Water is a good solvent for dissolving ionic compounds because
It has a high specific heat
It has no colour
It has a high dipole moment
It has a high boiling point
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UPSC CAPF – 2024
Water is an excellent solvent for ionic compounds because it is a polar molecule with a high dipole moment. An ionic compound is held together by strong electrostatic forces between positive and negative ions in a crystal lattice. Water molecules, being polar, have a partial positive charge on the hydrogen atoms and a partial negative charge on the oxygen atom. When an ionic compound is placed in water, the positive ends of water molecules are attracted to the negative ions, and the negative ends are attracted to the positive ions. These attractive forces between water molecules and ions (ion-dipole interactions) are strong enough to overcome the lattice energy of the ionic compound, causing the ions to separate and become surrounded by water molecules (hydration). A high dipole moment indicates strong polarity, which is crucial for this process. High specific heat, no colour, and high boiling point are characteristics of water but are not the primary reason for its ability to dissolve ionic compounds.
Water’s ability to dissolve ionic compounds stems primarily from its strong polarity and high dipole moment, which allows it to hydrate (surround and separate) the positive and negative ions.