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 25c
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (c) ammonium phosphate and calcium chloride
Verified step by step guidance1
Step 1: Write down the chemical formulas for the reactants. Ammonium phosphate is (NH4)3PO4 and calcium chloride is CaCl2.
Step 2: Predict the possible products of the reaction using the principle of 'cation-anion' exchange. The possible products are ammonium chloride (NH4Cl) and calcium phosphate (Ca3(PO4)2).
Step 3: Check the solubility rules to determine if any of the products will precipitate. According to the solubility rules, all ammonium salts (NH4+) are soluble, so ammonium chloride will not precipitate. However, most phosphate salts are insoluble, with some exceptions including salts of ammonium (NH4+). Therefore, calcium phosphate will precipitate.
Step 4: Since calcium phosphate precipitates, the calcium ions (Ca2+) from calcium chloride will react and will not remain in the solution. However, the chloride ions (Cl-) from calcium chloride will not react and will remain in the solution.
Step 5: Similarly, the phosphate ions (PO4^3-) from ammonium phosphate will react and will not remain in the solution. However, the ammonium ions (NH4+) from ammonium phosphate will not react and will remain in the solution.
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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. For example, most ammonium salts and phosphates are soluble, while many calcium salts can be insoluble. Understanding these rules is crucial for determining which ions remain in solution after mixing different ionic compounds.
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Solubility Rules
Ionic Compounds and Dissociation
Ionic compounds dissociate into their constituent ions when dissolved in water. For instance, ammonium phosphate dissociates into ammonium (NH4+) and phosphate (PO4^3-) ions, while calcium chloride dissociates into calcium (Ca^2+) and chloride (Cl-) ions. Recognizing how these compounds break apart in solution is essential for analyzing the resulting mixture.
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Precipitation Reactions
A precipitation reaction occurs when two soluble ionic compounds react to form an insoluble compound, or precipitate. In the case of mixing ammonium phosphate and calcium chloride, calcium phosphate may precipitate out of solution. Identifying which ions remain unreacted involves understanding the potential for precipitation based on solubility product constants.
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Related Practice
Textbook Question
Separate samples of a solution of an unknown ionic compound are treated with dilute AgNO3, Pb1NO322, and BaCl2. Precipitates form in all three cases. Which of the following could be the anion of the unknown salt: Br-, CO32-, NO3-?
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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
Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. a. Cr2(SO4)3(ππ)+(NH4)2CO3(ππ)βΆ
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Textbook Question
Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. c. Fe(NO3)2(ππ)+KOH(ππ)βΆ
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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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