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The molecular formula of Nitric acid is HNO₃, consisting of 1 hydrogen atom (H), 1 nitrogen atom (N), and 3 oxygen atoms (O). The molecular weight (or molar mass) of a compound is calculated by summing the atomic weights of all atoms in the molecule.
Using standard atomic masses:
Hydrogen (H) = 1.008 g/mol
Nitrogen (N) = 14.007 g/mol
Oxygen (O) = 16.000 g/mol
The molecular weight of HNO₃ is calculated as follows:
Molecular weight=(1×1.008)+(1×14.007)+(3×16.000)\text{Molecular weight} = (1 \times 1.008) + (1 \times 14.007) + (3 \times 16.000)Molecular weight=(1×1.008)+(1×14.007)+(3×16.000) =1.008+14.007+48.000= 1.008 + 14.007 + 48.000=1.008+14.007+48.000 =63.015≈63.012 g/mol= 63.015 \approx 63.012 \, \text{g/mol}=63.015≈63.012g/mol
Nitric acid is a strong mineral acid widely used in chemical synthesis, fertilizers, explosives, and laboratory applications. Its precise molecular weight is important for stoichiometric calculations, solution preparation, and titrations in analytical chemistry.
Other options are incorrect because they do not match the exact sum of atomic weights:
65.012 g/mol, 70.012 g/mol, and 81.011 g/mol exceed the correct molecular mass of HNO₃.
Understanding the molecular weight of compounds like nitric acid is essential in inorganic chemistry, as it allows students and chemists to calculate moles, concentrations, and reactant quantities in chemical reactions. Accurate calculation ensures safe and effective chemical handling in industrial and laboratory settings.
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