Domanda del libro di testo
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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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 4, Problema 25c
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (c) ammonium phosphate and calcium chloride
Guida verificata passo dopo passo1
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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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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Percorso guidato
00:28
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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Percorso guidato
02:11Ionic Compounds Naming
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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Percorso guidato
01:53Selective Precipitation
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