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Reactivity with Halogens and Hydrogen (Group 2)

The solubilit...

Question

The solubility of metal halides depends on their nature, lattice enthalpy and hydration enthalpy of the individual ions. Amongst fluorides of alkali metals, the lowest solubility of $L i F$ in water is due to:

A

ionic nature of lithium fluoride

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B

high lattice enthalpy

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C

high hydration enthalpy for lithium ion

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D

low ionization enthalpy of lithium atom

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Solution

The correct option is D high lattice enthalpy
In $L i F$ , due to the small size of cation and anion, lattice is very strong and so, lattice energy is very high. Due to this high lattice energy, $L i F$ is less soluble in water.

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Q. The solubility of metal halides depends on their nature, lattice enthalpy and hydration enthalpy of the individual ions.
Amongst fluorides of alkali metals, the lowest solubility of

L i F

in water is due to:

Q. Solubility of an ionic compound in water is mainly dependent on:
a. Lattice enthalpy
b. Hydration enthalpy
Both these factors oppose each other, and the resultant of these factors determines the solubility of an ionic compound in water. If the lattice enthalpy has a larger value, the compound is less soluble. If the hydration enthalpy has larger value, the compound is highly soluble in water.

B e F_{2}

is soluble in water while fluorides of other alkaline earth metals are insoluble because of:

Q. Solubility of an ionic compound in water is mainly dependent on:
a. Lattice enthalpy
b. Hydration enthalpy
Both these factors oppose each other, and the resultant of these factors determines the solubility of an ionic compound in water. If the lattice enthalpy has a larger value, the compound is less soluble. If the hydration enthalpy has larger value, the compound is highly soluble in water.

Compounds of alkaline earth metals are less soluble than alkali metals, due to:

Q. Solubility of an ionic compound in water is mainly dependent on:
a. Lattice enthalpy
b. Hydration enthalpy
Both these factors oppose each other, and the resultant of these factors determines the solubility of an ionic compound in water. If the lattice enthalpy has a larger value, the compound is less soluble. If the hydration enthalpy has larger value, the compound is highly soluble in water.

A compound is soluble in water if the hydration enthalpy is:

BeSO₄ is water soluble while CaSO₄ is not. This is because of:

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