Textbook Question
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (c) ammonium phosphate and calcium chloride
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Ch.4 - Reactions in Aqueous Solution
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 4, Problem 29
You know that an unlabeled bottle contains an aqueous solutionof one of the following: AgNO3, CaCl2, or Al21SO423. Afriend suggests that you test a portion of the solution withBa1NO322 and then with NaCl solutions. According to yourfriend's logic, which of these chemical reactions could occur,thus helping you identify the solution in the bottle?(a) Barium sulfate could precipitate. (b) Silver chloridecould precipitate. (c) Silver sulfate could precipitate.(d) More than one, but not all, of the reactions described inanswers a–c could occur. (e) All three reactions described inanswers a–c could occur.
Verified step by step guidance1
Identify the possible reactions with Ba(NO_3)_2: Ba(NO_3)_2 can react with SO_4^{2-} to form BaSO_4, a precipitate, if the solution contains Al_2(SO_4)_3.
Identify the possible reactions with NaCl: NaCl can react with Ag^+ to form AgCl, a precipitate, if the solution contains AgNO_3.
Consider the solubility rules: BaSO_4 and AgCl are both insoluble in water, leading to precipitation, while Ag_2SO_4 is slightly soluble.
Evaluate the possible outcomes: If BaSO_4 precipitates, the solution is Al_2(SO_4)_3. If AgCl precipitates, the solution is AgNO_3.
Determine the correct answer: Based on the reactions, both (a) and (b) could occur, so the correct choice is (d) More than one, but not all, of the reactions described in answers a–c could occur.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Precipitation Reactions
Precipitation reactions occur when two soluble salts react in solution to form an insoluble compound, known as a precipitate. This process is driven by the formation of a product that is less soluble than the reactants, leading to its separation from the solution. Understanding the solubility rules helps predict which combinations of ions will result in a precipitate.
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Solubility Rules
Solubility rules are guidelines that help predict whether a compound will dissolve in water. For example, most sulfates are soluble, except for those of barium, lead, and calcium, while chlorides are generally soluble except for silver and lead. Knowing these rules is essential for determining which reactions will produce precipitates in the given scenario.
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Ionic Compounds and Their Reactions
Ionic compounds, such as AgNO3, CaCl2, and Al2(SO4)3, dissociate into their constituent ions in aqueous solutions. When mixed with other ionic solutions, these ions can recombine to form new compounds. Identifying the ions present in the original solution allows for predicting possible reactions with Ba(NO3)2 and NaCl, leading to the formation of precipitates like barium sulfate or silver chloride.
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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
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) Ba(OH)2(aq) + FeCl3(aq) →
(b) ZnCl2(aq) + Cs2CO3(aq) →
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Textbook Question
State whether each of the following statements is true or false. Justify your answer in each case. (b) HCl is a weak acid.
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Textbook Question
State whether each of the following statements is true or false. Justify your answer in each case. (a) Sulfuric acid is a monoprotic acid.
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Textbook Question
State whether each of the following statements is true or false. Justify your answer in each case. (c) Methanol is a base.
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