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 56a
Determine whether or not the mixing of each pair of solutions results in a buffer. a. 155.0 mL of 0.15 M NH3 ; 175.0 mL of 0.17 M HCl
Guida verificata passo dopo passo1
Identify the components needed for a buffer solution: a weak base and its conjugate acid, or a weak acid and its conjugate base.
Recognize that NH3 (ammonia) is a weak base and HCl (hydrochloric acid) is a strong acid.
Calculate the moles of NH3 using the formula: moles = concentration (M) × volume (L).
Calculate the moles of HCl using the formula: moles = concentration (M) × volume (L).
Determine if the reaction between NH3 and HCl will result in a buffer by checking if there is an excess of NH3 after the reaction, which would leave a mixture of NH3 and NH4+ (the conjugate acid).
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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 maintain pH stability, which is crucial in many chemical and biological processes.
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03:02
Buffer Solutions
Weak Bases and Strong Acids
In the given question, NH3 (ammonia) is a weak base, while HCl (hydrochloric acid) is a strong acid. When mixed, the weak base can partially neutralize the strong acid, but the resulting solution may not form a buffer unless there is a sufficient amount of the weak base to react with the strong acid.
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01:09Strong Acid-Strong Base Titration
Stoichiometry of Acid-Base Reactions
Stoichiometry involves the calculation of reactants and products in chemical reactions. In this context, it is essential to determine the moles of NH3 and HCl to assess whether they can react completely or if excess amounts of either component will remain, influencing the ability to form a buffer solution.
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01:09Acid-Base Reaction
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