Question

Write the formula and calculate the molar mass of Aluminium Nitrate.

Answer 1

Hint: We have to know that salt of nitric acid and aluminium is aluminium nitrate. It appears as white solid and it is dissolved in water. We can calculate the molar mass of a compound using the atomic mass of each element present in the compound. The molar mass of aluminium nitrate using the atomic mass of aluminium, atomic mass of nitrogen, and atomic mass of oxygen.


Complete step by step answer:
We must have to know that the aluminum nitrate may rather be set up by the response of nitric corrosive with aluminium (III) chloride. Nitrosyl chloride is created as a result; it rises out of the arrangement as a gas. All the more advantageously, the salt can be made by responding to nitric acid with aluminum hydroxide.
Aluminium is mostly found in the crust of the earth combined with elements like silicon, oxygen, and fluorine. $Al{\left( {N{O_3}} \right)_3}$ is the chemical formula of aluminium nitrate.
We can determine molar mass of a compound by the atomic mass of each element found in the compound.
The atomic mass of aluminum is $26.98amu$.
The atomic mass of nitrogen is $14.01amu$.
The atomic mass of oxygen is $16.00amu$.
The molar mass of $Al{\left( {N{O_3}} \right)_3}$ is calculated as,
Molar mass of $Al{\left( {N{O_3}} \right)_3}$=$26.98 + 3\left( {14.01 + 16 \times 3} \right)$
Molar mass of $Al{\left( {N{O_3}} \right)_3}$=$213.01g/mol$
The molar mass of $Al{\left( {N{O_3}} \right)_3}$ is $213.01g/mol$.

Note: We must need to know that the melting point and boiling point of aluminum nitrate are $72.8^\circ C$ and $135^\circ C$ respectively. Some of the uses of aluminum nitrate include,
1.Powerful oxidizing agent
2.Corrosion inhibitor
3.Refining of petroleum
4.Core laminators in transformers
5.Extraction of uranium
6.Extraction of actinide elements uses hydrated salts of aluminum nitrate.