Chemistry Titration

Definition and Principle

• Titration is a laboratory technique used to determine the concentration of a known reactant (titrant) that reacts with a sample of unknown concentration (analyte).
• The principle of titration is based on the reaction between the titrant and analyte, which forms a product that can be measured quantitatively.

Types of Titration

• Acid-Base Titration: used to determine the concentration of an acid or base, often using a strong acid or base as the titrant.
• Redox Titration: used to determine the concentration of a reducing or oxidizing agent, often using a strong oxidizing or reducing agent as the titrant.
• Complexation Titration: used to determine the concentration of metal ions, often using a complexing agent as the titrant.

Titration Curve

• A graph that plots the volume of titrant added (x-axis) against the pH or some other property of the reaction (y-axis).
• The equivalence point (stoichiometric point) is the point at which the amount of titrant added is equal to the amount of analyte present.
• The endpoint is the point at which the indicator changes color, indicating the completion of the reaction.

Indicators

• Substances that change color or undergo a physical change in response to a specific pH range or reaction condition.
• Examples: phenolphthalein (acid-base), starch (iodine), and potassium chromate (redox).

Titration Calculations

• Molarity: moles of solute per liter of solution (M = moles/L).
• Normality: equivalents of solute per liter of solution (N = equivalents/L).
• Equivalence Point: the point at which the number of moles of titrant equals the number of moles of analyte.
• Percent Error: difference between the experimental and theoretical values, expressed as a percentage.

Titration Definition and Principle

• Titration is a laboratory technique used to determine the concentration of a known reactant (titrant) that reacts with a sample of unknown concentration (analyte).
• The principle of titration is based on the reaction between the titrant and analyte, which forms a product that can be measured quantitatively.

Types of Titration

• Acid-Base Titration: used to determine the concentration of an acid or base, often using a strong acid or base as the titrant.
• Redox Titration: used to determine the concentration of a reducing or oxidizing agent, often using a strong oxidizing or reducing agent as the titrant.
• Complexation Titration: used to determine the concentration of metal ions, often using a complexing agent as the titrant.

Titration Curve

• A graph that plots the volume of titrant added (x-axis) against the pH or some other property of the reaction (y-axis).
• The equivalence point is the point at which the amount of titrant added is equal to the amount of analyte present.
• The endpoint is the point at which the indicator changes color, indicating the completion of the reaction.

Indicators

• Substances that change color or undergo a physical change in response to a specific pH range or reaction condition.
• Examples: phenolphthalein (acid-base), starch (iodine), and potassium chromate (redox).

Titration Calculations

• Molarity: moles of solute per liter of solution (M = moles/L).
• Normality: equivalents of solute per liter of solution (N = equivalents/L).
• Equivalence Point: the point at which the number of moles of titrant equals the number of moles of analyte.
• Percent Error: difference between the experimental and theoretical values, expressed as a percentage.