Titration Molarity Calculator

Enter Calculation

Titrant concentration (mol/L)

Titrant volume used (mL)

Analyte volume (mL)

Analyte stoichiometric coefficient (na)

Titrant stoichiometric coefficient (nb)

Results

Analyte Molarity (Ma)

0.125

mol/L

Moles of titrant added	0.0025 mol
Moles of analyte reacted	0.0025 mol

What is the Titration Molarity Calculator?

This tool determines the unknown concentration (molarity) of an analyte solution from acid–base or redox titration data. At the equivalence point the amount of titrant added is chemically equivalent to the analyte present, so the relationship \(M_a \cdot V_a \cdot n_a = M_b \cdot V_b \cdot n_b\) holds. Here Ma and Mb are the molarities of analyte and titrant, Va and Vb are their volumes, and na/nb are the stoichiometric coefficients from the balanced reaction. The tool is universal — it applies to any titration regardless of country or laboratory.

A titration: titrant of known molarity (Mb, Vb) is added to the analyte (Ma, Va) until the endpoint.

How to use it

Enter the known titrant concentration (mol/L), the titrant volume delivered from the burette at the endpoint (mL), and the volume of analyte pipetted into the flask (mL). Then set the stoichiometric coefficients na and nb. For a simple 1:1 reaction such as HCl + NaOH, both coefficients are 1. For H₂SO₄ + 2NaOH, the acid coefficient (na, if acid is the analyte) is 1 and the base coefficient nb is 2.

The formula explained

Since moles = molarity × volume, equivalence gives \(M_a \cdot V_a \cdot n_a = M_b \cdot V_b \cdot n_b\). Rearranging for the unknown analyte molarity:

$$M_a = \dfrac{M_b \cdot V_b \cdot n_a}{V_a \cdot n_b}$$

Volumes can be entered in mL because the units cancel — only the ratio Vb/Va matters. The calculator also reports moles of titrant added (\(M_b \times V_b/1000\)) and the corresponding moles of analyte reacted.

At the equivalence point the two sides balance: \(M_a \cdot V_a \cdot n_a = M_b \cdot V_b \cdot n_b\).

Worked example

Suppose 25.0 mL of 0.100 mol/L NaOH neutralises 20.0 mL of HCl in a 1:1 reaction. Then

$$M_a = \frac{0.100 \times 25.0 \times 1}{20.0 \times 1} = 0.125 \ \text{mol/L}$$

The HCl solution is 0.125 M.

FAQ

Do volumes need to be in litres? No — as long as Va and Vb use the same unit, the result is correct because the units cancel.

What are na and nb? They are the mole ratio coefficients from the balanced equation. For a diprotic acid titrated with a monoprotic base, use na=1 and nb=2.

Can I use this for redox titrations? Yes. Use the electron-transfer stoichiometry to set na and nb.