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: Determine the molality of a solution prepared by dissolving 10.66 g of potassium chlorate in 74.9 g of water. Give your answer to 2 decimal places.a. 0.14 mb .1.16 mc. 0.96 md .1.16x10-3 me. 1.40x103

Problem

Determine the molality of a solution prepared by dissolving 10.66 g of potassium chlorate in 74.9 g of water. Give your answer to 2 decimal places.

a. 0.14 m
b .1.16 m
c. 0.96 m
d .1.16x10-3 m
e. 1.40x103 m

Solution

We’re being asked to calculate for the molality of a solution prepared by dissolving 10.66 g of potassium chlorate in 74.9 g of water.

When calculating for molality, we use the following equation:

molality(m)=moles solutekg solvent

solution → water is the solvent (H2O)
                     solute → potassium chlorate 

                          Potassium → Group 1A → +1 charge → K+
                          Chlorate → polyatomic ion → ClO3-

                          Potassium Chlorate:

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

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