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Ch.5 - Introduction to Solutions and Aqueous Solutions
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.5 - Introduction to Solutions and Aqueous SolutionsProblem 49
Chapter 5, Problem 49

Determine whether each compound is soluble or insoluble. If the compound is soluble, list the ions present in solution. a. AgNO3 b. Pb(C2H3O2)2 c. KNO3 d. (NH4)2S

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Identify the solubility rules for common ionic compounds in water. Nitrates (NO_3^-) and acetates (C_2H_3O_2^-) are generally soluble, while sulfides (S^2-) are often insoluble except with certain cations.
For AgNO_3: According to solubility rules, nitrates are soluble. Therefore, AgNO_3 is soluble in water. The ions present in solution are Ag^+ and NO_3^-.
For Pb(C_2H_3O_2)_2: Acetates are generally soluble, so Pb(C_2H_3O_2)_2 is soluble in water. The ions present in solution are Pb^2+ and C_2H_3O_2^-.
For KNO_3: Nitrates are soluble, and potassium compounds are also soluble. Therefore, KNO_3 is soluble in water. The ions present in solution are K^+ and NO_3^-.
For (NH_4)_2S: Ammonium compounds are generally soluble, so (NH_4)_2S is soluble in water. The ions present in solution are NH_4^+ and S^2-.

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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 state that certain ions, such as alkali metal ions and nitrate ions, are generally soluble, while others, like lead(II) and silver ions, often form insoluble compounds. Understanding these rules is essential for determining the solubility of various compounds in aqueous solutions.
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Ionic Compounds in Solution

When ionic compounds dissolve in water, they dissociate into their constituent ions. For example, when silver nitrate (AgNO3) dissolves, it separates into Ag+ and NO3- ions. Recognizing how compounds break down into ions in solution is crucial for identifying the ions present in soluble compounds.
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Ammonium Compounds

Ammonium compounds, such as (NH4)2S, are typically soluble in water due to the presence of the ammonium ion (NH4+), which is known for its solubility. This concept is important when evaluating the solubility of compounds containing ammonium, as they often behave differently compared to other cations.
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Related Practice
Textbook Question

Determine whether each compound is soluble or insoluble. If the compound is soluble, list the ions present in solution. a. AgI b. Cu3(PO4)2 c. CoCO3 d. K3PO4

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Textbook Question

A 55.0-mL sample of a 0.102 M potassium sulfate solution is mixed with 35.0 mL of a 0.114 M lead(II) acetate solution and this precipitation reaction occurs: K2SO4(aq) + Pb(C2H3O2)2(aq) → 2 KC2H3O2(aq) + PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 1.01 g. Determine the limiting reactant, theoretical yield, percent yield.

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Textbook Question

Classify each compound as a strong electrolyte or nonelectrolyte. a. K2SO4 b. C6H12O6 c. K2CO3 d. CH3OH

Textbook Question

A 25.0-mL sample of a 1.20 M potassium chloride solution is mixed with 15.0 mL of a 0.900 M lead(II) nitrate solution and this precipitation reaction occurs: 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq) The solid PbCl2 is collected, dried, and found to have a mass of 2.45 g. Determine the the percent yield.

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Textbook Question

Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' a. LiI(aq) + BaS(aq)

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