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Balance each redox reaction occurring in acidic aqueous solution. a. K(s) + Cr3+(aq) → Cr(s) + K+(aq) b. Al(s) + Fe2+(aq) → Al3+(aq) + Fe(s)
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Ch.20 - Electrochemistry
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Capitolo 20, Problema 13
A 0.0251-L sample of a solution of Cu+ requires 0.0322 L of 0.129 M KMnO4 solution to reach the equivalence point. The products of the reaction are Cu2+ and Mn2+. What is the concentration of the Cu+ solution?
Guida verificata passo dopo passo1
Identify the balanced chemical equation for the reaction: \[ 5 \text{Cu}^+ + \text{MnO}_4^- + 8\text{H}^+ \rightarrow 5\text{Cu}^{2+} + \text{Mn}^{2+} + 4\text{H}_2\text{O} \]
Calculate the moles of \( \text{KMnO}_4 \) used: \[ \text{moles of } \text{KMnO}_4 = 0.0322 \text{ L} \times 0.129 \text{ M} \]
Use the stoichiometry of the balanced equation to find the moles of \( \text{Cu}^+ \): \[ \text{moles of } \text{Cu}^+ = 5 \times \text{moles of } \text{KMnO}_4 \]
Calculate the concentration of \( \text{Cu}^+ \) in the original solution: \[ \text{Concentration of } \text{Cu}^+ = \frac{\text{moles of } \text{Cu}^+}{0.0251 \text{ L}} \]
Review the steps to ensure all calculations align with the stoichiometry and the given data.
Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to calculate the amounts of substances consumed and produced in a reaction based on balanced chemical equations. Understanding stoichiometry is essential for determining the concentration of solutions and the volumes of reactants needed to reach equivalence points in titrations.
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Percorso guidato
01:16
Stoichiometry Concept
Titration
Titration is a laboratory technique used to determine the concentration of a solute in a solution by reacting it with a solution of known concentration. The point at which the reaction is complete is called the equivalence point, which can be identified using indicators or pH meters. In this question, the titration of Cu+ with KMnO4 allows us to find the concentration of the Cu+ solution based on the volume and molarity of the titrant used.
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Percorso guidato
03:04Acid-Base Titration
Molarity
Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in units of moles per liter (M). In this problem, the molarity of the KMnO4 solution is crucial for calculating the moles of KMnO4 used in the titration, which can then be related to the moles of Cu+ in the original solution to find its concentration.
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Percorso guidato
01:13Molarity