Domanda del libro di testo
Match the following descriptions of titration curves with the diagrams: (a) strong acid added to strong base. [Section 17.3]
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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 4a
The following diagram represents a buffer composed of equal concentrations of a weak acid, HA, and its conjugate base, A-. The heights of the columns are proportional to the concentrations of the components of the buffer. (a) Which of the three drawings, (1), (2), or (3), represents the buffer after the addition of a strong acid? [Section 17.2]
Guida verificata passo dopo passo1
Identify the components of the buffer: a weak acid (HA) and its conjugate base (A-).
Understand that adding a strong acid to the buffer will increase the concentration of H+ ions.
Recognize that the added H+ ions will react with the conjugate base (A-) to form more of the weak acid (HA).
Determine that the concentration of the conjugate base (A-) will decrease, while the concentration of the weak acid (HA) will increase.
Look for the drawing where the column representing HA is taller and the column representing A- is shorter compared to the original buffer.
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Buffer Solutions
A buffer solution is a system that resists changes in pH upon the addition of small amounts of acid or base. It typically consists of a weak acid and its conjugate base in equilibrium. This equilibrium allows the buffer to neutralize added acids or bases, maintaining a relatively stable pH.
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03:02
Buffer Solutions
Weak Acids and Conjugate Bases
Weak acids partially dissociate in solution, establishing an equilibrium between the undissociated acid (HA) and its ions (H+ and A-). The conjugate base (A-) can react with added H+ ions from a strong acid, minimizing the change in pH. Understanding this equilibrium is crucial for predicting how a buffer will respond to external changes.
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01:46Conjugate Acid-Base Relationships
Effect of Strong Acid on Buffer
When a strong acid is added to a buffer solution, it increases the concentration of H+ ions. The weak acid component of the buffer will react with these H+ ions, shifting the equilibrium and converting some of the conjugate base (A-) into more weak acid (HA). This process helps to mitigate the pH change, but the buffer's capacity is limited and can be overwhelmed if too much strong acid is added.
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01:14Effective Buffer Range
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Domanda del libro di testo
The following diagram represents a buffer composed of equal concentrations of a weak acid, HA, and its conjugate base, A-. The heights of the columns are proportional to the concentrations of the components of the buffer. (c) Which of the three represents a situation that cannot arise from the addition of either an acid or a base? [Section 17.2]
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Domanda del libro di testo
The following figure represents solutions at various stages of the titration of a weak acid, HA, with NaOH. (The Na+ ions and water molecules have been omitted for clarity.) To which of the following regions of the titration curve does each drawing correspond: (b) after addition of NaOH but before the equivalence point? [Section 17.3]
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Domanda del libro di testo
The beaker on the right contains 0.1 M acetic acid solution with methyl orange as an indicator. The beaker on the left contains a mixture of 0.1 M acetic acid and 0.1 M sodium acetate with methyl orange. (a) Using Figures 16.8 and 16.9, which solution has a higher pH?
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Domanda del libro di testo
The beaker on the right contains 0.1 M acetic acid solution with methyl orange as an indicator. The beaker on the left contains a mixture of 0.1 M acetic acid and 0.1 M sodium acetate with methyl orange. (b) Which solution is better able to maintain its pH when small amounts of NaOH are added? Explain. [Sections 17.1 and 17.2]
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Domanda del libro di testo
A buffer contains a weak acid, HA, and its conjugate base. The weak acid has a pKa of 4.5, and the buffer has a pH of 4.3. Without doing a calculation, state which of these possibilities are correct at pH 4.3. (a) 3HA4 = 3A-4, (b) 3HA4 7 3A-4, or (c) 3HA4 6 3A-4. [Section 17.2]
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