Question

For the following chemical reactions, determine the precipitate produced when the two reactants listed below are mixed together. Indicate "none" if no precipitate will form.

Short answer

In the first example reaction, the precipitate produced is BaSO₄ (barium sulfate), and in the second example reaction, there is no precipitate formed.

Step-by-step solution

Write the balanced chemical equation.

First, we need to write the balanced chemical equation for the reaction between barium nitrate and sodium sulfate. Ba(NO₃)₂(aq) + Na₂SO₄(aq) → BaSO₄ + 2NaNO₃

Determine the solubility of the products.

We need to determine the solubility of BaSO₄ and NaNO₃ in water. By referring to the solubility rules mentioned in the analysis, we know that most nitrates are soluble, so NaNO₃ is soluble in water. Most sulfates are soluble, except for those with certain cations such as barium. Therefore, BaSO₄ is insoluble in water.

Identify the precipitate.

Since BaSO₄ is insoluble in water, it will form a precipitate when the two reactants are mixed. So, the precipitate produced in this reaction is BaSO₄. Example 2: Mixing together aqueous solutions of potassium chloride (KCl) and ammonium nitrate (NH₄NO₃).

Write the balanced chemical equation.

First, we need to write the balanced chemical equation for the reaction between potassium chloride and ammonium nitrate. KCl(aq) + NH₄NO₃(aq) → KNO₃ + NH₄Cl

Determine the solubility of the products.

We need to determine the solubility of KNO₃ and NH₄Cl in water. By referring to the solubility rules mentioned in the analysis, we know that most nitrates are soluble, so KNO₃ is soluble in water. Most chlorides are soluble, including those formed with ammonium, so NH₄Cl is soluble in water.

Identify the precipitate.

Since both KNO₃ and NH₄Cl are soluble in water, no precipitate is formed in this reaction. Therefore, the answer is "none".