Domanda del libro di testo
The osmotic pressure of a 0.010 M aqueous solution of CaCl2 is found to be 0.674 atm at 25 °C. Calculate the van't Hoff factor, i, for the solution.
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Ch.13 - Properties of Solutions
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
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 13, Problema 80
Lauryl alcohol is obtained from coconut oil and is used to make detergents. A solution of 5.00 g of lauryl alcohol in 0.100 kg of benzene freezes at 4.1 °C. What is the molar mass of lauryl alcohol from this data?
Guida verificata passo dopo passo1
Identify the freezing point depression formula: \( \Delta T_f = K_f \cdot m \), where \( \Delta T_f \) is the freezing point depression, \( K_f \) is the cryoscopic constant of the solvent, and \( m \) is the molality of the solution.
Calculate the freezing point depression \( \Delta T_f \) by subtracting the observed freezing point of the solution (4.1 °C) from the normal freezing point of benzene (5.5 °C).
Determine the molality \( m \) of the solution using the formula \( m = \frac{\text{moles of solute}}{\text{kg of solvent}} \).
Rearrange the freezing point depression formula to solve for the moles of solute: \( \text{moles of solute} = \frac{\Delta T_f}{K_f} \cdot \text{kg of solvent} \). Use the known \( K_f \) value for benzene.
Calculate the molar mass of lauryl alcohol by dividing the mass of lauryl alcohol (5.00 g) by the moles of solute obtained in the previous step.
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Freezing Point Depression
Freezing point depression is a colligative property that describes how the freezing point of a solvent decreases when a solute is added. The extent of this depression depends on the number of solute particles in the solution, not their identity. The formula used to calculate the change in freezing point is ΔTf = Kf * m, where Kf is the freezing point depression constant of the solvent and m is the molality of the solution.
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Percorso guidato
01:59
Freezing Point Depression
Molality
Molality (m) is a measure of concentration defined as the number of moles of solute per kilogram of solvent. It is particularly useful in colligative property calculations because it directly relates to the number of solute particles in a given mass of solvent. In this case, knowing the mass of lauryl alcohol and the mass of benzene allows for the calculation of molality, which is essential for determining the molar mass of lauryl alcohol.
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00:40Molality
Molar Mass Calculation
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To find the molar mass of lauryl alcohol in this scenario, one can rearrange the freezing point depression equation to solve for the molar mass using the known mass of the solute, the change in freezing point, and the mass of the solvent. This calculation is crucial for identifying the molecular weight of lauryl alcohol based on the experimental data provided.
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03:12Molar Mass Calculation Example
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Lysozyme is an enzyme that breaks bacterial cell walls. A solution containing 0.150 g of this enzyme in 210 mL of solution has an osmotic pressure of 0.953 torr at 25 °C. What is the molar mass of lysozyme?
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Domanda del libro di testo
Adrenaline is the hormone that triggers the release of extra glucose molecules in times of stress or emergency. A solution of 0.64 g of adrenaline in 36.0 g of CCl4 elevates the boiling point by 0.49 °C. Calculate the approximate molar mass of adrenaline from this data.
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Domanda del libro di testo
A dilute aqueous solution of an organic compound soluble in water is formed by dissolving 2.35 g of the compound in water to form 0.250 L of solution. The resulting solution has an osmotic pressure of 0.605 atm at 25 °C. Assuming that the organic compound is a nonelectrolyte, what is its molar mass?
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Domanda del libro di testo
Seawater contains 34 g of salts for every liter of solution. Assuming that the solute consists entirely of NaCl (in fact, over 90% of the salt is indeed NaCl), calculate the osmotic pressure of seawater at 20 °C
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