| Compound | Lattice enthalpy (in kJ \[mo{{l}^{-1}}\]) | Hydration enthalpy (in kJ \[mo{{l}^{-1}}\]) |
| P | +780 | -920 |
| Q | +1012 | -812 |
| R | +828 | -878 |
| S | +632 | -600 |
A) P and Q
B) Q and R
C) R and S
D) Q and S
E) P and R
Correct Answer: E
Solution :
The solubility of a compound mainly depends upon its hydration energy. If die hydration energy of a compound is greater than from its lattice enthalpy, then it is soluble in water. Thus for solubility hydration enthalpy > lattice enthalpy For compounds P and R hydration enthalpy exceeds the lattice enthalpy, so they are soluble in water.
You need to login to perform this action.
You will be redirected in
3 sec
