Even though entropy increases in ionic compounds when dissolved in water, not all ionic compounds are soluble.This can be explained by which of the following?

The strength of the intermolecular forces that hold the compound together.

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The strength of the ionic crystalline solid due to the tight arrangement of the atoms and the strong electrostatic forces.

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The high concentration needed to make the substance dissolve in water, which is why low molarities are inadequate for dissolution of some substances.

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The lack of potential energy in the ionic bonds of the solid compound.

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Solution

The correct option is A The strength of the intermolecular forces that hold the compound together.
For an ionic compound to dissociate, the forces of attraction between its component ions and the surrounding water molecules must be greater than the forces of attraction between the ions within the compound.

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Similar questions

Q. Choose the correct option regarding the statements given below:
Statement 1: Ionic compounds have high boiling points.
Statement 2: In ionic bonds the oppositely charged ions are held together by strong electrostatic forces of attraction.

Statement 1: Ionic compounds have high boiling points.
Statement 2: The oppositely charged ions are held together by strong electrostatic forces of attraction and require more heat energy to break the bonds.

Q. Statement 1: Ionic compounds only dissolve in water.
Statement 2: Hydration is the process of dissolving an ionic solid in water.

Q. A number of ionic compounds, e.g.

A g C l, C a F_{2}, B a S O_{4}

are insoluble in water. This is because:

Q. Two substance

X

and

Y

are dissolved in water under suitable conditions.

X

is a gas while Y is a solid under normal conditions. The solution of

Y

is found to conduct electricity but not '

X

'. Based on the conclusion identify the nature of bond present in

X

and

Y

with appropriate reasons as given below.

Arrange the steps given below in a sequence.
(a)

Y

is a solid at room temperature and its aqueous solution conducts electricity. This show that it is an ionic compound.
(b)

X

on dissolution in water doesn't conduct electricity and is a gas at room temperature. Hence it should be a non-polar covalent molecule.
(c) Aqueous solutions of both ionic compounds and polar covalent compounds conduct electricity because of the presence of free ions.
(d) All ionic compounds are solids and most of the non-polar covalent molecules are gases or solids at room temperature. Polar covalent compounds are liquids or gases.

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