Grams per mL to Grams per cm³ Density Converter
Common Conversions
| g/mL | g/cm³ |
|---|---|
| 0.1 | 0.1 |
| 0.5 | 0.5 |
| 1 | 1 |
| 2 | 2 |
| 5 | 5 |
| 10 | 10 |
| 25 | 25 |
| 50 | 50 |
| 100 | 100 |
| 1000 | 1000 |
Why this conversion matters in chemistry
Digital densimeter output reads in g/mL, like a 1.050 g/mL 5% NaCl brine standard from solution-prep certification. The volumetric-glassware calibration document for the same lab writes the same density in g/cm³. Same number, different convention — solution chemistry reaches for g/mL, while materials science and physics tend to write g/cm³. The identity is just a relabeling, but it's the relabeling that has to happen every time a density value crosses between those two worlds.
Formula
g/cm³ = g/mL × 1 (numerically identical)
Worked Examples
1 g/mL = 1 g/cm³
Water at 4 °C — the density anchor that pins both notations together.
1.84 g/mL = 1.84 g/cm³
Concentrated H₂SO₄ — the reagent-bottle density expressed in physics-style units.
0.684 g/mL = 0.684 g/cm³
Hexane at 20 °C — a typical low-density organic-solvent reference.
Frequently Asked Questions
Are g/mL and g/cm³ the same?
Yes — exactly. 1 mL ≡ 1 cm³ by the modern definition of the liter, so a density value transfers between the two notations without arithmetic. The choice between them is purely stylistic.
Why do references vary on the notation?
Solution chemistry and pharmacy default to g/mL; physics and materials science prefer g/cm³. Both notations describe the same physical quantity and produce the same numerical value.
How does solution density feed into molarity?
For concentrated stock acids, molarity = (density × 1000 × mass fraction) / molar mass. So concentrated HCl at 1.19 g/mL and 37% w/w lands at (1.19 × 1000 × 0.37) / 36.46 ≈ 12.1 M — the bottle concentration any dilution calculation starts from.