Textbook Question
Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. b. KOH and Cu(NO3)2
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Ch.4 - Reactions in Aqueous Solution
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 4, Problem 21
Using solubility guidelines, predict whether each of the following compounds is soluble or insoluble in water: (a) MgBr2 (b) NH4OH (c) Ni(CH3COO)2 (d) AgNO3 (e) FeCO3.
Verified step by step guidance1
Step 1: Understand the solubility rules. Some of the key rules are: (1) All nitrates (NO3-) are soluble. (2) All salts of alkali metals (Group 1 elements) and ammonium (NH4+) are soluble. (3) All chlorides (Cl-), bromides (Br-), and iodides (I-) are soluble, except those of silver (Ag+), lead (Pb2+), and mercury (Hg2+). (4) All sulfates (SO4^2-) are soluble, except those of barium (Ba2+), strontium (Sr2+), lead (Pb2+), calcium (Ca2+), silver (Ag+), and mercury (Hg2+).
Step 2: Identify the ions in the compound. In this case, MgBr2 is made up of Mg2+ and Br- ions.
Step 3: Apply the solubility rules to the ions in the compound. According to the rules, all bromides (Br-) are soluble except those of silver (Ag+), lead (Pb2+), and mercury (Hg2+). Since Mg2+ is not one of the exceptions, MgBr2 is soluble in water.
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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 a set of guidelines used to predict whether ionic compounds will dissolve in water. These rules take into account the nature of the ions involved, such as their charge and size, and categorize them into soluble and insoluble groups. For example, most salts containing alkali metal ions or ammonium ions are soluble, while many metal hydroxides and carbonates are generally insoluble.
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Solubility Rules
Ionic Compounds
Ionic compounds are formed from the electrostatic attraction between positively charged cations and negatively charged anions. Their solubility in water depends on the strength of these ionic bonds compared to the interactions with water molecules. Compounds like MgBr<sub>2</sub> consist of magnesium cations and bromide anions, and their solubility can be assessed using established solubility rules.
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Hydration Energy
Hydration energy refers to the energy released when ions are surrounded by water molecules. This process is crucial for the dissolution of ionic compounds in water. If the hydration energy is greater than the lattice energy (the energy holding the ions together in the solid), the compound will dissolve. For MgBr<sub>2</sub>, the hydration energy of the magnesium and bromide ions plays a significant role in determining its solubility.
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Related Practice
Textbook Question
Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH4Cl, is a strong electrolyte. (a) What are the solutes present in aqueous solutions of each compound? What solute particles are present in an aqueous solution of HClO?
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Textbook Question
Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH4Cl, is a strong electrolyte. (b) If 0.1 mol of each compound is dissolved in solution, which one contains 0.2 mol of solute particles, which contains 0.1 mol of solute particles, and which contains somewhere between 0.1 and 0.2 mol of solute particles?
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Textbook Question
Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH4Cl, is a strong electrolyte. (a) What are the solutes present in aqueous solutions of each compound? What solute particles are present in an aqueous solution of CH3COCH3?
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Textbook Question
Predict whether each of the following compounds is soluble in water: d. Al(OH)3
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Textbook Question
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (a) potassium carbonate and magnesium sulfate
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