Question

Aqueous solutions of the substance nickel(II) sulfate are bright green in color. If an aqueous solution of barium chloride is added to an aqueous solution of nickel(II) sulfate, a white precipitate of barium sulfate forms. From the information above, indicate one chemical property of nickel(II) sulfate in solution.

Short answer

One chemical property of nickel(II) sulfate in solution is its ability to form a precipitate when combined with solutions containing compounds such as barium chloride. This is demonstrated by the formation of barium sulfate (white precipitate) upon reacting with barium chloride.

Step-by-step solution

Write down the chemical formulas

The first step is to determine the chemical formulas of the compounds involved in the reaction. We have the following: 1. Nickel(II) sulfate (NiSO₄) 2. Barium chloride (BaCl₂) 3. Barium sulfate (BaSO₄)

Write the balanced equation for the reaction

The initial reaction will be between NiSO₄ and BaCl₂, and the given outcome of the reaction is formation of the white precipitate. Let's write down the balanced equation for this reaction: NiSO₄ (aq) + BaCl₂ (aq) → BaSO₄ (s) + NiCl₂ (aq)

Identify the precipitate

According to the given information, the white precipitate formed in the reaction is barium sulfate (BaSO₄).

Determine the chemical property of nickel(II) sulfate

Based on this information, we find that one chemical property of nickel(II) sulfate in solution is the ability to form a precipitate when combined with solutions containing compounds such as barium chloride. This property can be demonstrated by the formation of barium sulfate (white precipitate) upon reacting with barium chloride, as described in the balanced chemical equation.

Key concepts

Chemical Reactions

Chemical reactions are the processes by which substances interact to form new substances with different properties. In the reaction between nickel(II) sulfate and barium chloride, we observe the transformation of reactants into products, indicating a chemical change. Essential to understanding these transformations is recognizing the signs of a chemical reaction, such as color changes, temperature changes, gas production, or the formation of a precipitate.When nickel(II) sulfate, which is bright green, reacts with barium chloride, these signals are important. They help us conclude that a chemical reaction has taken place, as evidenced by the appearance of a white precipitate. This particular reaction showcases a common property of solutions: their ability to undergo chemical changes when brought together with other reactive species.

Precipitation Reactions

Precipitation reactions occur when two aqueous solutions combine to produce an insoluble solid called a precipitate. In the context of the nickel(II) sulfate and barium chloride reaction, the white precipitate of barium sulfate forms as a result of this process. This reaction is predictable if we know the solubility rules that govern which ionic compounds are soluble and which are not. Barium sulfate is designated as insoluble in water, hence its appearance as a precipitate.

• The key to identifying a precipitation reaction is the formation of a solid product from two clear solutions.
• Not all reactions between aqueous solutions yield a precipitate; the outcome depends on the solubility of the potential products.

The identification of the precipitate in this kind of reaction is crucial for laboratory analysis and industrial processes where separation of substances is necessary.

Balancing Chemical Equations

Balancing chemical equations is a fundamental skill in chemistry. It ensures the conservation of mass and the correct stoichiometry within a chemical reaction. In the reaction between nickel(II) sulfate and barium chloride, we must ensure that the number of atoms for each element is the same on both sides of the equation. This is achieved by adjusting coefficients in front of the chemical formulas.For example, the balanced equation for the given reaction is:\[\begin{equation} NiSO_4 (aq) + BaCl_2 (aq) \rightarrow BaSO_4 (s) + NiCl_2 (aq) \end{equation}\]In this equation, there is one nickel, one sulfur, four oxygen, one barium, and two chlorine atoms on both sides, hence it's already balanced. Understanding how to balance equations is crucial in predicting the amounts of reactants needed and products formed in a reaction.

Aqueous Solutions

An aqueous solution is a solution where water is the solvent. When substances like nickel(II) sulfate and barium chloride are dissolved in water, they form aqueous solutions. The chemical behavior of these substances in water, including reactivity and solubility, is pivotal to predicting the outcomes of reactions.In the studied reaction, both nickel(II) sulfate and barium chloride are soluble in water and are present as ions. This is a prerequisite for the reaction to occur and results in the formation of a precipitate:

• NiSO_4 (aq) dissociates into Ni^{2+} and SO_4^{2-} ions.
• BaCl_2 (aq) dissociates into Ba^{2+} and Cl^- ions.

These ions are then free to interact and form new combinations. The insoluble barium sulfate forms because the Ba^{2+} ions from the barium chloride solution meet the SO_4^{2-} ions from the nickel(II) sulfate solution, resulting in a compound that does not dissolve in water. Understanding aqueous solutions enables us to predict and explain these interactions clearly.