Calculate the molality of a 0.533 M aqueous solution of iron(II) chloride with a density, p = 1.059 g/mL. Report answer in three significant figures.
Calculate the molality of a 0.533 M aqueous solution of iron(II) chloride with a density, p = 1.059 g/mL. Report answer in three significant figures.
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter14: Mixtures And Solutions
Section: Chapter Questions
Problem 106A: Which solute has the greatest effect on the boiling pointof 1.00 kg of water: 50.0 g of strontium...
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Calculate the molality of a 0.533 M aqueous solution of iron(II) chloride with a density, p = 1.059 g/mL. Report answer in three significant figures.
Expert Solution
Step 1
We have been given, a 0.533 M aqueous solution, means, the molarity is 0.533.
Molarity is the number of moles present per liter of the solution.
Also, density = 1.059 g/mL.
We have to find out molality of the solution which is number of moles of solute present per kg of the solution.
Given solute is iron(II) Chloride
Molar mass of solute = 127 g/mol
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