Molar Mass of Copper(II) Hydrogen Carbonate (Cu(HCO3)2)
Molar Mass of Copper(II) Hydrogen Carbonate makes it easier to move between measured grams and moles in classroom precipitation problems. Molar Mass of Cu(HCO₃)₂ is 185.58 g/mol, based on 4 element types, with O contributing the largest share.
For fast checks, use the calculate molar mass, verify element values in the periodic table with molar mass, or explore more molar mass.
Molar Mass of Copper(II) Hydrogen Carbonate is:
185.58 g/mol
Molar Mass of Cu(HCO₃)₂ equals 185.58 g/mol, so 185.58 grams is one mole.
Element Breakdown Table
| Element | Count | Atomic mass | Calculation | Contribution |
|---|---|---|---|---|
| Copper (Cu) | 1 | 63.55 | 1 x 63.55 | 63.55 g/mol |
| Hydrogen (H) | 2 | 1.01 | 2 x 1.01 | 2.02 g/mol |
| Carbon (C) | 2 | 12.01 | 2 x 12.01 | 24.02 g/mol |
| Oxygen (O) | 6 | 16.00 | 6 x 16.00 | 95.99 g/mol |
Final molar mass 63.550 + 2.020 + 24.020 + 95.990 | 185.58 g/mol | |||
Computing Molar Mass of Copper(II) Hydrogen Carbonate Step by Step
Molar Mass of Copper(II) Hydrogen Carbonate: Step-by-Step Calculation
1. Identify Element Counts
Read Cu(HCO3)2 and list how many atoms of each element are present:
- 1 atom of Copper (Cu)
- 2 atoms of Hydrogen (H)
- 2 atoms of Carbon (C)
- 6 atoms of Oxygen (O)
2. Determine Atomic Masses
Look up each element mass from the periodic table:
- Copper (Cu) ~= 63.546 g/mol
- Hydrogen (H) ~= 1.008 g/mol
- Carbon (C) ~= 12.011 g/mol
- Oxygen (O) ~= 15.999 g/mol
3. Multiply Atomic Mass by Quantity
Multiply atom count by atomic mass for each element:
- Copper (Cu): 1 x 63.546 = 63.550 g/mol
- Hydrogen (H): 2 x 1.008 = 2.020 g/mol
- Carbon (C): 2 x 12.011 = 24.020 g/mol
- Oxygen (O): 6 x 15.999 = 95.990 g/mol
4. Sum Total Molar Mass
Add all contributions to get the final molar mass in g/mol.
Molar Mass = (1 x 63.546 + 2 x 1.008 + 2 x 12.011 + 6 x 15.999)
Molar Mass = 63.550 + 2.020 + 24.020 + 95.990
Molar Mass = 185.580 g/mol
Final rounded value shown on this page: 185.58 g/mol.
Visual Calculation Chart
| Element | Count | Mass | Count x mass | Contribution |
|---|---|---|---|---|
| Copper (Cu) | 1 | 63.546 | 1 x 63.546 | = 63.550 |
| Hydrogen (H) | 2 | 1.008 | 2 x 1.008 | = 2.020 |
| Carbon (C) | 2 | 12.011 | 2 x 12.011 | = 24.020 |
| Oxygen (O) | 6 | 15.999 | 6 x 15.999 | = 95.990 |
Final molar mass 63.550 + 2.020 + 24.020 + 95.990 | = 185.580 | |||
Easy Way to Remember
Easy way to remember Molar Mass of Copper(II) Hydrogen Carbonate
- Molar Mass of Copper(II) Hydrogen Carbonate: 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 |
|---|---|
| Double displacement | AgNO₃ + NaCl → AgCl + NaNO₃ |
| Acid-salt reaction | Na₂CO₃ + ₂HCl → ₂NaCl + H₂O + CO₂ |
Do You Know?
– Copper(II) Hydrogen Carbonate contains 4 element types: Cu, H, C, O.
– O contributes the largest share of this compound's total molar mass.
– In Cu(HCO₃)₂, O appears with the highest atom count.
– Its molar mass is 185.58 g/mol, which is used directly in gram-to-mole conversions.
– A common reaction for Copper(II) Hydrogen Carbonate is double displacement (AgNO₃ + NaCl → AgCl + NaNO₃).
Why This Compound Matters
Copper(II) Hydrogen Carbonate appears in ionic-reaction practice and precipitation examples in school chemistry.
Its molar mass helps students move quickly between grams, moles, and concentration problems.
Similar calculations can be compared with Copper(II) Acetate (Cu(C2H3O2)2) and Sodium Bicarbonate (NaHCO3).
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 Cu(HCO₃)₂ and miscounting atoms.
- Forgetting that parentheses in Cu(HCO₃)₂ multiply the entire grouped part.
- Mixing up O element contribution with total molar mass.
- Reporting a value without units; final answer should be in g/mol for Copper(II) Hydrogen Carbonate.
Spot a slip early by comparing your work with molar mass before you hand in a final value.
Quick Revision
Formula: Cu(HCO3)2
Molar Mass: 185.58 g/mol
Key takeaway: count atoms accurately, multiply by atomic masses, and sum only at the end.
Formula Explanation
Cu(HCO3)2 contains Copper (Cu) (1), Hydrogen (H) (2), Carbon (C) (2), Oxygen (O) (6). Add each element contribution to get total molar mass.
FAQ
Conclusion
Molar Mass of Copper(II) Hydrogen Carbonate and Molar Mass of Cu(HCO₃)₂ are now easy to revise with this structured page. You can use this method in exams, lab reports, and daily chemistry practice.