Ch.12 - SolutionsWorksheetSee all chapters
All Chapters
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

Which of the following represents the mass percent of H2SO4 (MM = 98) in a 2.00 m aqueous H2SOsolution?


We’re being asked to determine the volume (in mL) of solution that would contain 0.10 mol sucrose in a 0.40 molal solution.

Recall that molality is the ratio of the moles of solute and the mass of solvent (in kilograms)

In other words:

Molality(m)=moles solutekg solvent

Recall the mass percent formula shown below:

mass percent=mass componenttotal mass×100

Since we are dealing with a solution, we can rewrite the equation as:

% mass=mass solutemass solution×100

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