M = 58.440 g/mol
| Molarity | 1.8321 mol/L |
| Molality | 1.9013 mol/kg |
| Mass percent (% w/w) | 10 % |
| Mass/volume percent (% w/v) | 10.707 g/100 mL |
| Mass concentration | 107,070 mg/L |
| Parts per million (by mass) | 100,000 ppm |
| Mole fraction of solute | 0.033117 |
Worked on 1 L of solution: 1,070.7 g in total, of which 107.07 g is NaCl and 963.63 g is H2O. ppm here is by mass (mg per kg of solution); for dilute water solutions it is close to mg/L.
How it works
The converter works on one litre of solution. The density gives its total mass, your value gives the grams of solute in that litre, and the rest is solvent. From there, molarity, molality, mass percent, mg/L, ppm and mole fraction all follow using the molar masses of solute and solvent.
Density matters for conversions between volume-based measures (molarity, % w/v, mg/L) and mass-based ones (molality, % w/w, ppm, mole fraction). For dilute aqueous solutions, a density of 1.00 g/mL is a good approximation; for concentrated solutions, look up the density at your concentration and temperature.
Frequently asked questions
- How do I convert molarity to molality?
- You need the solution density. Find the mass of 1 L of solution, subtract the mass of solute to get the mass of solvent, then divide moles of solute by kilograms of solvent.
- Is ppm the same as mg/L?
- For dilute water solutions, very nearly: 1 L of dilute solution weighs about 1 kg, so 1 mg/L ≈ 1 mg/kg = 1 ppm. For dense or concentrated solutions they differ.
- What is the difference between % w/w and % w/v?
- % w/w is grams of solute per 100 g of solution; % w/v is grams per 100 mL of solution. They are equal only when the density is 1 g/mL.
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