Convert between different units of molar concentration with precision and ease. From moles per liter to millimoles per liter, micromoles per liter, and more - get accurate conversions instantly.
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About Molar Concentration
What is Molar Concentration?
Molar concentration, commonly known as molarity, is the fundamental unit of concentration in chemistry and biochemistry. It represents the number of moles of solute dissolved per liter of solution. The molarity formula is:
Molarity (M) = moles of solute / liters of solution
This definition makes molarity the most practical concentration unit for chemical reactions, as it directly relates to the number of molecules or ions present in a given volume. One mole contains exactly 6.022 × 10²³ particles (Avogadro's number), making molarity essential for stoichiometric calculations.
Common Molar Concentration Units and Conversions
| Unit | Symbol | Definition | Conversion to mol/L |
|---|---|---|---|
| Molar | M | moles per liter | 1 M = 1 mol/L |
| Millimolar | mM | millimoles per liter | 1 mM = 0.001 mol/L |
| Micromolar | μM | micromoles per liter | 1 μM = 10⁻⁶ mol/L |
| Nanomolar | nM | nanomoles per liter | 1 nM = 10⁻⁹ mol/L |
| Picomolar | pM | picomoles per liter | 1 pM = 10⁻¹² mol/L |
| Femtomolar | fM | femtomoles per liter | 1 fM = 10⁻¹⁵ mol/L |
Types of Concentration Measurements
| Type | Formula | Units | Real-world Example |
|---|---|---|---|
| Molarity | moles solute / L solution | mol/L, M | Blood glucose: 5.5 mM |
| Molality | moles solute / kg solvent | mol/kg, m | Antifreeze: 1.5 m ethylene glycol |
| Normality | equivalents / L solution | eq/L, N | Acid-base titrations: 0.1 N HCl |
| Parts per million | mg solute / kg solution | ppm | Drinking water: 10 ppm fluoride |
Molar Concentration Measurement Tools
Laboratory Equipment
- Volumetric flasks: Precise solution preparation with ±0.1% accuracy
- Analytical balances: Mass measurements to 0.0001 g precision
- Pipettes and burettes: Accurate volume delivery for titrations
- pH meters: Hydrogen ion concentration measurement
- Spectrophotometers: Concentration determination via absorbance
- Conductivity meters: Ionic concentration measurement
Modern Analytical Methods
- HPLC (High-Performance Liquid Chromatography): Separation and quantification
- Mass spectrometry: Molecular weight and concentration analysis
- Atomic absorption spectroscopy: Metal ion concentration
- Ion-selective electrodes: Specific ion concentration measurement
- Enzymatic assays: Biological molecule quantification
- Colorimetric methods: Visual concentration determination
Molarity - Mass - Volume Relationships
Understanding the relationships between molarity, mass, and volume is crucial for solution preparation and analysis.
Key Formulas:
Molarity = moles solute / liters solution
Moles = mass (g) / molar mass (g/mol)
Mass = moles × molar mass (g/mol)
Volume = moles / molarity (L)
Example Calculation:
To prepare 500 mL of 0.1 M NaCl solution: Molar mass of NaCl = 58.44 g/mol
Moles needed = 0.1 mol/L × 0.5 L = 0.05 mol
Mass needed = 0.05 mol × 58.44 g/mol = 2.922 g NaCl
Frequently Asked Questions About Concentration Molar Conversion
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