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Questions and Answers
What is the primary purpose of titration in a laboratory?
What is the primary purpose of titration in a laboratory?
What type of titration is used to determine the concentration of a reducing or oxidizing agent?
What type of titration is used to determine the concentration of a reducing or oxidizing agent?
What is the term for the point at which the amount of titrant added is equal to the amount of analyte present?
What is the term for the point at which the amount of titrant added is equal to the amount of analyte present?
What is the function of an indicator in a titration experiment?
What is the function of an indicator in a titration experiment?
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What is the unit of molarity?
What is the unit of molarity?
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What is the term for the difference between the experimental and theoretical values, expressed as a percentage?
What is the term for the difference between the experimental and theoretical values, expressed as a percentage?
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What is the purpose of a titration curve?
What is the purpose of a titration curve?
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What type of titration is used to determine the concentration of metal ions?
What type of titration is used to determine the concentration of metal ions?
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Study Notes
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.
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Description
A laboratory technique used to determine the concentration of a known reactant that reacts with a sample of unknown concentration. Understand the principle and types of titration, including acid-base titration.
