Molarity Calculator with Molality & Normality
All-in-one professional chemistry concentration tool
Common Compounds & Equivalents
| Compound | MW | n-factor | Example |
|---|---|---|---|
| HCl | 36.46 | 1 | 0.1 N = 0.1 M |
| H₂SO₄ | 98.08 | 2 | 0.1 N = 0.05 M |
| NaOH | 40.00 | 1 | 1 N = 40 g/L |
| KMnO₄ (acid) | 158.03 | 5 | 0.1 N = 3.161 g/L |
| K₂Cr₂O₇ | 294.18 | 6 | 49.03 g/L = 1 N |
| Ca(OH)₂ | 74.10 | 2 | 1 N = 37.05 g/L |
Free Online Molarity, Molality & Normality Calculator (2025 Updated)
Say “Bye-Bye” to Chemistry Concentration Calculations! Terms like molarity, molality, normality sound good only in textbooks but calculating them practically has become a common struggle for every student and professional. A small mistake can ruin your entire experiment accuracy, cost you precious marks in exams, and waste your valuable time. To solve this problem, we have brought the most advanced and free online molarity calculator of 2025!
Whether you’re a student preparing for exams, a lab technician creating perfect solutions, or a researcher researching precise titrations, this tool will be a reliable companion. It’s lightning fast, scientifically accurate, and specially designed so you can easily convert grams to moles, find the correct mass of solvent, or avoid the confusion of equivalence factors.
Try it today and join the thousands of students and professionals around the world who already rely on this trusted calculator – now you too can confidently say, “My Chemistry, My Choice!”
What is Molarity? (M = mol/L)
Molarity (M) is the most commonly used unit of concentration in chemistry. It tells you how many moles of solute are dissolved in one liter of solution.
Formula:
Molarity (M) = moles of solute / volume of solution in liters
M = n / V (L)
Example:
How to prepare 500 mL of 0.1 M NaCl solution?
- Moles needed = 0.1 mol/L × 0.5 L = 0.05 mol
- Mass of NaCl = 0.05 mol × 58.44 g/mol = 2.922 grams
What is Molality? (m = mol/kg)
Molality (m) is used when temperature changes affect the volume of the solution (common in colligative properties like boiling/freezing point).
Formula:
Molality (m) = moles of solute / mass of solvent in kilograms
m = n / kg solvent
Example:
Calculate the molality if 9.0 g of glucose (C₆H₁₂O₆, MW = 180 g/mol) is dissolved in 500 g of water.
- Moles of glucose = 9 / 180 = 0.05 mol
- Mass of solvent = 0.5 kg
- Molality = 0.05 / 0.5 = 0.1 m
What is Normality? (N = equivalents/L)
Normality (N) is widely used in acid-base and redox titrations. It depends on the n-factor (number of H⁺, OH⁻, or electrons transferred per molecule).
Formula:
Normality (N) = Molarity (M) × n-factor
N = M × n
Common n-factors:
| Compound | Reaction Type | n-factor |
|---|---|---|
| HCl | Acid | 1 |
| H₂SO₄ | Acid (full) | 2 |
| NaOH | Base | 1 |
| KMnO₄ | Acidic medium | 5 |
| K₂Cr₂O₇ | Acidic medium | 6 |
| Oxalic acid | Redox | 2 |
Example:
0.1 M H₂SO₄ has Normality = 0.1 × 2 = 0.2 N
Quick Reference Table – Popular Solutions
| Solution | Concentration | Mass per Liter | Notes |
|---|---|---|---|
| 1 M NaCl | 1 mol/L | 58.44 g | Physiological saline ~0.15 M |
| 1 N H₂SO₄ | 1 eq/L | 49.04 g | = 0.5 M H₂SO₄ |
| 0.1 N KMnO₄ (acidic) | 0.1 eq/L | 3.161 g | Standard in redox titrations |
| 1 M Glucose | 1 mol/L | 180.16 g | Used in IV drips (5% = 0.278 M) |
| 1 N NaOH | 1 eq/L | 40.00 g | Standard base solution |
Why Use Our Calculator?
- 100% free & no registration
- Works on phone, tablet, and desktop
- Auto-converts mL ↔ L and g ↔ kg
- Pre-loaded n-factors for common compounds
- Accurate to 6 decimal places
Bookmark this page now — you’ll thank yourself during lab work and exams!
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Frequently Asked Questions
What is the difference between molarity and molality?
Molarity (M) = moles of solute per liter of solution (volume-based). It changes slightly with temperature because solution volume expands/contracts.
Molality (m) = moles of solute per kilogram of solvent (mass-based). It is independent of temperature — ideal for boiling/freezing point calculations.
When should I use normality instead of molarity?
Use normality in:
Acid-base titrations
Redox titrations
Precipitation reactions involving equivalents Example: 0.1 M H₂SO₄ = 0.2 N (because it donates 2 H⁺), but 0.1 M HCl = 0.1 N.
How do I convert molarity to normality?
Normality (N) = Molarity (M) × n-factor Just multiply molarity by the number of H⁺, OH⁻, or electrons transferred per formula unit.
Can I calculate the mass needed to prepare a solution?
Yes! Select “Mass” as the target, enter desired concentration and volume — the calculator instantly tells you how many grams to weigh.
