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
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
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
Tutti i libri di testo
Brown 15th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 43c
Brown 15th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 43cCapitolo 17, Problema 43c
A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added:
(c) 20.0 mL.
Guida verificata passo dopo passo1
Step 1: Identify the type of reaction occurring. This is a neutralization reaction between a strong acid (HBr) and a strong base (NaOH). The reaction can be represented as: \[ \text{HBr} + \text{NaOH} \rightarrow \text{NaBr} + \text{H}_2\text{O} \]
Step 2: Calculate the moles of HBr initially present in the solution. Use the formula: \[ \text{moles of HBr} = \text{volume (L)} \times \text{molarity (M)} \]. For 20.0 mL of 0.200 M HBr, convert the volume to liters and calculate the moles.
Step 3: Calculate the moles of NaOH added. Similarly, use the formula: \[ \text{moles of NaOH} = \text{volume (L)} \times \text{molarity (M)} \]. For 20.0 mL of 0.200 M NaOH, convert the volume to liters and calculate the moles.
Step 4: Determine the limiting reactant. Since both HBr and NaOH have the same concentration and volume, they will react in a 1:1 ratio, and both will be completely consumed in the reaction.
Step 5: Calculate the pH of the resulting solution. After complete neutralization, the solution contains only water and the salt NaBr, which does not affect the pH. Therefore, the pH of the solution is neutral, which is 7.
Risposta video verificata per un problema simile:
Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
5mConcetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
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, NaOH) to a solution containing the analyte (HBr) until the reaction reaches its equivalence point, where the amount of titrant added is stoichiometrically equivalent to the amount of analyte present.
Video consigliato:
Percorso guidato
03:04
Acid-Base Titration
pH and Neutralization
pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. In a neutralization reaction between a strong acid (HBr) and a strong base (NaOH), the pH at the equivalence point is typically 7, indicating a neutral solution. Understanding how to calculate pH before and after the equivalence point is crucial for solving titration problems.
Video consigliato:
Percorso guidato
02:33The pH Scale
Stoichiometry of Acid-Base Reactions
Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. For the reaction between HBr and NaOH, the balanced equation shows a 1:1 molar ratio. This means that equal moles of HBr and NaOH will neutralize each other, allowing for the calculation of remaining concentrations and pH after specific volumes of base are added.
Video consigliato:
Percorso guidato
01:09Acid-Base Reaction
Pratica correlata
Domanda del libro di testo
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.
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: (b) 22.5 mL of 0.118 M NH3?
1024
views
Domanda del libro di testo
A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added:
(a) 15.0 mL
(b) 19.9 mL.
115
views
Domanda del libro di testo
A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added: (e) 35.0 mL.
1918
views
Domanda del libro di testo
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.
2003
views