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Ch.4 - Chemical Quantities & Aqueous Reactions
All textbooksTro 4th EditionCh.4 - Chemical Quantities & Aqueous ReactionsProblem 73
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Chapter 4, Problem 73

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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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

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

For each compound (all water soluble), would you expect the resulting aqueous solution to conduct electrical current? a. CsCl b. CH3OH c. Ca(NO2)2 d. C6H12O6

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Classify each compound as a strong electrolyte or nonelectrolyte. a. MgBr2 b. C12H22O11 c. Na2CO3 d. KOH

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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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Open Question
Complete and balance the following equation. If no reaction occurs, write “NO REACTION.” NaOH(aq) + FeCl3(aq) → ?
Textbook Question

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

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