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A 100.0-mL buffer solution is 0.175 M in HClO and 0.150 M in NaClO. c. What is the pH after addition of 85.0 mg of NaOH?
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Ch.17 - Aqueous Ionic Equilibrium
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Capitolo 17, Problema 48a
A 100.0-mL buffer solution is 0.175 M in HClO and 0.150 M in NaClO. a. What is the initial pH of this solution?
Guida verificata passo dopo passo1
Step 1: Identify the acid and its conjugate base in the buffer solution. In this case, HClO is the weak acid and ClO- (from NaClO) is its conjugate base.
Step 2: Use the Henderson-Hasselbalch equation to calculate the pH of the buffer solution. The equation is pH = pKa + log([A-]/[HA]), where [A-] is the molarity of the base (ClO-) and [HA] is the molarity of the acid (HClO).
Step 3: Look up the Ka value for HClO in a table of acid dissociation constants. Then, calculate the pKa by taking the negative logarithm of the Ka value.
Step 4: Substitute the values of pKa, [A-], and [HA] into the Henderson-Hasselbalch equation to calculate the pH.
Step 5: If the pH is less than 7, the solution is acidic. If the pH is greater than 7, the solution is basic. If the pH is 7, the solution is neutral. In this case, since we have a buffer solution, the pH should be close to the pKa value of the weak acid.
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Buffer Solutions
Buffer solutions are mixtures that resist changes in pH when small amounts of acid or base are added. They typically consist of a weak acid and its conjugate base, or a weak base and its conjugate acid. In this case, the buffer is made up of hypochlorous acid (HClO) and sodium hypochlorite (NaClO), which work together to maintain the pH of the solution.
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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 [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 of the given buffer solution containing HClO and NaClO.
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02:40Henderson-Hasselbalch Equation
pKa and Acid-Base Equilibria
pKa is the negative logarithm of the acid dissociation constant (Ka) and indicates the strength of an acid in solution. A lower pKa value signifies a stronger acid. Understanding the pKa of HClO is crucial for applying the Henderson-Hasselbalch equation to find the initial pH of the buffer solution, as it reflects the equilibrium between the acid and its conjugate base.
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04:30Acid-Base Indicators