Question

The gram molecular mass of \[F{e_2}{\left( {SO4} \right)_3}\] compound is:
A) \[117.69g\]
B) \[96.18g\]
C) \[405.862g\]
D) \[96.86g\]

Answer 1

Hint: We have to remember that the ferric sulfate appears as a yellow crystalline solid or a grayish-white powder. The primary hazard is the threat to the environment. Immediate steps should be taken to limit its spread to the environment. It is used for water purification, and as a soil conditioner.

Complete answer:
Iron $\left( {{3^ + }} \right)$ sulfate is a compound of iron and sulfate in which the ratio of to sulfate ions is $3:2$. It has a role as a catalyst, a mordant and an astringent. It is a metal sulfate and an iron molecular entity. It contains an . To calculate the molecular mass of ferrous sulfate we need to calculate the mass for individual atoms in order to get the combined mass of ferrous sulfate.
Molecular mass of Iron:
\[ = 2 \times 55.85g\]
On simplification we get,
\[ = 111.7g\]
Molecular mass of Oxygen: \[16g \times 4 = 64g\]
Molecular mass of Sulfur: \[32g\]
Total mass of sulfate:
\[ = 3 \times 98g\]
On simplification we get,
\[ = 294g\]
So on adding the masses in order to get the molecular mass of ferrous sulfate we will get \[405.7g\]
Ferric sulfate is used as a solution generated from iron wastes. The actual speciation is vague but its applications do not demand high purity materials. As such iron (III) sulfate is generated and handled as an aqueous solution. It is produced on a large scale by treating sulfuric acid, a hot solution of ferrous sulfate, and an oxidizing agent.

Note:
We have to know that the ferric sulfate is used in different fields such as dentistry and dermatology. It is thought to present haemostatic properties by interacting chemically with certain blood proteins. Typical oxidizing agents include chlorine, nitric acid, and hydrogen peroxide.