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Science Chemistry Chemistry: An Atoms-Focused Approach

How measurements of osmotic pressure, freezing point depression, and boiling point elevation be used to find the molar mass of a solute. The reasons why it is important to know whether the solute is an electrolyte or a nonelectrolyte. Solution: We can compare the value of concentration in moles per volume (L) with known concentration of solute in mass per volume, to determine the molar mass of a solute. To determine the value i (van’t Hoff factor), it is important to know whether the solute is electrolyte or non-electrolyte. Explanation: Osmotic pressure: From the osmotic pressure, we can determine the concentration of solution at a particular temperature by the following equation π = i M R T Where π = osmotic pressure i = van’t Hoff factor M = Molar concentration R = Gas constant T = Temperature Using osmotic pressure, temperature and van’t Hoff factor, we can calculate molarity. The formula for molarity is M = m o l e s o f s o l u t e v o l u m e o f s o l u t i o n i n L With calculated molality and volume of solution in L, we can calculate moles of solute. Using mass and calculated moles of solute, the molar mass of solute can be calculated. Freezing point depression: We can determine the molar concentration (mol/kg of solvent) of the solute in a solution from the freezing point depression using the following equation ∆ T f = i K f m Where, ∆ T f = freezing point depression K f = molal freezing point depression constant i = van’t Hoff factor Using ∆ T f , K f and i the molality of solution can be calculated. The formula for molality is, m = m o l e s o f s o l u t e m a s s o f s o l v e n t i n k g With calculated molality and mass of solvent in kg, the moles of solute can be calculated. Using mass and calculated moles of solute, the molar mass of solute can be calculated. Boiling point elevation: Similar is the case in boiling point elevation as in freezing point depression. Here also, we can determine the molal concentration (mol/kg) of solute in the solution from the boiling point elevation using the following equation, ∆ T b = i K b m Where, ∆ T b = boiling point elevation K b = molal boiling point elevation constant i = van’t Hoff factor With calculated molality and mass of solvent in kg, the moles of solute can be calculated. Using mass and calculated moles of solute, the molar mass of solute can be calculated. To determine the value of i (van’t Hoff factor), it is important to know whether, the solute is electrolyte or non-electrolyte. The value of i for non-electrolytes is 1, whereas for electrolytes it depends on the number of ions produced after dissociation. Conclusion: We first need to determine the concentration of solute using the measurements of osmotic pressure, freezing point depression, and boiling point elevation and then the molar mass can be found.

How measurements of osmotic pressure, freezing point depression, and boiling point elevation be used to find the molar mass of a solute. The reasons why it is important to know whether the solute is an electrolyte or a nonelectrolyte. Solution: We can compare the value of concentration in moles per volume (L) with known concentration of solute in mass per volume, to determine the molar mass of a solute. To determine the value i (van’t Hoff factor), it is important to know whether the solute is electrolyte or non-electrolyte. Explanation: Osmotic pressure: From the osmotic pressure, we can determine the concentration of solution at a particular temperature by the following equation π = i M R T Where π = osmotic pressure i = van’t Hoff factor M = Molar concentration R = Gas constant T = Temperature Using osmotic pressure, temperature and van’t Hoff factor, we can calculate molarity. The formula for molarity is M = m o l e s o f s o l u t e v o l u m e o f s o l u t i o n i n L With calculated molality and volume of solution in L, we can calculate moles of solute. Using mass and calculated moles of solute, the molar mass of solute can be calculated. Freezing point depression: We can determine the molar concentration (mol/kg of solvent) of the solute in a solution from the freezing point depression using the following equation ∆ T f = i K f m Where, ∆ T f = freezing point depression K f = molal freezing point depression constant i = van’t Hoff factor Using ∆ T f , K f and i the molality of solution can be calculated. The formula for molality is, m = m o l e s o f s o l u t e m a s s o f s o l v e n t i n k g With calculated molality and mass of solvent in kg, the moles of solute can be calculated. Using mass and calculated moles of solute, the molar mass of solute can be calculated. Boiling point elevation: Similar is the case in boiling point elevation as in freezing point depression. Here also, we can determine the molal concentration (mol/kg) of solute in the solution from the boiling point elevation using the following equation, ∆ T b = i K b m Where, ∆ T b = boiling point elevation K b = molal boiling point elevation constant i = van’t Hoff factor With calculated molality and mass of solvent in kg, the moles of solute can be calculated. Using mass and calculated moles of solute, the molar mass of solute can be calculated. To determine the value of i (van’t Hoff factor), it is important to know whether, the solute is electrolyte or non-electrolyte. The value of i for non-electrolytes is 1, whereas for electrolytes it depends on the number of ions produced after dissociation. Conclusion: We first need to determine the concentration of solute using the measurements of osmotic pressure, freezing point depression, and boiling point elevation and then the molar mass can be found.

Solution Summary: The author explains how osmotic pressure, freezing point depression, and boiling point elevation can be used to determine the molar mass of a solute.

Chemistry: An Atoms-Focused Approach

Chemistry: An Atoms-Focused Approach

14th Edition

ISBN: 9780393912340

Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster

Publisher: W. W. Norton & Company

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Chemistry: An Atoms-Focused Approach

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