Ch.12 - SolutionsWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Calculate the molality of a 6.35 M aqueous methanol (CH3OH) solution with a density of 0.953 g/mL. A. 7.28 m B. 6.99 m C. 5.87 m D. 8.47 m

Problem

Calculate the molality of a 6.35 M aqueous methanol (CH3OH) solution with a density of 0.953 g/mL.

A. 7.28 m
B. 6.99 m
C. 5.87 m
D. 8.47 m

Solution

We’re being asked to calculate for the molality of a 6.35 M methanol (CH3OH) solution. 

When calculating for molality, we use the following equation:

molality m = mol solutekg solvent


We will calculate the molality of the solution using the following steps:

Step 1: Calculate the mass of the solute.

Step 2: Calculate the mass of the solution.

Step 3: Calculate the mass of the solvent (in kg).

Step 4: Calculate the molality of the solution.

Solute → CH3OH

Solvent → water (H2O)

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