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

Solution: In a sample consisting of 1.00 mol NaBr and 0.300 mol KI, what is the mass percent of iodine?

Problem

In a sample consisting of 1.00 mol NaBr and 0.300 mol KI, what is the mass percent of iodine?

Solution

We are asked to calculate for the percent by mass (mass %) of Iodinein this mixture and to do that we’re going to use the mass percent formula shown below:


https://lightcat-files.s3.amazonaws.com/problem_images/2af505efffdb9887-1563418668086.jpg.


First, get the moles of I. We do that by doing a mole to mole comparison using KI. We see that for every mole of KI we have 1 mole of I. 


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