Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 13, Problem 57GQ

Dimethylglyoxime [DMG, (CH3CNOH)2] is used as a reagent to precipitate nickel ion. Assume that 53.0 g of DMC has been dissolved in 525 g of ethanol (C2H5OH).

sChapter 13, Problem 57GQ, Dimethylglyoxime [DMG, (CH3CNOH)2] is used as a reagent to precipitate nickel ion. Assume that 53.0

The red, insoluble compound formed between nickel(II)ion and dimethylglyoxime (DMG) is precipitated when DMG is added to a bask solution of Ni2+ (aq).

  1. (a) What is the mole fraction of DMG?
  2. (b) What is the molality of the solution?
  3. (c) What is the vapor pressure of the ethanol over the solution at ethanol’s normal boiling point of 78.4 °C?
  4. (d) What is the boiling point of the solution? (DMG does not produce ions in solution.) (Kbp for ethanol = +1.22 °C/m)

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: Mole fraction of DMG has to be calculated.

Concept introduction:

Raoult’s law: In a solution, vapor pressure of solvent is proportional to its mole fraction.

  Psolvent=XsolventP0solvent

  where,

  P0solvent is the vapor pressure of pure solvent.

Mole fraction: Amount of that component divided by the total amount of all of the components of the mixture ( nA +  nB +  n...).

  Mole fraction of A (χA)= nA nA +  nB +  n...

Answer to Problem 57GQ

Mole fraction of DMG is 0.0385

Explanation of Solution

Given,

Massofethanol=53.0gMassofDMG=525gMolarmassofethanol=46.07g/molMolarmassofDMG=116.12g/mol

The number of moles of any substance can be determined using the equation

  Numberofmole=GivenmassofthesubstanceMolarmass

Number of moles of dimethylglyoxime is,

  nDMG=53.0g116.12g/mol=0.4564mol

Number of moles of ethanol is,

  nethanol=525g46.07g/mol=11.4mol

Mole fraction of DMG is calculated

Molefraction,XDMG=nDMGnDMG+nethanol=0.4564mol(0.4564mol)+(11.4mol)=0.0385

Mole fraction of DMG is 0.0385

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: Molality of the solution has to be determined.

Concept introduction:

Raoult’s law: In a solution, vapor pressure of solvent is proportional to its mole fraction.

  Psolvent=XsolventP0solvent

  where,

  P0solvent is the vapor pressure of pure solvent.

Mole fraction: Amount of that component divided by the total amount of all of the components of the mixture ( nA +  nB +  n...).

  Mole fraction of A (χA)= nA nA +  nB +  n...

Answer to Problem 57GQ

Molality of the solution is 0.869m

Explanation of Solution

Given,

Massofethanol=53.0gMassofDMG=525gMolarmassofethanol=46.07g/molMolarmassofDMG=116.12g/mol

The number of moles of any substance can be determined using the equation

  Numberofmole=GivenmassofthesubstanceMolarmass

Number of moles of dimethylglyoxime is,

  nDMG=53.0g116.12g/mol=0.4564mol

Molality of the solution is calculated

  Molality (m) =0.4564mol0.525kg=0.869m

Molality of the solution is 0.869m

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: Mole fraction of DMG and molality of the solution are to be determined. Vapour pressure of ethanol over the solution and Boiling point of the solution are to be calculated.

Concept introduction:

Raoult’s law: In a solution, vapor pressure of solvent is proportional to its mole fraction.

  Psolvent=XsolventP0solvent

  where,

  P0solvent is the vapor pressure of pure solvent.

Mole fraction: Amount of that component divided by the total amount of all of the components of the mixture ( nA +  nB +  n...).

  Mole fraction of A (χA)= nA nA +  nB +  n...

Answer to Problem 57GQ

Vapor pressure of ethanol over the solution is 730.7mmHg

Explanation of Solution

(c)

Given,

Massofethanol=53.0gMassofDMG=525gMolarmassofethanol=46.07g/molMolarmassofDMG=116.12g/molVapourpressureofpureethanolat78.40C=760mmHg

The number of moles of any substance can be determined using the equation

  Numberofmole=GivenmassofthesubstanceMolarmass

Number of moles of dimethylglyoxime is,

  nDMG=53.0g116.12g/mol=0.4564mol

Number of moles of ethanol is,

  nethanol=525g46.07g/mol=11.4mol

Molefraction,Xethanol=nethanolnDMG+nethanol=11.4mol(0.4564mol)+(11.4mol)=0.9615

Mole fraction of ethanol is 0.9615

Vapour pressure of ethanol over the solution is calculated

Pethanol=XethanolP0ethanol=(0.9615)×(760mmHg)=730.7mmHg

Vapour pressure of ethanol over the solution is 730.7mmHg

(d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: Mole fraction of DMG and molality of the solution are to be determined. Vapour pressure of ethanol over the solution and Boiling point of the solution are to be calculated.

Concept introduction:

Raoult’s law: In a solution, vapor pressure of solvent is proportional to its mole fraction.

  Psolvent=XsolventP0solvent

  where,

  P0solvent is the vapor pressure of pure solvent.

Mole fraction: Amount of that component divided by the total amount of all of the components of the mixture ( nA +  nB +  n...).

  Mole fraction of A (χA)= nA nA +  nB +  n...

Answer to Problem 57GQ

Boiling point of the solution is 79.50C

Explanation of Solution

(d)

Given,

  Massofethanol=53.0gMassofDMG=525gMolarmassofethanol=46.07g/molMolarmassofDMG=116.12g/mol

Number of moles of dimethylglyoxime is,

  nDMG=53.0g116.12g/mol=0.4564mol

Molality of the solution is calculated

  Molality (m) =0.4564mol0.525kg=0.869m

Molality of the solution is 0.869m

Elevation in boiling point of the solution is calculated

  ΔTbp=Kbpmsolute=(1.220C/m)×(0.869m)=1.060C

Therefore,

Boiling point of the solution is (78.40C+1.060C)=79.50C

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