Answered

[tex]\[ \text{Na}_2\text{SO}_4(aq) + \text{BaI}_2(aq) \rightarrow \][/tex]

Express your answer as a chemical equation. Enter "noreaction" if no precipitate is formed.

[tex]\[\square\][/tex]

A chemical reaction does not occur for this question.



Answer :

Certainly! Let's address the chemical equation and determine if a reaction occurs:

When we mix sodium sulfate [tex]\( \text{Na}_2\text{SO}_4 \)[/tex] with barium iodide [tex]\( \text{BaI}_2 \)[/tex], we need to consider the possible products and whether a precipitate forms. The ions in solution are:

[tex]\( \text{Na}_2\text{SO}_4 \rightarrow 2\text{Na}^+ + \text{SO}_4^{2-} \)[/tex]

[tex]\( \text{BaI}_2 \rightarrow \text{Ba}^{2+} + 2 \text{I}^- \)[/tex]

Upon mixing, the ions can combine to form:

1. Sodium iodide [tex]\( \text{NaI} \)[/tex]
2. Barium sulfate [tex]\( \text{BaSO}_4 \)[/tex]

Now we check the solubility rules:

1. Sodium iodide [tex]\( \text{NaI} \)[/tex] is soluble in water.
2. Barium sulfate [tex]\( \text{BaSO}_4 \)[/tex] is insoluble in water and will form a precipitate.

So, by combining these ions:

[tex]\[ \text{Na}_2\text{SO}_4 (aq) + \text{BaI}_2 (aq) \rightarrow 2 \text{NaI} (aq) + \text{BaSO}_4 (s) \][/tex]

Thus, a reaction occurs and a precipitate of barium sulfate is formed:

[tex]\[ \text{BaSO}_4 (s) \][/tex]

So the balanced chemical equation for the reaction is:

[tex]\[ \text{Na}_2\text{SO}_4 (aq) + \text{BaI}_2 (aq) \rightarrow 2 \text{NaI} (aq) + \text{BaSO}_4 (s) \][/tex]

This confirms that a reaction does occur and results in the formation of a precipitate.