QuestionMultiple Choice 1 point
Which of the following would be a precipitate when the following aqueous solutions are mixed: $\mathrm{MgSO}_{4}$ and $\mathrm{BaCl}_{2}$ MgBa $\mathrm{Cl}_{2} \mathrm{SO}_{4}$ $\mathrm{BaSO}_{4}$ $\mathrm{MgCl}_{2}$ Previous

Studdy Solution

STEP 1

1. We are mixing two aqueous solutions: $\text{MgSO}_4$ and $\text{BaCl}_2$ .
2. A precipitate forms when an insoluble solid is produced in a reaction.
3. We need to determine which compound forms a precipitate.

STEP 2

1. Identify the possible products of the reaction.
2. Determine the solubility of each product.
3. Identify the insoluble product, which is the precipitate.

STEP 3

When $\text{MgSO}_4$ and $\text{BaCl}_2$ are mixed, a double displacement reaction can occur, leading to the formation of $\text{MgCl}_2$ and $\text{BaSO}_4$ .
The reaction is: $\text{MgSO}_4 (aq) + \text{BaCl}_2 (aq) \rightarrow \text{MgCl}_2 (aq) + \text{BaSO}_4 (s)$

STEP 4

Check the solubility of the products: - $\text{MgCl}_2$ is soluble in water. - $\text{BaSO}_4$ is insoluble in water.

STEP 5

Since $\text{BaSO}_4$ is insoluble, it will form a precipitate when the solutions are mixed.
The precipitate formed is:
$\boxed{\text{BaSO}_4}$

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