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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.)
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Ch.13 - Solutions
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- 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
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Capitolo 13, Problema 64e
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
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Calculate the mass of methanol using its volume and density: \( \text{mass of methanol} = \text{volume} \times \text{density} = 20.2 \, \text{mL} \times 0.782 \, \text{g/mL} \).
Convert the mass of methanol to moles using its molar mass: \( \text{moles of methanol} = \frac{\text{mass of methanol}}{\text{molar mass of CH}_3\text{OH}} \). The molar mass of methanol (CH3OH) is approximately 32.04 g/mol.
Calculate the mass of water using its volume and density: \( \text{mass of water} = \text{volume} \times \text{density} = 100.0 \, \text{mL} \times 1.00 \, \text{g/mL} \).
Convert the mass of water to moles using its molar mass: \( \text{moles of water} = \frac{\text{mass of water}}{\text{molar mass of H}_2\text{O}} \). The molar mass of water (H2O) is approximately 18.02 g/mol.
Calculate the mole percent of methanol in the solution: \( \text{mole percent} = \left( \frac{\text{moles of methanol}}{\text{moles of methanol} + \text{moles of water}} \right) \times 100\% \).
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Molarity and Concentration Units
Molarity is a common way to express concentration, defined as the number of moles of solute per liter of solution. In addition to molarity, concentrations can also be expressed in terms of mole percent, which indicates the ratio of moles of a specific component to the total moles of all components in the solution, multiplied by 100. Understanding these units is essential for accurately calculating and comparing concentrations.
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01:13
Molarity
Density and Mass Calculation
Density is the mass of a substance per unit volume, typically expressed in grams per milliliter (g/mL). To find the mass of a liquid from its volume and density, the formula mass = density × volume is used. This concept is crucial for converting the volume of methanol and water into mass, which is necessary for calculating the number of moles and ultimately the concentration.
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03:12Molar Mass Calculation Example
Mole Concept
The mole is a fundamental unit in chemistry that quantifies the amount of substance. One mole contains approximately 6.022 x 10²³ entities (Avogadro's number), allowing chemists to relate mass to the number of particles. In this context, calculating the number of moles of methanol and water is essential for determining their contributions to the mole percent of the solution.
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01:25Mole Concept
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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
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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. d. mole fraction
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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.)
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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
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