Domanda del libro di testo
Household hydrogen peroxide is an aqueous solution containing 3.0% hydrogen peroxide by mass. What is the molarity of this solution? (Assume a density of 1.01 g/mL.)
1802
views
1
rank
Ch.14 - Solutions
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Capitolo 14, Problema 64d
A solution is prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water at 25 °C. The final volume of the solution is 118 mL. The densities of methanol and water at this temperature are 0.782 g/mL and 1.00 g/mL, respectively. For this solution, calculate the concentration in each unit. d. mole fraction
Guida verificata passo dopo passo1
Calculate the mass of methanol using its volume and density: \( \text{mass of methanol} = \text{volume} \times \text{density} = 20.2 \text{ mL} \times 0.782 \text{ g/mL} \).
Calculate the moles of methanol using its molar mass (32.04 g/mol): \( \text{moles of methanol} = \frac{\text{mass of methanol}}{32.04 \text{ g/mol}} \).
Calculate the mass of water using its volume and density: \( \text{mass of water} = \text{volume} \times \text{density} = 100.0 \text{ mL} \times 1.00 \text{ g/mL} \).
Calculate the moles of water using its molar mass (18.02 g/mol): \( \text{moles of water} = \frac{\text{mass of water}}{18.02 \text{ g/mol}} \).
Calculate the mole fraction of methanol: \( \text{mole fraction of methanol} = \frac{\text{moles of methanol}}{\text{moles of methanol} + \text{moles of water}} \).
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:
3mConcetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Mole Fraction
Mole fraction is a way of expressing the concentration of a component in a mixture. It is defined as the ratio of the number of moles of a specific component to the total number of moles of all components in the solution. For a solution containing methanol and water, the mole fraction of methanol can be calculated by dividing the moles of methanol by the sum of the moles of methanol and water.
Video consigliato:
Percorso guidato
00:36
Mole Fraction Formula
Density and Volume Relationships
Density is defined as mass per unit volume and is crucial for converting between mass and volume when calculating concentrations. In this problem, the densities of methanol and water allow us to determine their masses from their respective volumes. Understanding how to manipulate these relationships is essential for calculating the total moles of each component in the solution.
Video consigliato:
Percorso guidato
01:09Relationship of Volume and Moles Example
Concentration Units
Concentration can be expressed in various units, including molarity, mass percent, and mole fraction. Each unit provides different insights into the composition of a solution. In this case, calculating the mole fraction requires knowing the moles of each component, which can be derived from their masses and molar masses, emphasizing the importance of unit conversions in solution chemistry.
Video consigliato:
Percorso guidato
02:13SI Units
Pratica correlata
Domanda del libro di testo
A solution is prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water at 25 °C. The final volume of the solution is 118 mL. The densities of methanol and water at this temperature are 0.782 g/mL and 1.00 g/mL, respectively. For this solution, calculate the concentration in each unit. e. mole percent
334
views
Domanda del libro di testo
A solution is prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water at 25 °C. The final volume of the solution is 118 mL. The densities of methanol and water at this temperature are 0.782 g/mL and 1.00 g/mL, respectively. For this solution, calculate the concentration in each unit. b. molality
1192
views
Domanda del libro di testo
A solution is prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water at 25 °C. The final volume of the solution is 118 mL. The densities of methanol and water at this temperature are 0.782 g/mL and 1.00 g/mL, respectively. For this solution, calculate the concentration in each unit. a. molarity
1041
views
Domanda del libro di testo
One brand of laundry bleach is an aqueous solution containing 4.55% sodium hypochlorite (NaOCl) by mass. What is the molarity of this solution? (Assume a density of 1.02 g/mL.)
1822
views
2
rank
Domanda del libro di testo
A solution is prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water at 25 °C. The final volume of the solution is 118 mL. The densities of methanol and water at this temperature are 0.782 g/mL and 1.00 g/mL, respectively. For this solution, calculate the concentration in each unit. c. percent by mass
454
views