Domanda del libro di testo
(b) What is the ratio of HCO3- to H2CO3 in an exhausted marathon runner whose blood pH is 7.1?
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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
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Brown 15th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 27c
Brown 15th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 27cCapitolo 17, Problema 27c
A buffer contains 0.10 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L. c. What is the pH of the buffer after the addition of 0.020 mol of HNO3?
Guida verificata passo dopo passo1
Step 1: Identify the components of the buffer system. The buffer consists of acetic acid (CH3COOH) and its conjugate base, sodium acetate (CH3COONa).
Step 2: Write the chemical equation for the reaction between the added HNO3 and the buffer. HNO3 will react with the acetate ion (CH3COO^-) to form acetic acid (CH3COOH) and nitrate ion (NO3^-).
Step 3: Calculate the moles of acetate ion (CH3COO^-) and acetic acid (CH3COOH) after the reaction with HNO3. Subtract the moles of HNO3 from the moles of acetate ion and add the same amount to the moles of acetic acid.
Step 4: Use the Henderson-Hasselbalch equation to find the pH of the buffer. The equation is pH = pKa + log([A^-]/[HA]), where [A^-] is the concentration of acetate ion and [HA] is the concentration of acetic acid.
Step 5: Substitute the values of pKa for acetic acid, and the concentrations of acetate ion and acetic acid into the Henderson-Hasselbalch equation to calculate the pH.
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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. In this case, acetic acid (a weak acid) and sodium acetate (its conjugate base) form a buffer that can maintain pH stability when acids or bases are introduced.
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Percorso guidato
03:02
Buffer Solutions
Henderson-Hasselbalch Equation
The Henderson-Hasselbalch equation is a mathematical formula used to calculate the pH of a buffer solution. It is expressed as pH = pKa + log([A-]/[HA]), where pKa is the negative logarithm of the acid dissociation constant, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the weak acid. This equation is essential for determining the pH after the addition of an acid or base.
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Percorso guidato
02:40Henderson-Hasselbalch Equation
Acid-Base Neutralization
When an acid is added to a buffer solution, it reacts with the conjugate base present in the buffer, leading to a neutralization reaction. In this scenario, the added HNO3 will react with sodium acetate, converting some of it into acetic acid. This reaction alters the concentrations of the acid and base in the buffer, which must be accounted for when calculating the new pH.
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Percorso guidato
05:04Lewis Acids and Bases
Pratica correlata
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You are asked to prepare a pH = 4.00 buffer starting from 1.50 L of 0.0200 M solution of benzoic acid 1C6H5COOH2 and any amount you need of sodium benzoate 1C6H5COONa2. (b) How many grams of sodium benzoate should be added to prepare the buffer? Neglect the small volume change that occurs when the sodium benzoate is added.
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Domanda del libro di testo
A buffer contains 0.10 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L. (a) What is the pH of this buffer?
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Domanda del libro di testo
A buffer contains 0.10 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L. b. What is the pH of the buffer after the addition of 0.020 mol of KOH?
Domanda del libro di testo
(a) What is the ratio of HCO3- to H2CO3 in blood of pH 7.4?
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