Domanda del libro di testo
Determine whether or not the mixing of each pair of solutions results in a buffer. b.155.0 mL of 0.15 M NH3 ; 155.0 mL of 0.10 M HCl
Ch.18 - Aqueous Ionic Equilibrium
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
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Capitolo 18, Problema 56d
Determine whether or not the mixing of each pair of solutions results in a buffer. d. 150.0 mL of 0.15 M HCl; 135.0 mL of 0.25 M NaOH
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Identify the components needed for a buffer solution: a weak acid and its conjugate base, or a weak base and its conjugate acid.
Recognize that HCl is a strong acid and NaOH is a strong base, neither of which are suitable for forming a buffer directly.
Calculate the moles of HCl: \( \text{moles of HCl} = 0.15 \, \text{M} \times 0.150 \, \text{L} \).
Calculate the moles of NaOH: \( \text{moles of NaOH} = 0.25 \, \text{M} \times 0.135 \, \text{L} \).
Determine if there is an excess of either HCl or NaOH after the reaction, as a buffer requires a weak acid/base and its conjugate pair, not excess strong acid or base.
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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 or a weak base and its conjugate acid. Buffers are crucial in maintaining stable pH levels in various chemical and biological processes.
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03:02
Buffer Solutions
Strong Acids and Bases
Strong acids, like HCl, completely dissociate in water, releasing all their hydrogen ions (H+), while strong bases, like NaOH, completely dissociate to release hydroxide ions (OH-). The complete dissociation of these substances means they do not contribute to the buffering capacity, as they do not exist in equilibrium with their conjugate forms.
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01:09Strong Acid-Strong Base Titration
Neutralization Reaction
A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this case, HCl and NaOH will react to form water and sodium chloride (NaCl). The resulting solution's pH will depend on the relative amounts of acid and base, and if they are present in stoichiometric amounts, the solution will be neutral, not a buffer.
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05:56Lewis Dot Structures: Neutral Compounds
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