Which of the following statements regarding solubility of LiF and LiI in water at room temperature is correct ?
LiI is more soluble than LiF
The solubility of an ionic salt reflects the balance between its lattice enthalpy, which must be overcome, and the hydration enthalpy released when the ions are solvated. For lithium halides the cation is the same, so the difference comes from the anion and from how well the cation and anion sizes match in the lattice.
In LiF both ions are very small, so the lattice is extremely stable (lattice enthalpy about 1030 kJ mol–1) and the hydration energy of the small ions cannot compensate; LiF dissolves only to about 0.13 g per 100 g of water. In LiI the large, polarisable iodide gives a much weaker lattice (about 750 kJ mol–1) and strong partial covalent character, while the small Li+ is still strongly hydrated; LiI is very soluble, about 165 g per 100 g of water.
So the two salts are far from equally soluble, they are not both insoluble (LiI is highly soluble and even deliquescent), and the claim that the fluoride dissolves better than the iodide reverses the observed trend.
LiI is more soluble than LiF option is correct.
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.................... is a client server application that identifies each host on the internet with a unique user-friendly name.
Every OS has a ................ or .......... which primarily resides in the main memory of the computer to perform some of the basic functions of the OS.
(i) Kernel
(ii) Interface
(iii) Nucleus
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(i) Machine language
(ii) Assembly language
(iii) High level language
(iv) Natural language
Codes:
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