Molarity Calculator

Calculate the molarity of a solution. Enter solute mass, solute formula weight (MW), and final volume of the solution.

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Solution Formulation

Specify mass, formula weight, and volume.

Calculated Molarity

1.000 M

* Equal to 1000.0 mM (millimolar).

Total Moles of Solute 0.100 mol
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Temperature Dependency

Liquid volume expands with rising temperature, slightly lowering molarity. For high-precision thermal work, use molality.

Common Laboratory Reagent Molecular Weights Reference Table

Chemical Compound Chemical Formula Molecular Weight (g/mol) Typical Stock Concentration
Sodium Chloride (NaCl) NaCl 58.44 g/mol 5 M (292.2 g/L)
Tris Base C₄H₁₁NO₃ 121.14 g/mol 1 M (121.1 g/L)
EDTA Disodium Salt C₁₀H₁₄N₂Na₂O₈·2H₂O 372.24 g/mol 0.5 M (186.1 g/L at pH 8.0)
Glucose (Dextrose) C₆H₁₂O₆ 180.16 g/mol 1 M (180.2 g/L)

Methodology & Equations

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Molarity Formula

Molarity (M) = (Mass / MW) / Volume (L)

Molarity ($M$) equals total solute moles divided by solution volume in liters.

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Preparation Protocol

Weigh solid solute, dissolve in ~80% final volume of solvent, then adjust final volume using a volumetric flask.

Frequently Asked Questions

What is Molarity (M)?

Molarity (M) is the molar concentration of a solution, defined as the number of moles of solute dissolved per liter of solution (mol/L).

How does Molarity differ from Molality?

Molarity measures moles of solute per liter of final solution ($V_{}$) and changes slightly with temperature, whereas Molality measures moles of solute per kilogram of pure solvent ($m_{}$) and is temperature-independent.

How do I prepare a 1 M NaCl solution?

Weigh 58.44 g of pure NaCl (molecular weight = 58.44 g/mol). Dissolve it in approximately 800 mL of deionized water, then bring the total solution volume to exactly 1.0 L in a volumetric flask.

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