Question

When the following solutions are mixed together, what precipitate (if any) will form? a. \(\mathrm{FeSO}_{4}(a q)+\mathrm{KCl}(a q)\) b. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q)\) c. \(\mathrm{CaCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)\) d. \(\mathrm{K}_{2} \mathrm{~S}(a q)+\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)\)

Short answer

Precipitates formed in each case are: - a. No precipitate - b. Al(OH)₃ - c. CaSO₄ - d. NiS

Step-by-step solution

a. FeSO4(aq) + KCl(aq)

1. Analyze the chemical equation: The given solutions are: FeSO4(aq) - containing Fe²⁺ and SO₄²⁻ ions, and KCl(aq) - containing K⁺ and Cl⁻ ions. 2. Determine the possible combinations: The possible combinations of these ions are: FeCl₂ and K₂SO₄. 3. Check solubility: According to the solubility rules, both FeCl₂ and K₂SO₄ are soluble, so no precipitate will form in this case.

b. Al(NO₃)₃(aq) + Ba(OH)₂(aq)

1. Analyze the chemical equation: The given solutions are: Al(NO₃)₃(aq) - containing Al³⁺ and NO₃⁻ ions, and Ba(OH)₂(aq) - containing Ba²⁺ and OH⁻ ions. 2. Determine the possible combinations: The possible combinations of these ions are: Al(OH)₃ and Ba(NO₃)₂. 3. Check solubility: According to the solubility rules, Al(OH)₃ is insoluble, and Ba(NO₃)₂ is soluble. 4. Write down the balanced chemical equation: When these two solutions are combined, a precipitate will form as Al(OH)₃. \[ Al^{3+}(aq) + 3OH^{-}(aq) \rightarrow Al(OH)_3(s) \]

c. CaCl₂(aq) + Na₂SO₄(aq)

1. Analyze the chemical equation: The given solutions are: CaCl₂(aq) - containing Ca²⁺ and Cl⁻ ions, and Na₂SO₄(aq) - containing Na⁺ and SO₄²⁻ ions. 2. Determine the possible combinations: The possible combinations of these ions are: CaSO₄ and NaCl. 3. Check solubility: According to the solubility rules, CaSO₄ is slightly soluble (which can still form a precipitate), and NaCl is soluble. 4. Write down the balanced chemical equation: When these two solutions are combined, a precipitate will form as CaSO₄. \[ Ca^{2+}(aq) + SO_{4}^{2-}(aq) \rightarrow CaSO_4(s) \]

d. K₂S(aq) + Ni(NO₃)₂(aq)

1. Analyze the chemical equation: The given solutions are: K₂S(aq) - containing K⁺ and S²⁻ ions, and Ni(NO₃)₂(aq) - containing Ni²⁺ and NO₃⁻ ions. 2. Determine the possible combinations: The possible combinations of these ions are: KNO₃ and NiS. 3. Check solubility: According to the solubility rules, KNO₃ is soluble, and NiS is insoluble. 4. Write down the balanced chemical equation: When these two solutions are combined, a precipitate will form as NiS. \[ Ni^{2+}(aq) + S^{2-}(aq) \rightarrow NiS(s) \] In summary, precipitates will form in the following cases: - b. Al(NO₃)₃(aq) + Ba(OH)₂(aq) will form Al(OH)₃ - c. CaCl₂(aq) + Na₂SO₄(aq) will form CaSO₄ - d. K₂S(aq) + Ni(NO₃)₂(aq) will form NiS

Key concepts

Solubility Rules

Solubility rules are guidelines that help determine whether a substance will dissolve in water, forming an aqueous solution, or remain as a solid, forming a precipitate. These rules are essential in predicting the outcomes of chemical reactions, especially when dealing with ionic compounds in water.

- **Common soluble substances:** Nitrates ( O_3^-), acetates, and ammonium compounds are typically soluble. Most alkali metal salts, such as those containing sodium or potassium, also dissolve in water.
- **Common insoluble substances:** Carbonates, phosphates, sulfides, and hydroxides often do not dissolve, with exceptions like calcium and barium hydroxides being slightly soluble. By using these rules, you can predict if a combination of ions will stay soluble in an aqueous solution or form a precipitate.

For example, in one of the cases from the exercise, we found that Al(OH)_3 is an insoluble hydroxide, which formed a precipitate when Al(NO_3)_3 and Ba(OH)_2 were mixed.

Chemical Equation Balancing

Balancing chemical equations is crucial to accurately represent chemical reactions.Every balanced equation reflects the Law of Conservation of Mass, where the number of each type of atom is conserved from reactants to products.

A balanced equation provides the correct stoichiometric quantities for each substance involved and predicts how much product will form or how much reagent is needed. To balance a chemical equation:

• Write the unbalanced equation based on the reactant and product formulas.
• Count the number of atoms of each element on both sides.
• Add coefficients (numbers in front of compounds) to match the number of atoms on each side.

Using this approach, the reaction between Al(NO_3)_3 and Ba(OH)_2 can be balanced as:\[ Al^{3+}(aq) + 3OH^{-}(aq) \rightarrow Al(OH)_3(s) \]
Here, one aluminum ion reacts with three hydroxide ions to form insoluble aluminum hydroxide.

Aqueous Solutions

An aqueous solution is formed when a substance is dissolved in water. In chemistry, they are often used to carry out reactions due to water's excellent solvent properties. When ionic compounds dissolve, they dissociate into their component ions, which then freely move in the solution, allowing for reactions.

When iron(II) sulfate and potassium chloride are mixed, they form an aqueous solution containing Fe²⁺, SO₄²⁻, K⁺, and Cl⁻ ions. These ions can move around freely in the solution, but they do not produce any new insoluble compounds, as shown by the solubility rules.
- **Formation of aqueous solutions** allows reactions to occur more readily due to increased ion mobility.
- **Dissociation**: The process in which ionic compounds separate into their individual ions in solution is key to the behavior of ionic reactions.

Chemical Reactions Analysis

Analyzing chemical reactions involves not only recognizing reactants and products but also understanding how they change and what new substances might form. This requires a comprehension of ionic transformations and the formation of any precipitates.

- **Combining Ions:** When aqueous solutions of CaCl_2 and Na_2SO_4 are mixed, new combinations of ions can occur, such as Ca^{2+} and SO_4^{2-}, which precipitate as CaSO_4(s).
- **Predicting Outcomes:** By understanding solubility rules and ion reactivity, one can predict when a reaction will result in a precipitate, like NiS from Ni(NO_3)_2 and K_2S.
- **Reaction Pathways:** It's crucial to identify what is occurring in a solution at a molecular level, ensuring recognition of the solid precipitates forming from soluble ions. Be mindful of which ions remain in solution as spectator ions, as they don't participate in the chemical change.