Domanda del libro di testo
Identify each substance as an acid or a base and write a chemical equation showing how it is an acid or a base according to the Arrhenius definition. a. HNO3(aq) b. NH4+(aq) d. HC2H3O2(aq)
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Ch.16 - Acids and Bases
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Capitolo 16, Problema 9
Determine the concentrations of OH-, pH, and pOH of a solution that is 0.125 M in CO32-.
Guida verificata passo dopo passo1
Identify the relevant equilibrium reactions for carbonate ion (\( \text{CO}_3^{2-} \)) in water: \( \text{CO}_3^{2-} + \text{H}_2\text{O} \rightleftharpoons \text{HCO}_3^{-} + \text{OH}^- \).
Use the equilibrium constant expression for the reaction: \( K_b = \frac{[\text{HCO}_3^-][\text{OH}^-]}{[\text{CO}_3^{2-}]} \).
Assume initial concentration of \( \text{CO}_3^{2-} \) is 0.125 M and set up an ICE table to find changes in concentration at equilibrium.
Solve for \([\text{OH}^-]\) using the equilibrium expression and the known \( K_b \) value for carbonate ion.
Calculate pOH from \([\text{OH}^-]\) using the formula \( \text{pOH} = -\log[\text{OH}^-] \) and then find pH using \( \text{pH} = 14 - \text{pOH} \).
Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Carbonate Ion Chemistry
The carbonate ion (CO32-) is a polyatomic ion that can act as a base in aqueous solutions. It can accept protons (H+) to form bicarbonate (HCO3-), which is crucial for understanding its role in acid-base equilibria. The presence of CO32- in a solution will influence the concentrations of hydroxide ions (OH-) and the overall pH of the solution.
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Percorso guidato
06:17
Ion Formation
pH and pOH Calculations
pH is a measure of the hydrogen ion concentration in a solution, while pOH measures the hydroxide ion concentration. They are related through the equation pH + pOH = 14 at 25°C. Understanding how to calculate pH and pOH from ion concentrations is essential for determining the acidity or basicity of a solution.
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Percorso guidato
02:09pH and pOH Calculations
Equilibrium Constants and Ionization
The ionization of carbonate ions involves equilibrium constants such as Kb for the reaction with water to form hydroxide ions. The concentration of OH- can be derived from the equilibrium expression, which relates the concentrations of the reactants and products at equilibrium. This concept is vital for calculating the resulting pH and pOH of the solution.
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Percorso guidato
01:14Equilibrium Constant K