Domanda del libro di testo
Suggest how the cations in each of the following solution mixtures can be separated: (c) Pb2 + and Al3 +.
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Ch.17 - Additional Aspects of Aqueous Equilibria
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 17, Problema 84
Rainwater is acidic because CO21g2 dissolves in the water, creating carbonic acid, H2CO3. If the rainwater is too acidic, it will react with limestone and seashells (which are principally made of calcium carbonate, CaCO3). Calculate the concentrations of carbonic acid, bicarbonate ion 1HCO3-2 and carbonate ion 1CO32 - 2 that are in a raindrop that has a pH of 5.60, assuming that the sum of all three species in the raindrop is 1.0 * 10-5 M.
Guida verificata passo dopo passo1
Identify the relevant chemical equilibria: CO2 dissolves in water to form H2CO3, which can dissociate into HCO3^- and CO3^2-. The equilibria are: CO2 + H2O ⇌ H2CO3, H2CO3 ⇌ H^+ + HCO3^-, and HCO3^- ⇌ H^+ + CO3^2-.
Use the given pH to find the concentration of H^+ ions in the solution. Since pH = -log[H^+], calculate [H^+] from the pH of 5.60.
Apply the equilibrium expressions for the dissociation of H2CO3 into HCO3^- and CO3^2-. Use the known equilibrium constants for these reactions: K_a1 for H2CO3 ⇌ H^+ + HCO3^- and K_a2 for HCO3^- ⇌ H^+ + CO3^2-.
Set up the mass balance equation: [H2CO3] + [HCO3^-] + [CO3^2-] = 1.0 \(\times\) 10^{-5} M, which represents the total concentration of carbonic acid species in the raindrop.
Solve the system of equations using the equilibrium expressions and the mass balance equation to find the concentrations of H2CO3, HCO3^-, and CO3^2-.
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Acid-Base Chemistry
Acid-base chemistry involves the study of acids, bases, and their reactions. Acids donate protons (H+) in solution, while bases accept protons. The pH scale measures the acidity or basicity of a solution, with lower pH values indicating higher acidity. Understanding these principles is crucial for analyzing the behavior of carbonic acid in rainwater and its impact on the environment.
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Percorso guidato
02:00
Arrhenius Acids and Bases
Carbonic Acid Equilibrium
Carbonic acid (H2CO3) is a weak acid that exists in equilibrium with bicarbonate (HCO3-) and carbonate ions (CO32-). The equilibrium can be represented by the following reactions: H2CO3 ⇌ HCO3- + H+ and HCO3- ⇌ CO32- + H+. The pH of the solution influences the distribution of these species, making it essential to understand this equilibrium when calculating their concentrations in acidic rainwater.
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6:47Triprotic Acid Equilibrium
Concentration Calculations
Concentration calculations involve determining the amount of a substance in a given volume of solution, typically expressed in molarity (M). In this context, the total concentration of carbonic acid, bicarbonate, and carbonate ions is given as 1.0 * 10-5 M. Using the pH to find the concentration of H+ ions allows for the application of equilibrium expressions to calculate the individual concentrations of the species present in the raindrop.
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07:35Calculate Concentration of the Basic Form
Pratica correlata
Domanda del libro di testo
(b) What is the most significant difference between the sulfides precipitated in group 2 and those precipitated in group 3?
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Domanda del libro di testo
The acid–base indicator bromcresol green is a weak acid. The yellow acid and blue base forms of the indicator are present in equal concentrations in a solution when the pH is 4.68. What is the pKa for bromcresol green?
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Domanda del libro di testo
Which of these equations relates the pOH of a buffer to the p𝐾𝑏 of its weak base, analogous to the Henderson–Hasselbalch equation for weak acids?
a. p𝐾𝑏=pOH+p𝐾𝑏=pOH+log[acid]/[base]
b. p𝐾𝑏=pOH−log[acid]/[base]
c. p𝐾𝑏=pOH−log[base]/[acid]
d. p𝐾𝑏=pOH+log[base]/[[acid]