Chapter 23, Problem 59A

Interpretation Introduction

Interpretation: To compare the solubility 1-butanol and diethyl ether and explain why 1-Butanol has a higher boiling point than diethyl ether.

Concept Introduction: Several factors affect the boiling point. The boiling point is affected by the pressure, impurities present, intermolecular forces, molecular weight of the compound, and branching.

Answer to Problem 59A

1-butanol has hydrogen bonding whereas diethyl ether has weak London dispersion forces as well as dipole-dipole interactions. Therefore, 1-butanol has a higher boiling point and 1-butanol will be highly soluble in water as compared to diethyl ether.

Explanation of Solution

In 1-butanol there is hydrogen bonding present between the electronegative atom oxygen and the hydrogen. Whereas, diethyl ether is less polar so there is no chance of hydrogen bonding. Since it is very less polar it will have weak dipole-dipole interactions. Therefore, 1-butanol will have a higher boiling point than the di ethyl ether. As 1-butanol has a higher boiling point it will be more soluble as compared to that diethyl ether.

Conclusion

Intermolecular forces present in the molecule will affect the boiling point of the molecule. If intermolecular forces are weak then the boiling point will be low because less energy is required to break the bonds. If intermolecular forces are strong then the boiling point will be high because high energy is required to break the bond. The greater the boiling point, the greater will be the solubility. Hence, 1-butanol is more soluble.