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Ch.4 - Reactions in Aqueous Solution
All textbooksBrown 14th EditionCh.4 - Reactions in Aqueous SolutionProblem 94
Chapter 4, Problem 94

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
1
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.
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.
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?

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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?

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Open Question
Suppose you have a solution that might contain any or all of the following cations: Ni2+, Ag+, Sr2+, and Mn2+. Addition of HCl solution causes a precipitate to form. After filtering off the precipitate, H2SO4 solution is added to the resulting solution and another precipitate forms. This is filtered off, and a solution of NaOH is added to the resulting solution. No precipitate is observed. Which of the four ions listed above must be absent from the original solution?
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: (d) NaAl1CO3)1OH221s2

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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?

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

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