Calculate the molar mass of zinc nitrate.

Understand the Problem

The question is asking for the calculation of the molar mass of zinc nitrate, which involves determining the atomic masses of zinc and nitrate components and then summing them up according to their stoichiometric ratios in the compound.

Answer

The molar mass of zinc nitrate is $189.40 \, \text{g/mol}$.

Steps to Solve

Identify the components of zinc nitrate

Zinc nitrate has the chemical formula $Zn(NO_3)_2$. This indicates it contains one zinc (Zn) atom and two nitrate (NO₃) groups.

Determine the atomic masses

Zinc (Zn) has an atomic mass of approximately 65.38 g/mol.
A nitrate (NO₃) group consists of one nitrogen (N) atom and three oxygen (O) atoms. The atomic masses are:
- Nitrogen (N) = 14.01 g/mol
- Oxygen (O) = 16.00 g/mol

Now, calculate the molar mass of the nitrate group: $$ \text{Molar mass of NO}_3 = \text{N} + 3 \times \text{O} = 14.01 , \text{g/mol} + 3 \times 16.00 , \text{g/mol} $$

Calculating this yields: $$ \text{Molar mass of NO}_3 = 14.01 + 48.00 = 62.01 , \text{g/mol} $$

Calculate the total molar mass of zinc nitrate

Now, calculate the total molar mass of $Zn(NO_3)_2$: $$ \text{Molar mass of Zn(NO}_3)_2 = \text{Molar mass of Zn} + 2 \times \text{Molar mass of NO}_3 $$

This can be calculated as follows: $$ = 65.38 , \text{g/mol} + 2 \times 62.01 , \text{g/mol} $$

Final calculation

Now, simplify the expression: $$ \text{Molar mass of Zn(NO}_3)_2 = 65.38 + 124.02 = 189.40 , \text{g/mol} $$

The molar mass of zinc nitrate ($Zn(NO_3)_2$) is approximately $189.40 , \text{g/mol}$.

More Information

Zinc nitrate is commonly used in fertilizers and chemical synthesis. Understanding how to calculate molar masses is a fundamental skill in chemistry that helps in stoichiometry and reaction calculations.

Tips

Failing to account for the number of nitrate groups can lead to incorrect calculations.
Neglecting to use the correct atomic masses of elements can also result in inaccuracies.
Sometimes students forget to multiply the molar mass of the nitrate group by 2 when there are two nitrate ions in the formula.

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