Titration Calculator

Molarity, Volume, and Stoichiometry Tool

Calculate unknown concentrations or volumes in titration experiments. Enter any three values and solve for the fourth. Supports stoichiometry and unit selection.

Example Calculations

Click an example to load it into the calculator.

Acid-Base: Find Unknown Molarity

Acid-Base: Find Unknown Molarity

25.00 mL of 0.100 M HCl titrated with 0.200 M NaOH. Find the volume of NaOH needed.

Calculate For: Titrant Volume (V1)

C1: 0.200 C1 Unit: Molar (M)

V1: undefined V1 Unit:

C2: 0.100 C2 Unit: Molar (M)

V2: 25.00 V2 Unit: Milliliters (mL)

n1: 1

n2: 1

Redox: Stoichiometry 2:1

Redox: Stoichiometry 2:1

50.0 mL of 0.0500 M Fe2+ titrated with 0.0250 M Ce4+ (2:1 ratio). Find volume of Ce4+ needed.

Calculate For: Titrant Volume (V1)

C1: 0.0250 C1 Unit: Molar (M)

V1: undefined V1 Unit:

C2: 0.0500 C2 Unit: Molar (M)

V2: 50.0 V2 Unit: Milliliters (mL)

n1: 1

n2: 2

Normality: Find Analyte Normality

Normality: Find Analyte Normality

10.0 mL of 0.100 N H2SO4 titrated with 0.0500 N NaOH. Find normality of NaOH if 20.0 mL used.

Calculate For: Titrant Concentration (C1)

C1: C1 Unit: Normal (N)

V1: 20.0 V1 Unit: Milliliters (mL)

C2: 0.100 C2 Unit: Normal (N)

V2: 10.0 V2 Unit: Milliliters (mL)

n1: 2

n2: 1

Education: Find Unknown Volume

Education: Find Unknown Volume

What volume of 0.250 M NaOH is needed to titrate 30.0 mL of 0.150 M HCl?

Calculate For: Titrant Volume (V1)

C1: 0.250 C1 Unit: Molar (M)

V1: undefined V1 Unit:

C2: 0.150 C2 Unit: Molar (M)

V2: 30.0 V2 Unit: Milliliters (mL)

n1: 1

n2: 1

Other Titles
Understanding Titration: A Comprehensive Guide
Master titration calculations, stoichiometry, and endpoint analysis with this in-depth guide for students and professionals.

What is Titration?

  • Definition and Purpose
  • Types of Titration
  • Key Concepts
Titration is a laboratory technique used to determine the concentration of an unknown solution by reacting it with a solution of known concentration. It is widely used in chemistry, biology, and environmental science.
Types of Titration
Common types include acid-base, redox, complexometric, and precipitation titrations. Each type uses different indicators and calculations.
Key Concepts
Equivalence point, endpoint, and stoichiometry are fundamental to understanding titration calculations.

Titration in Practice:

  • Determining the concentration of acetic acid in vinegar
  • Measuring water hardness
  • Analyzing vitamin C content in juice

Step-by-Step Guide to Using the Titration Calculator

  • Choosing the Variable to Calculate
  • Entering Values and Units
  • Interpreting Results
The calculator allows you to solve for any one of the four main variables in the titration equation. Select which variable you want to calculate, then enter the other three values, units, and stoichiometry.
Selecting the Unknown
Use the 'Calculate For' dropdown to choose which variable to solve for: C1, V1, C2, or V2. The input fields will adjust accordingly.
Inputting Values and Units
Enter the known values and select the appropriate units for concentration and volume. Enter stoichiometric coefficients if the reaction is not 1:1.
Understanding the Output
The result section displays the calculated value, the formula used, and a step-by-step breakdown of the calculation.

Calculator Usage Examples:

  • Calculate V1: What volume of 0.200 M NaOH is needed to titrate 25.00 mL of 0.100 M HCl?
  • Calculate C2: What is the analyte concentration if 20.0 mL of 0.150 M titrant is used for 30.0 mL of analyte?

Real-World Applications of Titration

  • Laboratory Science
  • Medical and Pharmaceutical
  • Environmental Testing
Titration calculations are essential in many fields. In labs, they are used to prepare reagents and standards. In medicine, they ensure correct drug dosages. In environmental science, they help analyze pollutant concentrations.
Lab Applications
Standard solutions, titrations, and sample preparations all require accurate titration calculations.
Medical Uses
IV fluids, injectable drugs, and diagnostic reagents are all prepared using titration principles.
Environmental Science
Water and soil samples are often titrated to bring analyte concentrations within measurable ranges.

Application Examples:

  • Determining the strength of bleach
  • Measuring vitamin C in supplements
  • Testing acidity of rainwater

Common Misconceptions and Correct Methods

  • Unit Confusion
  • Stoichiometry Errors
  • Endpoint vs. Equivalence Point
Mistakes in titration calculations often arise from unit mismatches, incorrect stoichiometry, or confusing the endpoint with the equivalence point.
Unit Consistency
Always ensure that concentration and volume units match or are properly converted before calculation.
Stoichiometry Matters
Use the correct stoichiometric coefficients from the balanced equation. Not all titrations are 1:1.
Endpoint vs. Equivalence Point
The endpoint is when the indicator changes color; the equivalence point is when stoichiometric amounts have reacted. They should be as close as possible.

Misconception Examples:

  • Mixing mL and L without conversion
  • Using 1:1 formula for a 2:1 reaction
  • Stopping titration at the wrong color change

Mathematical Derivation and Examples

  • Deriving the Formula
  • Worked Examples
  • Tips for Accuracy
The titration formula is derived from the conservation of moles: the amount of titrant and analyte at equivalence are related by stoichiometry.
Derivation
(C1 × V1) / n1 = (C2 × V2) / n2, where C = concentration, V = volume, n = stoichiometric coefficient. Rearranging allows you to solve for any variable.
Worked Example
To titrate 25.00 mL of 0.100 M HCl with 0.200 M NaOH: V1 = (C2 × V2 × n1) / (C1 × n2) = (0.100 × 25.00 × 1) / (0.200 × 1) = 12.5 mL.
Tips for Accurate Calculations
Double-check units, use calibrated equipment, and record all values for reproducibility.

Derivation and Example Calculations:

  • V1 = (C2 × V2 × n1) / (C1 × n2)
  • C2 = (C1 × V1 × n2) / (V2 × n1)