Question

The formula for aluminum sulfate is \[A{l_2}{(S{O_4})_3}\]. What is the molar mass of aluminum sulfate to the nearest gram?

Answer 1

Hint: The mass of a given chemical element or chemical compound (g) divided by the volume of material is the molar mass (mol). The molar mass of a compound can be determined by adding the constituent atoms' normal atomic masses. It is denoted by \[g{(mol)^{ - 1}}\].

Complete answer:
We know that aluminum sulfate is an aluminum salt composed of aluminum, sulfur, and oxygen elements. The molar mass of aluminium sulphate, \[Al{(S{O_4})_3}\], would be equal to the number of the molar masses of all the atoms that make up a mole of this compound.
Here, 1 mole of aluminium sulphate contains two moles of aluminium, three moles of sulfur and twelve moles of oxygen.
That is,
1. \[2 \times Al\]
2. \[3 \times S\]
3. \[3 \times 4 \times O\]
From the periodic table we know that,
\[{M_{MAl}} = 26.981g{(mol)^{ - 1}}\]
\[{M_{MS}} = 32.065g{(mol)^{ - 1}}\]
\[{M_{MO}} = 15.994g{(mol)^{ - 1}}\]
So to find the molar mass of aluminium sulphate,
\[2 \times {M_{MAl}} + 3 \times {M_{MS}} + 12 \times {M_{MO}}\]
That is, \[2 \times 26.981 + 3 \times 32.065 + 12 \times 15.9994\]
Therefore, \[{M_{MA{l_2}{{(S{O_4})}_3}}} = 342.1508gmo{l^{ - 1}}\]
That is, \[{M_{MA{l_2}{{(S{O_4})}_3}}} = 342gmo{l^{ - 1}}\]
Hence, the molar mass of aluminum sulfate to the nearest gram is \[342gmo{l^{ - 1}}\].

Additional Information:
When it comes to setting up an experiment, molar mass is crucial. The molar mass helps you to figure out how much you can weigh out on your scale while evaluating principles concerning specific quantities of a drug.

Note:
Remember that the molar mass of a compound would be equal to the number of the molar masses of all the atoms that make up a mole of this compound. The molar mass by molecular weight is actually the sum of the total mass in grams of the atoms present to make up a molecule per mole. The unit of molar mass is grams by mole.