{MgCl}_2 \)[/tex] (magnesium chloride)
- Other suggested products include complex and unlikely combinations such as [tex]\( \text{BaMg} + \text{ClSO}_4 \)[/tex], [tex]\( \text{Ba}( \text{SO}_4)_2(s) + \text{MgCl} \)[/tex], and [tex]\( \text{Ba} + \text{Mg} + \text{Cl}_2 \)[/tex].
3. Determine the precipitate:
- Barium sulfate ([tex]\( \text{BaSO}_4 \)[/tex]) is insoluble in water and will form a solid precipitate.
- Magnesium chloride ([tex]\( \text{MgCl}_2 \)[/tex]) is soluble in water and will remain in solution.
4. Write the balanced chemical equation:
[tex]\[
\text{BaCl}_2 (aq) + \text{MgSO}_4 (aq) \rightarrow \text{BaSO}_4 (s) + \text{MgCl}_2 (aq)
\][/tex]
5. Confirm the products:
- According to the solubility rules and balanced equation, the resulting products are barium sulfate ([tex]\( \text{BaSO}_4 \)[/tex]) and magnesium chloride ([tex]\( \text{MgCl}_2 \)[/tex]).
Based on this detailed analysis, the correct products of the reaction are barium sulfate ([tex]\( \text{BaSO}_4 \)[/tex]) in solid form and magnesium chloride ([tex]\( \text{MgCl}_2 \)[/tex]) in aqueous form.
Therefore, the correct answer is:
[tex]\[ \text{BaSO}_4 (s) + \text{MgCl}_2 (aq) \][/tex]
