Molar Mass of Nitric Acid (HNO3)
Molar Mass of Nitric Acid gives a reliable base for titration work, where even small mass errors can shift final concentration. Molar Mass of HNO₃ is 63.01 g/mol, based on 3 element types, with O contributing the largest share.
For fast checks, use the molar mass calculator, verify element values in the periodic table, or explore more molar mass page.
Molar Mass of Nitric Acid is:
63.01 g/mol
Molar Mass of HNO₃ equals 63.01 g/mol, so 63.01 grams is one mole.
Element Breakdown Table
| Element | Count | Atomic mass | Calculation | Contribution |
|---|---|---|---|---|
| Hydrogen (H) | 1 | 1.01 | 1 x 1.01 | 1.01 g/mol |
| Nitrogen (N) | 1 | 14.01 | 1 x 14.01 | 14.01 g/mol |
| Oxygen (O) | 3 | 16.00 | 3 x 16.00 | 48.00 g/mol |
Final molar mass 1.010 + 14.010 + 48.000 | 63.01 g/mol | |||
Computing Molar Mass of Nitric Acid Step by Step
Molar Mass of Nitric Acid: Step-by-Step Calculation
1. Identify Element Counts
Read HNO3 and list how many atoms of each element are present:
- 1 atom of Hydrogen (H)
- 1 atom of Nitrogen (N)
- 3 atoms of Oxygen (O)
2. Determine Atomic Masses
Look up each element mass from the periodic table:
- Hydrogen (H) ~= 1.008 g/mol
- Nitrogen (N) ~= 14.007 g/mol
- Oxygen (O) ~= 15.999 g/mol
3. Multiply Atomic Mass by Quantity
Multiply atom count by atomic mass for each element:
- Hydrogen (H): 1 x 1.008 = 1.010 g/mol
- Nitrogen (N): 1 x 14.007 = 14.010 g/mol
- Oxygen (O): 3 x 15.999 = 48.000 g/mol
4. Sum Total Molar Mass
Add all contributions to get the final molar mass in g/mol.
Molar Mass = (1 x 1.008 + 1 x 14.007 + 3 x 15.999)
Molar Mass = 1.010 + 14.010 + 48.000
Molar Mass = 63.010 g/mol
Final rounded value shown on this page: 63.01 g/mol.
Visual Calculation Chart
| Element | Count | Mass | Count x mass | Contribution |
|---|---|---|---|---|
| Hydrogen (H) | 1 | 1.008 | 1 x 1.008 | = 1.010 |
| Nitrogen (N) | 1 | 14.007 | 1 x 14.007 | = 14.010 |
| Oxygen (O) | 3 | 15.999 | 3 x 15.999 | = 48.000 |
Final molar mass 1.010 + 14.010 + 48.000 | = 63.010 | |||
Easy Way to Remember
Easy way to remember Molar Mass of Nitric Acid
- Molar Mass of Nitric Acid: count atoms, multiply masses, and add totals.
- Write each element in a table so you do not miss subscripts.
- Keep 2-3 decimals during steps, then round only at the end.
Sample Reactions
| Type | Reaction |
|---|---|
| Neutralization | HCl + NaOH → NaCl + H₂O |
| Acid-carbonate | ₂HNO₃ + CaCO₃ → Ca(NO₃)₂ + H₂O + CO₂ |
Use these reactions with molar mass calculations when you need the molar mass for each species.
Do You Know?
– Nitric Acid contains 3 element types: H, N, O.
– O contributes the largest share of this compound's total molar mass.
– In HNO₃, O appears with the highest atom count.
– Its molar mass is 63.01 g/mol, which is used directly in gram-to-mole conversions.
– A common reaction for Nitric Acid is neutralization (HCl + NaOH → NaCl + H₂O).
Why This Compound Matters
Nitric Acid is important in acid-base work, especially when preparing safe measured solutions in lab sessions.
O chemistry is frequently tested in titration and neutralization chapters.
Similar calculations can be compared with Nitrous Acid (HNO2) and Sulfuric Acid (H2SO4).
Where This Is Used
- Competitive exams and school chemistry tests.
- Lab work when preparing measured solutions.
- Real-world manufacturing and quality checks.
Common Mistakes When Calculating This
- Skipping subscripts in HNO₃ and miscounting atoms.
- Rounding atomic masses too early before finishing all multiplication steps.
- Mixing up O element contribution with total molar mass.
- Reporting a value without units; final answer should be in g/mol for Nitric Acid.
Quick Revision
Formula: HNO3
Molar Mass: 63.01 g/mol
Key takeaway: count atoms accurately, multiply by atomic masses, and sum only at the end.
Formula Explanation
HNO3 contains Hydrogen (H) (1), Nitrogen (N) (1), Oxygen (O) (3). Add each element contribution to get total molar mass.
FAQ
Conclusion
Molar Mass of Nitric Acid and Molar Mass of HNO₃ are now easy to revise with this structured page. You can use this method in exams, lab reports, and daily chemistry practice.