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Relation Between r and a

Do ionic comp...

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Do ionic compounds always have hydration enthalpy more than lattice enthalpy?

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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:

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.

B e F_{2}

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

Q. Which of the following alkaline earth metal sulphates has hydration enthalpy higher than the lattice enthalpy?

Q. The lattice enthalpy and hydration enthalpy of four compounds are given below:

Compound	Lattice enthalpy $(k J / m o l)$	Hydration enthalpy $(k J / m o l)$
$P$	$+ 780$	$- 920$
$Q$	$+ 1012$	$- 812$
$R$	$+ 828$	$- 878$
$S$	$+ 632$	$- 600$

The pair of compounds which is soluble in water is:

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