Molarity Calculator
Molarity (M, mol/L) is the moles of solute per litre of solution — the workhorse concentration unit in chemistry, biology and pharmacy labs. This tool applies M = n / V = m / (Mw × V) to interchange among molarity M, solute mass m, molar mass Mw and solution volume V. Pick which variable to solve for, enter the other three with the units you prefer, and read both the answer and the equivalent moles of solute n.
Enter three valid positive numbers (the fourth is solved from the formula) and pick a unit for each.
Result
—
Formula
M = n / V = m / (Mw × V)
Enter the other three positive numbers. Mass, molar mass and volume are converted internally to g, g/mol and L; choosing a different unit does not change the answer.
Formula
M = n / V = m / (Mw × V) (n = m / Mw)
- · Unit convention: M in mol/L, m in g, Mw in g/mol, V in L; the widget converts mg / µg / kg, mL / µL and mM / µM / nM to this base before solving.
- · “Volume V” means the FINAL solution volume (solute included) — not the volume of solvent you added. Bringing a 100 mL volumetric flask up to the mark gives V = 100 mL exactly.
- · Mw is the molar mass in g/mol; numerically it equals the molecular weight in daltons (Da). Common solutes are preset (NaCl, NaOH, glucose, sucrose, CaCO₃, …) — pick “Custom” to type your own.
- · Molarity depends slightly on temperature because it uses solution volume; for high-precision analytical work prefer molality (mol per kg of solvent), which is temperature-independent.
- · For hydrated salts (e.g. CuSO₄·5H₂O, Mw = 249.69 g/mol), weigh against the hydrate molar mass. The CuSO₄ preset here is the ANHYDROUS salt (159.61 g/mol).
- · References: IUPAC Gold Book “amount-of-substance concentration”; Skoog, West, Holler & Crouch, Fundamentals of Analytical Chemistry, 10e, §4D.
Frequently asked
What is the difference between molarity (M, mol/L) and mass-by-volume percent (% w/v)?
Molarity (mol/L) counts how many MOLES of solute are in one litre of solution — it tracks particle count, which is what governs chemical reactions, osmotic pressure, pH, and so on. % w/v counts how many GRAMS of solute are in 100 mL of solution — a mass measure, common on pharmacy labels and nutrition panels. The two interconvert as M = (10 × % w/v) / Mw. For example, 0.9 % w/v NaCl ≈ 10 × 0.9 / 58.44 ≈ 0.154 mol/L (the familiar 154 mM "physiological saline"). To use a % w/v figure here, just multiply by 10 and divide by Mw to get M, then enter that.
How do I prepare 1 L of 0.1 M NaCl solution?
Switch the "Solve for" selector to "m (solute mass)", enter M = 0.1 mol/L, Mw = 58.44 g/mol (pick the "NaCl" preset) and V = 1 L — the tool returns m = 5.844 g. In the lab: weigh 5.844 g of NaCl precisely, transfer to a 1 L volumetric flask, dissolve in a smaller amount of deionised water, then add water UP TO the 1 L mark and invert several times to mix. "Bringing the solution to 1 L" is what the molarity definition assumes — it is NOT the same as adding 1 L of water on top of the solute.
For diluting an existing stock, should I use this tool or the dilution formula?
They solve different problems. THIS molarity tool builds a solution from "mass + molar mass + final volume" — use it when you start from a solid powder or a concentrated reagent. If instead you already have a stock at a known molarity and want to dilute it to a lower one (e.g. 10 M HCl down to 1 M), use the dilution equation C₁V₁ = C₂V₂ in the Dilution Calculator — molar mass is not needed there. Short rule: weighing a powder → this tool; diluting an existing stock → the dilution tool.
How do mol/L, mM and µM convert?
They are just scaled versions of "moles per litre of solution": 1 mol/L = 1 M = 1 000 mM = 1 000 000 µM = 1 000 000 000 nM. So 1 mM glucose = 0.001 mol/L and 100 nM antibody = 1 × 10⁻⁷ mol/L. The widget switches freely among M, mM, µM and nM — changing the unit only changes how the answer is displayed; the underlying solve uses the SI base mol/L throughout.
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