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? ExplainCations: Na+, Ca2+, Ag+, Ni2+ Anions: Cl-, CO32-, 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.
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-.
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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