Titration Calculator

Titration is a lab technique used to find the unknown concentration of an acid or base by reacting it with a solution of known concentration until neutralization is reached. Enter your analyte volume, titrant volume, titrant molarity, and the number of H⁺/OH⁻ ions per molecule into the Titration Calculator to find the Analyte Molarity. Secondary outputs include moles of analyte, moles of titrant, and the equivalence ratio.

mL

Volume of the unknown solution being analyzed

M

Leave blank if this is what you want to calculate

Number of hydrogen ions donated (e.g., HCl = 1, H₂SO₄ = 2)

mL

Volume of known solution added to reach endpoint

M

Known concentration of titrant solution

Number of hydroxide ions donated (e.g., NaOH = 1, Ba(OH)₂ = 2)

Results

Analyte Molarity

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Moles of Analyte

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Moles of Titrant

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Equivalence Ratio

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Frequently Asked Questions

How do I calculate titrations?

Use the neutralization equation: nH⁺ × Ma × Va = nOH⁻ × Mb × Vb. Where n is the number of ions donated, M is molarity, and V is volume. Rearrange to solve for the unknown value.

What is a titration?

Titration is an analytical technique used to determine the concentration of an unknown solution by reacting it with a solution of known concentration until neutralization is reached, indicated by a color change.

What is the equivalence point in titration?

The equivalence point is when the moles of acid equal the moles of base in the reaction, meaning complete neutralization has occurred. This is where the indicator changes color.

How many H⁺ or OH⁻ ions should I enter?

Enter the number of hydrogen or hydroxide ions each molecule can donate. For example: HCl = 1, H₂SO₄ = 2, NaOH = 1, Ba(OH)₂ = 2.

What units should I use for volume and concentration?

Use milliliters (mL) for volume and molarity (M) for concentration. The calculator will handle the unit conversions automatically in the calculations.

Can I calculate titrant molarity instead of analyte molarity?

Currently this calculator solves for analyte molarity when it's unknown. You can rearrange the neutralization equation manually to solve for titrant molarity if needed.

What is the difference between strong and weak acids in titrations?

Strong acids completely ionize in solution, while weak acids only partially ionize. This affects the pH curve shape but not the basic neutralization calculation at the equivalence point.