Magnesium Concentration Unit Converter

Convert magnesium (Mg) concentration values between molarity (M), mass per volume (mg/L), parts-per-million (ppm), and other common lab units. This tool runs entirely offline, designed for students, researchers, and lab technicians preparing solutions, analyzing samples, or interpreting data.

Educational only. Follow your lab SOPs and SDS.

Converter

Concentration Value

Enter number (supports 1e-3, 2.5, 0,01)

From Unit

Molar Mass of Mg (g/mol) (adjust if using a salt)

Default is atomic mass of elemental Mg. For MgCl₂·6H₂O, use 203.30 g/mol.

Solvent Density (g/mL) (for ppm↔mass/vol conversions)

Default is pure water at ~25°C (1.00 g/mL). Adjust for other solvents.

Decimals:

Conversion Results

Main Result

1.000 M

All Units

Molar (M):1.000

millimolar (mM):1000.00

micromolar (µM):1.000e+6

g/L:24.31

mg/L:24305.0

ppm (in water):24305.0

Notes & Checks

✔ Molar mass used: 24.305 g/mol

✔ Solvent density: 1.00 g/mL

✔ 1 ppm (aqueous) ≈ 1 mg/L

Understanding Magnesium Concentration Conversions

Magnesium is a critical cation in biological buffers, industrial processes, and clinical assays. Converting between molarity and mass concentration is essential for preparing stock solutions, interpreting water hardness reports (often in ppm CaCO₃ equivalents), and adjusting culture media.

How to Use This Tool

Enter your known concentration value in the input field. Use scientific notation (e.g., 2.5e-3) or regular decimals.
Select the unit of your input value from the dropdown.
Adjust the molar mass if you are working with a magnesium salt (e.g., MgSO₄·7H₂O = 246.47 g/mol).
Click "Convert". The results panel updates instantly with values in all common units.
Use "Swap Mass ↔ Molar" to quickly toggle the focus between mass‑based and mole‑based units.

Real‑World Examples

Scenario	Input	Key Outputs	Use‑Case
Cell culture media	0.8 mM	0.0008 M, 19.44 mg/L	Preparing 10× stock
Drinking water standard	30 mg/L	1.234 mM, 30 ppm	Compliance reporting
Sea water Mg²⁺	0.0528 M	52.8 mM, 1283 mg/L	Oceanography studies
IV solution (MgSO₄)	1% w/v (10 g/L)	0.081 M Mg²⁺ (MW 246.47)	Clinical pharmacy

Common Mistakes Checklist

Forgetting to adjust molar mass when using a salt (not elemental Mg).
Assuming ppm always equals mg/L (only true for aqueous solutions with density ≈1 g/mL).
Confusing millimolar (mM) with micromolar (µM) when pipetting.
Neglecting ionic strength effects in concentrated solutions (this converter assumes ideal dilute conditions).

Quick Pair Converter

Instantly convert between two specific units—useful for comparing data sheets or method protocols.

Value

From

Conversion

50 mg/L = 2.058 mM

Formula: mg/L ÷ molar mass (g/mol) = mM

Frequently Asked Questions

What is the difference between ppm and mg/L?

For aqueous solutions with density close to 1 g/mL, 1 ppm = 1 mg/L. For solvents with different densities (e.g., ethanol), ppm is a mass‑per‑mass ratio and conversion requires the solvent density.

When should I adjust the molar mass?

Always adjust when your source material is a magnesium salt (e.g., MgCl₂, MgSO₄·7H₂O). Use the formula weight of the salt, not the atomic mass of Mg (24.305 g/mol). The converter will then give correct mass‑based concentrations for that salt.

How accurate are these conversions for concentrated solutions?

The conversions are mathematically exact for ideal, dilute solutions. In concentrated solutions (>0.1 M), activity coefficients deviate from 1 due to ionic strength, affecting effective concentration. This tool does not correct for non‑ideality.

Can I convert from % w/v to molarity?

Yes. Enter the % w/v value as g/100mL, so 1% w/v = 10 g/L. Select "g/L" as the input unit, adjust the molar mass if needed, and convert to molarity.

What safety precautions are relevant for magnesium solutions?

While magnesium salts are generally low hazard, always consult the SDS for specific salts. Some (e.g., Mg powder) are flammable. High concentrations can be hyperosmotic. Use appropriate PPE (gloves, goggles) and follow waste disposal regulations.

Formulas & Assumptions

• Molarity (M) to mg/L: mg/L = M × molar mass (g/mol) × 1000

• mg/L to ppm (aqueous): ppm = mg/L ÷ solvent density (g/mL)

• Molarity to molality (mol/kg): m ≈ M / (solvent density in kg/L) for dilute solutions.

• Molar mass of elemental Mg: 24.305 g/mol (IUPAC atomic weight).

• Default solvent density: 1.00 g/mL (pure water near 25°C).

• Rounding: Results are rounded to the selected decimal places without trailing zeros in scientific notation.

• Assumption: Ideal dilute solution behavior; no activity corrections.

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Magnesium Concentration Unit Converter

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