Textbook Question
Describe how you would prepare each of the following aqueous solutions from water and solid KBr: b. 125 g of 0.180 m KBr.
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Ch.13 - Properties of Solutions
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 13, Problem 51c
Calculate the number of moles of solute present in each of the following aqueous solutions: (c) 124.0 g of a solution that is 6.45% glucose (C6H12O6) by mass.
Verified step by step guidance1
Identify the mass percentage of glucose in the solution, which is given as 6.45%.
Calculate the mass of glucose in the solution by multiplying the total mass of the solution (124.0 g) by the mass percentage (6.45%) expressed as a decimal.
Determine the molar mass of glucose (C_6H_12O_6) by adding the atomic masses of all the atoms in the molecular formula: 6 carbon atoms, 12 hydrogen atoms, and 6 oxygen atoms.
Use the mass of glucose obtained in step 2 and the molar mass from step 3 to calculate the number of moles of glucose using the formula: \( \text{moles} = \frac{\text{mass of glucose}}{\text{molar mass of glucose}} \).
The result from step 4 will give you the number of moles of glucose present in the solution.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Percent by Mass
Percent by mass is a way to express the concentration of a solution, indicating the mass of solute present in a given mass of solution. In this case, a 6.45% glucose solution means that there are 6.45 grams of glucose for every 100 grams of solution. This concept is essential for determining the mass of solute in a specific mass of solution.
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For glucose (C6H12O6), the molar mass is approximately 180.18 g/mol. Knowing the molar mass allows us to convert between grams of solute and moles, which is crucial for calculating the number of moles in a solution.
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Molar Mass Concept
Moles of Solute
The number of moles of solute can be calculated using the formula: moles = mass (g) / molar mass (g/mol). This relationship is fundamental in stoichiometry and solution chemistry, as it allows us to quantify the amount of solute present in a solution, which is necessary for various calculations in chemistry.
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Related Practice
Textbook Question
Calculate the number of moles of solute present in each of the following aqueous solutions: (b) 86.4 g of 0.180 m KCl,
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Textbook Question
The density of acetonitrile (CH3CN) is 0.786 g/mL and the density of methanol (CH3OH) is 0.791 g/mL. A solution is made by dissolving 22.5 mL of CH3OH in 98.7 mL of CH3CN. (c) Assuming that the volumes are additive, what is the molarity of CH3OH in the solution?
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Textbook Question
Calculate the number of moles of solute present in each of the following solutions: (a) 255 mL of 1.50 M HNO3(aq),
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Textbook Question
The density of toluene (C7H8) is 0.867 g/mL, and the density of thiophene (C4H4S) is 1.065 g/mL. A solution is made by dissolving 8.10 g of thiophene in 250.0 mL of toluene. (a) Calculate the mole fraction of thiophene in the solution.
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