Estimate dissolved gases from Henry's law inputs. Switch units, save tables, and review chemistry outputs. Use the calculator for labs, teaching, and quick validation.
These reference values are approximate and editable. They are suitable for learning, screening, and quick estimation.
| Gas | Example kH (mol/L·atm) | Molecular Weight (g/mol) | Comment |
|---|---|---|---|
| Carbon Dioxide | 0.0330 | 44.01 | Common in water treatment and beverage work. |
| Oxygen | 0.0013 | 32.00 | Useful for environmental and biological systems. |
| Nitrogen | 0.00061 | 28.01 | Often used for inert gas estimation. |
| Methane | 0.0014 | 16.04 | Helpful in energy and process studies. |
Henry's Law: C = kH × P
Here, C is dissolved gas concentration, kH is the Henry constant in concentration form, and P is gas partial pressure.
Temperature Adjustment: kH(T) = kH(ref) × exp[ F × (1/T − 1/Tref) ]
T and Tref use Kelvin. F is an adjustable temperature factor. It helps model how solubility changes as temperature changes.
Salt Effect: Ccorrected = Cbase × 10−ks×I
ks is the Setchenov constant and I is ionic strength. This correction reduces gas solubility when dissolved salts are present.
Mass Conversion: g/L = mol/L × molecular weight
Total Dissolved Mass: total mass = g/L × solution volume
Gas solubility is important in chemistry, biology, and process design. It explains how much gas can dissolve in a liquid under fixed conditions. This value changes with pressure, temperature, and solution composition. A reliable estimate helps with planning, testing, and reporting.
Henry's law is a common starting point. It links dissolved concentration to gas partial pressure. When pressure rises, dissolved gas often rises too. This simple relationship is useful for water treatment, beverage systems, environmental checks, and laboratory calculations.
Temperature strongly affects dissolved gas behavior. Many gases become less soluble as temperature increases. Salts can also lower gas solubility. That is why advanced calculations should allow temperature correction and salt correction. This calculator includes both options for faster screening.
Different users need different output units. Some prefer molar concentration. Others need mass concentration in grams per liter or milligrams per liter. Process teams may also want total dissolved mass in a known liquid volume. This tool converts those outputs from one calculation path.
You can use this calculator for classroom examples, method planning, and preliminary design work. It is also helpful for comparing gases, checking pressure effects, and preparing quick estimate tables. It does not replace validated laboratory data, but it gives a strong first estimate.
Always use Henry constants that match your solvent, temperature range, and unit definition. Gas data can vary across references. Solvent density and molar mass also affect mole fraction estimates. If your project is sensitive, confirm every constant before making final decisions. Good inputs create better chemistry outputs.
It estimates how much gas dissolves in a liquid from Henry's law inputs, temperature adjustment, pressure, and optional salt correction.
Higher gas partial pressure usually increases dissolved concentration. Henry's law directly links those two values in many dilute systems.
Gas solubility often decreases as temperature rises. The calculator uses an adjustable factor to model that shift.
It estimates salting-out effects. Dissolved salts can reduce gas solubility, especially in process and environmental samples.
Yes. Choose the custom option and enter your own Henry constant and molecular weight values.
No. They are reference values for quick work. Use source-specific laboratory or literature data for final calculations.
Choose mol/L for chemistry work, mg/L for water reporting, and g/L for mass-based process summaries.
It is best for estimation, comparison, and teaching. Final design work should use validated data and system-specific models.
Important Note: All the Calculators listed in this site are for educational purpose only and we do not guarentee the accuracy of results. Please do consult with other sources as well.