Concentration Converter

Convert between molarity, normality, % w/v, ppm, mg/L and more

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Result:

1 M = 1 N

What is Concentration?

Concentration quantifies the amount of a substance (solute) dissolved in a given volume of solution. It's a fundamental concept in chemistry, biology, and environmental science, essential for preparing solutions, conducting experiments, and analyzing results.

Why Use This Tool?

This concentration converter is vital for:

  • Laboratory work - preparing accurate solutions
  • Environmental testing - water quality analysis
  • Industrial applications - formulation and quality control
  • Academic studies - chemistry and biology coursework
  • Pharmaceutical preparation - drug formulation
Safety Note: Always verify molar masses and solution densities for accurate conversions in real laboratory work. This tool provides theoretical calculations only.

Conversion Formulas

Molarity to mg/L:
mg/L = mol/L × Molar Mass (g/mol) × 1000
mg/L to Molarity:
mol/L = mg/L ÷ (Molar Mass × 1000)
Molarity to Normality:
Normality = Molarity × n (equivalents)
% w/v calculation:
% w/v = (grams of solute / 100 mL of solution) × 100
ppm calculation (for dilute aqueous solutions):
ppm = mg of solute per liter of solution
ppb calculation:
ppb = µg of solute per liter of solution

Frequently Asked Questions

Molarity (M) is the number of moles of solute per liter of solution. Normality (N) is the number of equivalents of solute per liter of solution. Normality takes into account the reactive capacity of the solute in a specific chemical reaction.

ppm (parts per million) and mg/L are equivalent for dilute aqueous solutions where the density is approximately 1 g/mL. For more concentrated solutions or non-aqueous solutions, you need to consider the solution density.

% w/v (weight/volume) is grams of solute per 100 mL of solution. % w/w (weight/weight) is grams of solute per 100 grams of solution. To convert between them, you need to know the solution density.

The equivalent factor depends on the specific reaction. For acids, it's the number of H+ ions donated. For bases, it's the number of OH- ions donated. For redox reactions, it's the number of electrons transferred. Examples: HCl = 1, H₂SO₄ = 2, NaOH = 1, Ca(OH)₂ = 2.