Dipole Moment of Water: Explaining Its Ability to Solve Substances

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SUMMARY

The dipole moment of water, measured at 6.1 x 10-30C.m, is a critical factor in its effectiveness as a solvent. The bent molecular structure of water, with an angle of 105 degrees, contributes to its polarity, allowing it to interact favorably with various solutes. This unique property enables water to dissolve a wide range of substances, making it an essential solvent in both biological and chemical processes.

PREREQUISITES
  • Understanding of molecular polarity
  • Basic knowledge of molecular geometry
  • Familiarity with dipole moments
  • Concept of solvation and solvent properties
NEXT STEPS
  • Research the role of molecular geometry in solvent properties
  • Study the effects of dipole moments on solubility
  • Explore the concept of hydrogen bonding in water
  • Learn about the solvation process in different solvents
USEFUL FOR

Chemistry students, educators, and researchers interested in molecular interactions and solvent properties will benefit from this discussion.

Reshma
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Certain molecules have built-in dipole moments. The dipole moment of water is unusually large: 6.1 x 10-30C.m. How does this account for the effectiveness of water as a solvent?
 
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Looks like a standard textbook question.

This thread shoud go into the Coursework section where it will be subject to the requirement that you first tell us what you think.
 
OK, I did not realize this is a HW-type question :blushing:.

So, in a water molecule, electrons cluster around the oxygen atom and the molecule is bent at an angle of 105 degrees. How does this make water an excellent solvent?
 
Last edited:
The molecule is polar, that should be the "bridge" between clustered electrons and excelent solvents.

I can't blame you though. The question is worded all weird but the concept is nevertheless the same, so you are better off researching about this.
 

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