You choose to investigate some of the solubility guidelines for two ions not listed in Table 4.1, the chromate ion (CrO₄²⁻) and the oxalate ion (C₂O₄²⁻). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: When these solutions are mixed, the following observations are made: (a) Write a net ionic equation for the reaction that occurs in the first experiment. (b) Identify the precipitate formed in the first experiment. (c) Write a net ionic equation for the reaction that occurs in the third experiment. (d) Identify the precipitate formed in the third experiment. (e) Write a net ionic equation for the reaction that occurs in the fourth experiment. (f) Identify the precipitate formed in the fourth experiment. (g) Write a net ionic equation for the reaction that occurs in the fifth experiment. (h) Identify the precipitate formed in the fifth experiment. (i) Write a net ionic equation for the reaction that occurs in the sixth experiment. (j) Identify the precipitate formed in the sixth experiment.

Verified step by step guidance

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Step 1: Identify the ions present in each of the given 0.01 M solutions (A, B, C, D) based on the salts they contain.

Step 2: Use the solubility rules to determine which combinations of ions will form insoluble compounds, leading to the formation of a precipitate.

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Step 3: For each experiment, write the balanced chemical equation for the reaction, then derive the net ionic equation by removing the spectator ions.

Step 4: Identify the precipitate in each experiment by determining which product of the reaction is insoluble in water.

Step 5: Repeat steps 3 and 4 for each of the specified experiments to write the net ionic equations and identify the precipitates formed.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Solubility Rules

Solubility rules are guidelines that help predict whether a compound will dissolve in water. They categorize ions based on their solubility, indicating which combinations will form soluble or insoluble salts. For example, most alkali metal salts and nitrates are soluble, while many transition metal salts are often insoluble. Understanding these rules is crucial for determining the formation of precipitates in reactions.

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Solubility Rules

Net Ionic Equations

A net ionic equation represents the actual chemical species involved in a reaction, excluding spectator ions that do not participate in the reaction. It highlights the ions that form precipitates or undergo a change. Writing net ionic equations requires identifying the reactants, determining the products, and eliminating ions that remain unchanged. This concept is essential for accurately describing the reactions occurring in the experiments.

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Net Ionic Equations

Precipitation Reactions

Precipitation reactions occur when two aqueous solutions are mixed, resulting in the formation of an insoluble solid, known as a precipitate. This process is driven by the interactions between ions in solution, leading to the formation of a compound that cannot remain dissolved. Identifying the precipitate involves applying solubility rules to predict which products will be insoluble. Understanding these reactions is key to answering the questions about the experiments.

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Selective Precipitation

Related Practice

Textbook Question

The accompanying photo shows the reaction between a solution of Cd(NO₃)₂ and one of Na₂S. (b) What ions remain in solution?

Textbook Question

The accompanying photo shows the reaction between a solution of Cd(NO₃)₂ and one of Na₂S. (d) Is this a redox reaction?

Textbook Question

Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the aqueous HCl in the stomach and each of the following substances used in various antacids: (a) Al(OH)₃(s) (b) Mg(OH)₂(s) (c) MgCO₃(s) (d) NaAl(CO₃)(OH)₂(s) (e) CaCO₃(s).

Textbook Question

The commercial production of nitric acid involves the following chemical reactions:

4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g)

2 NO(g) + O₂(g) → 2 NO₂(g)

3 NO₂(g) + H₂O(l) → 2 HNO₃(aq) + NO(g)

(a) Which of these reactions are redox reactions?

Textbook Question

The commercial production of nitric acid involves the following chemical reactions:

4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g)

2 NO(g) + O₂(g) → 2 NO₂(g)

3 NO₂(g) + H₂O(l) → 2 HNO₃(aq) + NO(g)

(b) Identify the element undergoing oxidation and the element undergoing reduction.

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