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Indicate the type of solute-solvent interaction that should be most important in each of the following solutions.a. LiCl in waterb. NF3 in acetonitrile (CH3CN)c. CCl4 in benzene (C6H6)d. methylamine (CH3NH2) in watere. Dispersion forcesf. Dipole-dipole forcesg. Ion-dipole forcesh. Hydrogen bonding

Sagot :

Explanation:

a. LiCl is an ionic molecule whereas water is a polar molecule with net dipole moment in it. There LiCl in water would have an ion-dipole force of interaction.

b. Both NF3 and CH3CN have dipole moment in them, since both are polar molecule. Hence, there would be dipole-dipole interaction.

c. Here both CCl4 and benzene are non polar molecules therefore, they have London dispersion force of interaction.

d. In methylamine and water both have hydrogen bonding in them. The nitrogen of CH3NH2 forms hydrogen bond with water.

The type of interactions in the following solutions are:

  • LiCl in water - Ion-dipole force
  • [tex]\rm NF_3[/tex]  in acetonitrile - Dipole-dipole force
  • [tex]\rm CCl_4[/tex] in benzene - London Dispersion force
  • Methylamine in water - Hydrogen bonding

In a solution, the dissolution of solute molecules is driven by the interactions between the solute and solvent molecules.

Which interaction is present in solutions?

The solute solvent interaction is based on the nature of the molecules. The interactions in the following solutions are:

  • LiCl in water

The water is polar solvent and LiCl is an ionic molecule. The interaction between the molecules will be Ion-dipole force.

  • [tex]\rm NF_3[/tex] in acetonitrile

The acetronitrile and [tex]\rm NF_3[/tex] both are polar molecules. The force present in the interactions is Dipole-dipole force.

  • [tex]\rm CCl_4[/tex] in benzene

The benzene and [tex]\rm CCl_4[/tex] both are nonpolar molecules. The type of interaction present in the solution is London Dispersion force.

  • Methylamine in water

The water is a polar solvent, and Methylamine is an organic compound. The interaction in the solution is hydrogen bonding.

Learn more about solute-solvent interactions, here:

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