Textbook Question
The following three solutions are mixed: 100.0 mL of 0.100 M Na2SO4, 50.0 mL of 0.300 M ZnCl2, and 100.0 mL of 0.200 M Ba(CN)2. (a) What ionic compounds will precipitate out of solution?
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Ch.4 - Reactions in Aqueous Solution
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 4, Problem 90b
How could you use a precipitation reaction to separate each of the following pairs of cations? Write the formula for each reactant you would add, and write a balanced net ionic equation for each reaction. (b)
Verified step by step guidance1
Identify the cations present in the solution and research their solubility properties with common anions to determine which anion will selectively precipitate one of the cations while leaving the other in solution.
Choose a suitable anion that will react with one of the cations to form an insoluble precipitate. The choice of anion depends on the solubility rules and the specific cations involved in the mixture.
Write the formula for the reactant (anion source) you would add to the solution to initiate the precipitation reaction. Ensure that the reactant is soluble in the solution to effectively release the anion.
Write the balanced molecular equation for the reaction between the chosen anion and the target cation, showing the formation of the precipitate.
Convert the molecular equation to a net ionic equation by eliminating the spectator ions and focusing on the ions that participate directly in the formation of the precipitate.
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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 solid, known as a precipitate. This process is driven by the formation of a compound 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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Selective Precipitation
Net Ionic Equations
A net ionic equation represents the actual chemical species involved in a reaction, excluding spectator ions that do not participate in the reaction. To write a net ionic equation, one must first write the balanced molecular equation, then dissociate the soluble ionic compounds into their constituent ions, and finally eliminate the spectator ions to focus on the ions that form the precipitate.
Cation Separation Techniques
Cation separation techniques involve using selective precipitation to isolate specific cations from a mixture. By adding a reagent that forms a precipitate with one cation while leaving others in solution, it is possible to separate and identify different cations. This method is commonly used in analytical chemistry for qualitative analysis of metal ions.
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Related Practice
Textbook Question
Assume that you have an aqueous solution of an unknown salt. Treatment of the solution with dilute NaOH, Na2SO4, and KCl produces no precipitate. Which of the following cations might the solution contain?(a) Ag+(b) Cs+(c) Ba2+(d) NH4 +
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Textbook Question
How could you use a precipitation reaction to separate each of the following pairs of anions? Write the formula for each reactant you would add, and write a balanced net ionic equation for each reaction.(a)
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Textbook Question
The following three solutions are mixed: 100.0 mL of 0.100 M Na2SO4, 50.0 mL of 0.300 M ZnCl2, and 100.0 mL of 0.200 M Ba(CN)2. (b) What is the molarity of each ion remaining in the solution assuming complete precipitation of all insoluble compounds?
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Textbook Question
Assume that you have an aqueous solution of an unknown salt. Treatment of the solution with dilute BaCl2, AgNO3, and Cu(NO3)2 produces no precipitate. Which of the following anions might the solution contain?(a) Cl-(b) NO3 (c) OH-(d) SO4- 2-
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Textbook Question
Assume that you have an aqueous mixture of BaCl2 and CuCl2. How could you use a precipitation reaction to sepa-rate the two metal ions?
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