🧪 Quantitative Solution Chemistry
Molality, Molarity & Normality Converter
Convert solution concentrations across Molarity ($M$), Molality ($m$), Normality ($N$), Mass Percentage ($\% w/w$), and Mole Fraction with solution density corrections.
🧂 NaCl (1.0 M, eq=1)
⚗️ H₂SO₄ (1.0 M, eq=2)
🧪 HCl (1.0 M, eq=1)
🧪 H₃PO₄ (1.0 M, eq=3)
🧼 NaOH (1.0 M, eq=1)
Solute & Solution Parameters
g/mol
Number of reactive $H^+$, $OH^-$, or electrons transferred.
mol/L
g/mL
Calculated Molality (m)
1.019 m
Mass Percentage (% w/w)
5.62%
Normality (N)
1.000 N
Mass Concentration
58.44 g/L
Mole Fraction ($X_{\text{solute}}$)
0.0180
💡 Physical Chemistry Definition:
1 Liter of this solution weighs 1,040.0 g, containing 58.44 g of solute dissolved in 981.56 g of solvent (water).
Concentration Formulas in Chemistry
Formulas for converting between volume-dependent and mass-dependent concentration units:
- Molarity ($M$): $$M = \frac{\text{moles of solute}}{\text{Liters of solution}}$$
- Normality ($N$): $$N = M \times n_{\text{eq}}$$
- Molality ($m$): $$m = \frac{\text{moles of solute}}{\text{kg of solvent}} = \frac{M}{\rho - \frac{M \times M_w}{1000}}$$
- Mass Percent ($\% w/w$): $$\% = \left(\frac{M \times M_w}{1000 \times \rho}\right) \times 100\%$$