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: 12.00 grams of acetic acid HC2H3O2 (Molar mass= 60.00 g/mol) are dissolved in 188.0 grams of water. Density of solution is 1.12g/mL.a. What is the wt/wt % concentration of the solution? b. What is the molarity of this solution?  c. What is the molality of the solution?

Solution: 12.00 grams of acetic acid HC2H3O2 (Molar mass= 60.00 g/mol) are dissolved in 188.0 grams of water. Density of solution is 1.12g/mL.a. What is the wt/wt % concentration of the solution? b. What is the

Problem

12.00 grams of acetic acid HC2H3O2 (Molar mass= 60.00 g/mol) are dissolved in 188.0 grams of water. Density of solution is 1.12g/mL.

a. What is the wt/wt % concentration of the solution?

 

b. What is the molarity of this solution?

 

 

c. What is the molality of the solution?

Solution

Here we are given the mass of both the solute (acetic acid) and solvent (water) so we can easily get the wt/wt % or also called mass %. Remember that this is the mass of solute over the mass of solution times a hundred so we still have to find the mass of the solution. We can easily get the mass of the solution by adding the masses of the solute and solvent.

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