   Chapter 12, Problem 12.81QP General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343

Solutions

Chapter
Section General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343
Textbook Problem

A 0.0140-g sample of an ionic compound with the formula Cr(NH3)5Cl3 was dissolved in water to give 25.0 mL of solution at 25°C. The osmotic pressure was determined to be 119 mmHg. How many ions arc obtained from each formula unit when the compound is dissolved in water?

Interpretation Introduction

Interpretation:

Osmotic pressure of a solution of a compound is given and number of ions in the solute compound has to be determined.

Concept Introduction:

In the process of osmosis, the solvent molecules pass through a semi - permeable membrane from less concentrated solution to more concentrated solution.  The pressure that has to be applied to prevent the flow of solvent molecules is called osmotic pressure.  It is expressed as,

π = MRT

Where,

π = osmotic pressureM = Molar concentrationR = Universal gas constantT = Temperature

Molarity or molal concentration is one of the many parameters that is used to express concentration of a solution.  It is expressed as,

Molarity = number of moles of solutevolume of solution in L

Explanation

Given that osmotic pressure of solution is 119 mmHg at 25°C . Mass of the solute Cr(NH3)5Cl3 is 0.0140 g and volume of solution is 25.0 mL .

Calculate the number of moles of solute Cr(NH3)5Cl3 and molarity of the solution as follows –

no.of moles massmolar mass = 0.0140 g243.5 g/mol = 5.749×105 molMolarity no.of moles of solutevolume of solution in L = 5

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