2. A 28.0 % by mass solution of Iodine( not Iodide ) andCCl 4 has a density of 1
ID: 691070 • Letter: 2
Question
2.
A 28.0 % by mass solution of Iodine(not Iodide) andCCl4 has a density of 1.56 g/mL.
Convert this mass percent into the following concentrationexpressions:
Since it doesn't state how much solutionyou have, assume you have 100 g ofsolution. Then a 28.0 % solution would contain 28.0 g Iodine.
A Map of Concentration Units and the relationships betweenthese units and Molarity, molality, mass %, ppm, and mole fractioncan be found under the ReferenceMaterial link and then the Expressing Concentrations link (or click here).
Reconstruct this Map of Concentration Units on a sheet of paper andplace the numbers in red in theirappropriate places. Fill in the rest of the Map and then use theinformation in the Map to express the solution's concentration inthe terms below.
Molarity
molality
Parts per million Iodine
Mole fraction Iodine
Mole fraction CCl4
Explanation / Answer
A 28.0 % by mass solution of Iodine(not Iodide) and CCl4 has a density of1.56 g/mL. .100 g of solution would contain 28.0 gIodine. Moles of Iodine = mass / molar mass = 28.0 g /253.81 g/mol = 0.11moles. . Volume of solution = mass / density = 100 g / 1.56 g/mL = 64.1 mL or 0.064 L . Molarity = moles / volume =0.11 moles / 0.064 L =1.72 M . Mass of solvent = mass of solution - mass of solute = 100 g - 28g = 72 g or 0.072kg Molality = moles / mass of solvent (kg) = 0.11 /0.072 kg = 1.53m . ppm of iodine = (mass of iodine / mass of solution ) * 10^6 = ( 28 g / 100 g ) * 10^6 = 2.8 * 10^5 ppm . Moles of solvent, (CCl4) = 72 g / 153.82 g/mol = 0.468 moles Moles of iodine = 0.111 . Mole fraction of Iodine = moles of Iodine / total moles = 0.111 / (0.111 + 0.468 moles) = 0.192 . Mole fraction of CCl4 = 0.468 moles / (0.111 + 0.468 ) moles = 0.808
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