Answered: Calculate the molality of a 0.533 M…

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.

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter8: Solutions

Section: Chapter Questions

Problem 8.9EP: A solution is made by dissolving 34.0 g of NaCl in 100 g of H2O at 0C. Based on the data in Table...

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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

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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