Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Use the solubility rules to determine which are soluble.KCl                                    HClNH3                                   Ca(OH)    2CO2                                   PbSMgBr2       

Problem

Use the solubility rules to determine which are soluble.

KCl                                    HCl

NH3                                   Ca(OH)    2

CO2                                   PbS

MgBr2                                HC   2H3O2

The majority of ionic substances are solids at room temperature. Describe what you would observe if you placed a soluble ionic compound and an insoluble ionic compound in separate beakers of water.

Solution

Establish the solubility rules to determine which compound will be soluble and not.

Step 1. Recall the solubility rules:

  • Ionic compounds are usually composed of a nonmetal and a metal. 
  • On the other hand, molecular compounds are composed of exclusively non-metals
  • Note that molecular compounds cannot be analyzed as soluble or insoluble using the solubility rules.
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