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# 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? Verified
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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 $g{(mol)^{ - 1}}$.

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 $342gmo{l^{ - 1}}$.