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Frenkel Defect

what is the d...

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what is the difference between hydration and lattice enthalpy ? what are their applications ? are they both exothermic

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Q. The lattice enthalpy of solid

N a C l

772 k J {m o l}^{- 1}

and enthalpy of solution is

2 k J {m o l}^{- 1}

. If the hydration enthalpy of

{N a}^{+}

{C l}^{-}

ions are in the ratio of

3 : 2.5

, what is the enthalpy of hydration of chloride ion?

Q. The lattice energy of solid

K C l

is 181 kcal/mol. The enthalpy of solution of

K C l

in water is 1 kcal/mol. If the hydration enthalpies of potassium and chloride ions are in the ratio

2 : 1

, what is the hydration enthalpy (kcal/mol) of potassium ions?

Q. Enthalpy of a solution of

C s B r (s)

10 k J / m o l

. If the enthalpies of hydration of

C s^{+} (g)

B r (g)

are 475 and 655 kJ.mol, what should be the lattice energy of

C s B r (s)

k J / m o l

:

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:

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:

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