Domanda del libro di testo
A 100.0 mL sample of a solution that is 0.100 M in HCl and 0.100 M in HCN is titrated with 0.100 M NaOH. Calculate the pH after the addition of the following volumes of NaOH:
(a) 0.0 mL
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Ch.16 - Aqueous Equilibria: Acids & Bases
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 16, Problema 17.142
The acidity of lemon juice is derived primarily from citric acid (H3Cit), a triprotic acid. What are the concentrations of H3Cit, H2Cit-, HCit2-, and Cit3- in a sample of lemon juice that has a pH of 2.37 and a total concentration of the four citrate-containing species of 0.350 M?
Guida verificata passo dopo passo1
Identify the relevant acid dissociation constants (Ka) for citric acid (H3Cit). Citric acid is a triprotic acid, meaning it can donate three protons. The dissociation reactions are: H3Cit
ightarrow H2Cit^- + H^+, H2Cit^-
ightarrow HCit^{2-} + H^+, and HCit^{2-}
ightarrow Cit^{3-} + H^+.
Write the expression for the pH of the solution and relate it to the concentration of H+ ions. Since pH = -log[H+], calculate [H+] using the pH given (2.37).
Set up the equilibrium expressions for each dissociation step using the Ka values and the concentrations of H3Cit, H2Cit-, HCit2-, and Cit3-. Use the formula Ka = [Products]/[Reactants] for each step.
Since the total concentration of all citrate species (H3Cit, H2Cit-, HCit2-, Cit3-) is given as 0.350 M, use this information to set up an equation summing the concentrations of all species to equal 0.350 M.
Solve the system of equations derived from the equilibrium expressions and the total concentration equation to find the individual concentrations of H3Cit, H2Cit-, HCit2-, and Cit3-.
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Triprotic Acids
Triprotic acids, like citric acid, can donate three protons (H+) in a stepwise manner. Each deprotonation step has a distinct dissociation constant (Ka), which indicates the strength of the acid at each stage. Understanding the behavior of triprotic acids is crucial for calculating the concentrations of their various ionic forms in solution.
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Percorso guidato
6:47
Triprotic Acid Equilibrium
pH and Concentration Relationship
The pH of a solution is a measure of its hydrogen ion concentration, defined as pH = -log[H+]. In this case, a pH of 2.37 corresponds to a hydrogen ion concentration of approximately 0.0042 M. This relationship is essential for determining the concentrations of the different species of citric acid in lemon juice.
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Percorso guidato
02:09pH and pOH Calculations
Equilibrium and Species Concentration
In a solution containing a weak acid and its conjugate bases, the concentrations of the various species are determined by the acid dissociation equilibria. For citric acid, the total concentration of all species must equal the given total concentration (0.350 M), and the individual concentrations can be calculated using the equilibrium constants and the pH value.
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Percorso guidato
03:03Amphoteric Species
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