Domanda del libro di testo
How many milliliters of 0.105 M HCl are needed to titrate each of the following solutions to the equivalence point: (a) 45.0 mL of 0.0950 M NaOH? (c) 125.0 mL of a solution that contains 1.35 g of NaOH per liter?
Ch.17 - Additional Aspects of Aqueous Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
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Brown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 41b
Brown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 41bCapitolo 17, Problema 41b
How many milliliters of 0.0850 M NaOH are required to titrate each of the following solutions to the equivalence point: (b) 35.0 mL of 0.0850 M CH3COOH?
Guida verificata passo dopo passo1
Identify the balanced chemical equation for the reaction: \( \text{CH}_3\text{COOH} + \text{NaOH} \rightarrow \text{CH}_3\text{COONa} + \text{H}_2\text{O} \). This shows a 1:1 molar ratio between acetic acid (CH3COOH) and sodium hydroxide (NaOH).
Calculate the moles of CH3COOH present in the solution using the formula: \( \text{moles} = \text{Molarity} \times \text{Volume (L)} \). Convert 35.0 mL to liters by dividing by 1000.
Since the reaction is a 1:1 molar ratio, the moles of NaOH required will be equal to the moles of CH3COOH calculated in the previous step.
Use the moles of NaOH and its molarity to find the volume required using the formula: \( \text{Volume (L)} = \frac{\text{moles}}{\text{Molarity}} \).
Convert the volume from liters to milliliters by multiplying by 1000 to find the final volume of NaOH solution needed for the titration.
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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 (a solution of known concentration) to a sample solution until the reaction reaches its equivalence point, where the amount of titrant equals the amount of substance in the sample. This process is often indicated by a color change or a pH change.
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Percorso guidato
03:04
Acid-Base Titration
Molarity
Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (mol/L) and is crucial for calculations in titration, as it allows for the determination of how much of a titrant is needed to react with a given volume of analyte. Understanding molarity is essential for accurately calculating the volumes required in titration experiments.
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Percorso guidato
01:13Molarity
Neutralization Reaction
A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this context, acetic acid (CH₃COOH) reacts with sodium hydroxide (NaOH) in a 1:1 molar ratio. Recognizing the stoichiometry of the reaction is vital for determining the volume of NaOH needed to reach the equivalence point when titrating the acetic acid solution.
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05:56Lewis Dot Structures: Neutral Compounds
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