Domanda del libro di testo
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)
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Ch.4 - Reactions in Aqueous Solution
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Capitolo 4, Problema 92b
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?
Guida verificata passo dopo passo1
Calculate the initial moles of each ion in the solutions. For Na2SO4, use the formula: moles = molarity \(\times\) volume (in liters). Do the same for ZnCl2 and Ba(CN)2.
Write down the possible precipitation reactions that could occur based on the ions present in the solutions. Consider the solubility rules to determine which compounds are likely to precipitate.
For each potential precipitate, use the stoichiometry of the reaction to determine how many moles of each ion would be needed to form the precipitate. Compare this to the moles available in the solution to find the limiting reactant.
Subtract the moles of ions that precipitate from the initial moles to find the moles of each ion remaining in the solution.
Calculate the final molarity of each ion by dividing the remaining moles of each ion by the total volume of the solution in liters.
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Molarity
Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (M) and is crucial for calculating the amounts of ions present in a solution after mixing different solutions. Understanding molarity allows for the determination of how much of each ion will remain in the solution after any reactions, such as precipitation.
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01:13
Molarity
Precipitation Reactions
Precipitation reactions occur when two soluble salts react in solution to form an insoluble compound, or precipitate. This process is essential in the context of the question, as it determines which ions will remain in solution and which will form solid precipitates. Identifying the solubility rules helps predict the formation of precipitates and the resulting concentrations of ions in the final solution.
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01:53Selective Precipitation
Stoichiometry
Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced chemical equations. It is vital for determining the amounts of ions produced or consumed during reactions, including precipitation. By applying stoichiometric principles, one can calculate the remaining concentrations of ions after the complete precipitation of insoluble compounds in the mixed solutions.
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01:16Stoichiometry Concept
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Assume that you are given a solution of an unknown acid or base. How can you tell whether the unknown substance is acidic or basic?
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Domanda del libro di testo
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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Domanda del libro di testo
(b) What is the mass of each substance in the original 250 g mixture?
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Domanda del libro di testo
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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Domanda del libro di testo
A 250.0 g sample of a white solid is known to be a mixture of KNO3, BaCl2, and NaCl. When 100.0 g of this mixture is dis-solved in water and allowed to react with excess H2SO4, 67.3 g of a white precipitate is collected. When the remaining 150.0 g of the mixture is dissolved in water and allowed to react with excess AgNO3, 197.6 g of a second precipitate is collected. (a) What are the formulas of the two precipitates?
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