Question

The molar mass of barium nitrate (\[Ba{(N{O_3})_2}\]) is $261.35g/mol$. What is the mass of \[5.30 \times {10^{22}}\] formula units of \[Ba{(N{O_3})_2}\]?

Answer 1

Hint: We need to know that the barium nitrate is an inorganic salt which is composed of barium and nitrate ions having chemical formula \[Ba{(N{O_3})_2}\], Most of the barium salts, is colorless, toxic, and water-soluble. It burns with a green flame and is an oxidizer. It is found in white crystals having an odorless smell. The crystals of barium nitrate are lustrous in nature.

Complete answer:
We will solve this question step by step: It is a fact that \[6.022 \times {10^{23}}\] formula units of barium nitrate have a mass of $261.35g/mol$. This is what we specify when we say molar mass. And thus the mass of \[5.30 \times {10^{22}}\] formula units of barium nitrate is the quotient multiplied by the molar mass:
The mass of \[5.30 \times {10^{22}}\] formula units of \[Ba{(N{O_3})_2}\]
\[ = \dfrac{{5.30 \times {{10}^{22}}}}{{6.022 \times {{10}^{23}}}}mol \times 261.35g/mol\]
On simplification we get,
$ = 230 \times {10^{ - 1}}g$
Avogadro's number, number of units in one mole of any substance (defined as its molecular weight in grams), equal to \[6.022 \times {10^{23}}\]. The units may be electrons, atoms, ions, or molecules, depending on the nature of the substance and the character of the reaction. One mole of a substance is equal to \[6.022 \times {10^{23}}\] units of that substance (such as atoms, molecules, or ions).

Note:
We have to remember that barium nitrate enhances the combustibility of many compounds even if it is not combustible. We have to know that it cannot be boiled as it decomposes on high temperature. It is an oxidizing agent which helps others to get burned. We need to remember that it is widely used in paints, in making explosives and it is also used in making green signal lights.