Question

What would be the formula of a barium iodide hydrate that contains $0.0243.mol.Ba{I_2}$ and $0.75mol$ water?

Answer 1

Barium iodide hydrate is an ionic compound with the molecular formula of $Ba{I_2}.n{H_2}O$ . Given that the formula of a barium hydrate contains $0.0243.mol.Ba{I_2}$ and $0.75mol$ water. By dividing the moles of each molecule with the moles of barium iodide as it is small to determine the formula of a barium hydrate.

Complete Step By Step Answer:
Ionic compounds are the compounds that are formed by the combination of atoms other than carbon and hydrogen. Hydrated salts are the compounds that consist of water molecules along with salt. Hydrated salts are the salts that do not have water molecules.
Given that the formula of a barium iodide hydrate contains $0.0243.mol.Ba{I_2}$ and $0.75mol$ water.
The number of moles of barium iodide is $0.0243mol$
The number of moles of water is $0.75mol$
Mole ratio will be obtained by dividing the moles of two molecules or groups with the moles of barium iodide as the moles of barium iodide is small.
$Ba{I_2}:{H_2}O = \dfrac{{0.0243}}{{0.0243}}:\dfrac{{0.75}}{{0.0243}}$
From the above calculation, the simplest mole ratio will be $Ba{I_2}:{H_2}O = 1:30$
Thus, the moles of barium iodide and water in the formula of a barium hydrate is $Ba{I_2}:{H_2}O = 1:30$
Thus, the formula of a barium iodide hydrate that contains $0.0243.mol.Ba{I_2}$ and $0.75mol$ water is $Ba{I_2}30{H_2}O$

Note:
In any compound, the ratio of moles gives the mole ratio of elements or molecules in that compound. The important point is the moles of each molecule or element should be divided with the element or molecule containing a small number of moles only.