Titration Calculator

Calculate titrant concentration, analyte concentration, or volumes for titration experiments based on equivalence point data and stoichiometry.

Calculate Your Titration Calculator

:

The molar ratio between titrant and analyte (e.g., 1:1, 2:1, 1:2)

Titration Calculator

Calculate titrant concentration, analyte concentration, or volumes required for titration based on equivalence point data.

Selected Calculation:

Calculating titrant concentration from analyte concentration, volumes, and stoichiometry

Titration is a common laboratory method used to determine the concentration of an analyte (the substance being analyzed) in a solution. It involves the controlled addition of a solution of known concentration (the titrant) to a solution of unknown concentration (the analyte) until the reaction reaches its endpoint.

Types of Titrations

There are several types of titrations, classified based on the type of reaction involved:

  • Acid-Base Titration: Determines the concentration of an acid or base by neutralizing it with a base or acid of known concentration.
  • Redox Titration: Involves a redox reaction between the analyte and titrant.
  • Complexometric Titration: Measures metal ion concentration using a complexing agent like EDTA.
  • Precipitation Titration: Forms an insoluble precipitate when the titrant reacts with the analyte.

Titration Calculations

The concentration of the analyte can be calculated using the following formula:

n₁ × M₁ = n₂ × M₂

Where:

  • n₁ = Mole ratio of the analyte from the balanced equation
  • M₁ = Molarity of the analyte
  • n₂ = Mole ratio of the titrant from the balanced equation
  • M₂ = Molarity of the titrant

For simple 1:1 reactions where n₁ = n₂, the formula simplifies to:

M₁V₁ = M₂V₂

Titration Curve

A titration curve is a graph of the pH of the solution being analyzed as a function of the volume of titrant added. The curve provides information about:

  • The equivalence point: where the amount of titrant added is exactly enough to react with all of the analyte
  • The pH at the equivalence point
  • The buffering regions of the solution
  • The strength of the acid or base being analyzed

Indicators

Indicators are substances that change color at or near the equivalence point of a titration. The choice of indicator depends on the pH range of the equivalence point:

  • Phenolphthalein: colorless in acid, pink in base (pH range 8.2-10.0)
  • Methyl orange: red in acid, yellow in base (pH range 3.1-4.4)
  • Bromothymol blue: yellow in acid, blue in base (pH range 6.0-7.6)

Alternatively, a pH meter can be used for more precise determination of the equivalence point, especially in titrations where the pH change at the equivalence point is small.

See Also

Related Calculators

Molarity Calculator

Calculate solution concentration in moles per liter.

pH Calculator

Calculate pH values and solution acidity/alkalinity.

Stoichiometry Calculator

Calculate reactant and product quantities in chemical reactions.

Gas Laws Calculator

Calculate pressure, volume, temperature, and amount of gas.

Frequently Asked Questions

Titration is used to determine the concentration of an unknown solution by measuring the amount of a standard solution needed to react completely with it. Common applications include determining the acidity of foods and beverages, analyzing water hardness, testing blood glucose levels, and quality control in pharmaceutical manufacturing.

To calculate concentration from titration data, use the formula: C₁ = (C₂ × V₂ × n₁) / (V₁ × n₂), where C₁ is the unknown concentration, C₂ is the known concentration of the titrant, V₁ and V₂ are the volumes of the analyte and titrant respectively, and n₁ and n₂ are the stoichiometric coefficients from the balanced equation.

The equivalence point is the point in a titration where the amount of titrant added is exactly sufficient to completely react with the analyte. At this point, the moles of titrant equal the moles of analyte multiplied by their stoichiometric ratio from the balanced chemical equation.

The equivalence point is the theoretical point where the reaction is complete according to stoichiometry. The endpoint is the experimentally observable point, typically detected by a color change of an indicator or a sharp change in a measured property (like pH). Ideally, they should be very close, but there is often a small difference called the titration error.

The right indicator should change color at or very near the equivalence point of the titration. For acid-base titrations, the pH at the equivalence point determines the appropriate indicator. For example, phenolphthalein (pH range 8.2-10.0) is suitable for strong acid-weak base titrations, while methyl orange (pH range 3.1-4.4) works well for weak acid-strong base titrations.

Share This Calculator

Found this calculator helpful? Share it with your friends and colleagues!