Domanda del libro di testo
A 35.0-mL sample of 0.150 M acetic acid 1CH3COOH2 is titrated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added: (b) 17.5 mL.
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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 44d,e
Brown 15th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 44d,eCapitolo 17, Problema 44d,e
A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: (d) 25.0 mL. (e) 30.0 mL.
Guida verificata passo dopo passo1
Step 1: Begin by calculating the initial moles of KOH in the 20.0 mL sample. Use the formula: \( \text{moles} = \text{volume (L)} \times \text{molarity (M)} \). Convert 20.0 mL to liters by dividing by 1000.
Step 2: Calculate the moles of HClO4 added for each volume (25.0 mL and 30.0 mL). Use the same formula: \( \text{moles} = \text{volume (L)} \times \text{molarity (M)} \). Convert the volumes from mL to liters.
Step 3: Determine the reaction between KOH and HClO4. The balanced chemical equation is: \( \text{KOH} + \text{HClO4} \rightarrow \text{KClO4} + \text{H2O} \). This is a 1:1 reaction, meaning one mole of KOH reacts with one mole of HClO4.
Step 4: For each volume of HClO4 added, calculate the remaining moles of KOH or HClO4 after the reaction. Subtract the moles of HClO4 from the initial moles of KOH to find the excess reactant.
Step 5: Calculate the pH based on the excess reactant. If KOH is in excess, calculate the concentration of OH⁻ ions and use \( \text{pOH} = -\log[\text{OH}^-] \) to find pH. If HClO4 is in excess, calculate the concentration of H⁺ ions and use \( \text{pH} = -\log[\text{H}^+] \).
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Titration
Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant (in this case, HClO4) to a solution of the analyte (KOH) until the reaction reaches its equivalence point, where the amount of titrant added is stoichiometrically equivalent to the amount of analyte present.
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03:04
Acid-Base Titration
pH Calculation
pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. In titration problems, pH can be calculated at various points by considering the concentrations of the remaining acid or base after neutralization, as well as the resulting solution's characteristics, such as whether it is acidic, basic, or neutral.
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02:15pH Calculation Example
Neutralization Reaction
A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this scenario, KOH (a strong base) reacts with HClO4 (a strong acid) to form water and potassium perchlorate. Understanding the stoichiometry of this reaction is crucial for determining the amounts of reactants and products at different stages of the titration.
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05:56Lewis Dot Structures: Neutral Compounds
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A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: (a) 20.0 mL. (b) 23.0 mL.
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A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: (c) 24.0 mL.
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