Ch.4 - Reactions in Aqueous Solution

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

McMurry 8th Edition

Ch.4 - Reactions in Aqueous Solution

Problem 39

Chapter 4, Problem 39

Assume that an aqueous solution of a cation, represented as a blue sphere, is allowed to mix with a solution of an anion, repre-sented as a red sphere, and that the following result is obtained: Which combinations of cation and anion, chosen from the fol-lowing lists, are compatible with the observed results? Explain Cations: Na+, Ca2+, Ag+, Ni2+ Anions: Cl-, CO3 2-, CrO4 2-, NO3

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Identify the possible products formed by combining each cation with each anion. For example, combining Na+ with Cl- would yield NaCl.

Consider the solubility rules for each potential product. Soluble compounds will remain in solution and not form a precipitate, while insoluble compounds will form a precipitate.

Check for any color indications that might be associated with the ions or the precipitates formed. For instance, CrO4 2- typically forms a yellow precipitate, which could be a clue if a yellow color is observed in the experiment.

Match the observed results from the experiment (such as color of the solution, presence of precipitate) with the expected outcomes based on the solubility and color of the products formed.

Eliminate combinations where the expected outcome does not match the observed results, and confirm the combinations where the expected outcome aligns with the observations.

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Key Concepts

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

Ionic Compounds and Solubility

Ionic compounds are formed from the electrostatic attraction between cations and anions. The solubility of these compounds in water depends on the nature of the ions involved. Some combinations of cations and anions will form soluble compounds, while others may precipitate out of solution. Understanding solubility rules helps predict which combinations will remain in solution.

Charge Balance in Ionic Compounds

In ionic compounds, the total positive charge from cations must balance the total negative charge from anions. This charge neutrality is essential for the stability of the compound. For example, a divalent cation like Ca2+ requires two monovalent anions like Cl- to achieve charge balance, while a monovalent cation like Na+ can pair with one Cl-.

Common Ion Effect and Precipitation

The common ion effect refers to the decrease in solubility of an ionic compound when a common ion is added to the solution. This can lead to precipitation, where the solid form of the compound separates from the solution. Identifying whether the mixing of specific cations and anions leads to precipitation is crucial for determining compatibility in the observed results.

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Common Ion Effect

Related Practice

Textbook Question

Assume that an aqueous solution of OH-, represented as a blue sphere, is allowed to mix with a solution of an acid HnA, represented as a red sphere. Three possible outcomes are depicted by boxes (1)–(3), where the green spheres represent An-, the anion of the acid: Which outcome corresponds to each of the following reactions? (a) (b) (c)

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Textbook Question

The concentration of an aqueous solution of NaOCl (sodium hypochlorite; the active ingredient in household bleach) can be determined by a redox titration with iodide ion in acidic solution:

Assume that the blue spheres in the buret represent I-ions, the red spheres in the flask represent OCl-ions, the con-centration of the I-ions in the buret is 0.120 M, and the volumes in the buret and the flask are identical. What is the concentration of NaOCl in the flask? What percentage of the I-solution in the buret must be added to the flask to react with all the OCl-ions?

Textbook Question

Box (a) represents 1.0 mL of a solution of particles at a given concentration. Which of the boxes (b)–(d) represents 1.0 mL of the solution that results after (a) has been diluted by doubling the volume of its solvent? (a)

(b)

(c)

(d)

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Textbook Question

Assume that an aqueous solution of a cation, represented as a red sphere, is allowed to mix with a solution of an anion, represented as a yellow sphere. Three possible outcomes are represented by boxes (1)–(3):

Which outcome corresponds to each of the following reactions? (a) 2 Na+(aq) + CO32-(aq) S (b) Ba2+(aq) + CrO42-(aq) S (c) 2 Ag+(aq) + SO32-(aq) S

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Textbook Question

The concentration of a solution of potassium permanganate, KMnO4, can be determined by titration with a known amount of oxalic acid, H2C2O4, according to the following equation: What is the concentration of a KMnO4 solution if 22.35 mL reacts with 0.5170 g of oxalic acid? (LO 4.22) (a) 0.6423 M (b) 0.1028 M (c) 0.4161 M (d) 0.2569 M

Textbook Question

The following pictures represent aqueous solutions of three acids HA (A = X, Y, or Z), with surrounding water mol-ecules omitted for clarity. Which of the three is the strongest acid, and which is the weakest?