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Questions and Answers
What is the main purpose of using an indicator in an acid-base titration?
Why is it important to repeat the acid-base titration experiment three times?
What happens when a strong acid reacts with a strong base?
Why is it necessary to standardize the NaOH solution by titrating it with HCl?
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Which type of glassware is NOT mentioned as necessary for an acid-base titration experiment?
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What does it mean when it is stated that 'Strong acids and strong bases dissociate completely in water'?
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What is the purpose of titration in chemistry?
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What is the primary purpose of using an indicator in a titration process?
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In titration, what is a primary standard solution known for?
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What defines the equivalence point in a titration?
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What distinguishes secondary standard solutions from primary standard solutions?
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Why is an indicator used in titration?
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Study Notes
Titration
- Titration is a technique used to determine the concentration of a solution by measuring the volume of another solution needed to completely react with it.
Principles of Titration
- Based on the complete chemical reaction between the analyte and the reagent (titrant) of known concentration.
- Analyte: a solution of unknown concentration but known volume in a conical flask.
- Titrant: a solution of known concentration in a burette.
Standard Solutions
- Primary standard solution: extremely pure, highly stable, and can be weighed easily.
- Secondary standard solution: less pure, less stable, and cannot be weighed easily.
Titration Process
- Equivalence point: the theoretical point where the amounts of two reactants are just equivalent.
- End point: the practical point at which the reaction is observed to be complete, usually detected with an indicator.
- Indicator: an auxiliary substance that helps detect the completion of the titration process at the end point.
Acid-Base Titration
- Involves a sample of unknown concentration of acid estimated with a known concentrated base or vice versa.
- Strong acids and strong bases dissociate completely in water.
- Example: determination of the normality of sodium hydroxide solution by a standard solution of hydrochloric acid.
Equipment and Materials
- Glassware: burette, stand, conical flask, funnel, beaker, pipette, graduated cylinder, dropper, and washing bottle.
- Materials: HCl solution (standard), NaOH solution (unknown normality), and phenol naphthalene indicator.
Procedure
- Transfer 5 ml of unknown NaOH solution to a conical flask.
- Add 2-3 drops of phenol naphthalene indicator.
- Fill the burette with HCl solution to the zero mark.
- Titrate NaOH against HCl until the color changes from colorless to pink.
- Repeat the experiment three times and record the results.
Calculations
- Calculate the average volume of HCl used.
- Calculate the unknown concentration of NaOH using the average volume of HCl used.
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Description
Learn about the technique of titration in chemistry where the concentration of a solution is determined by measuring the volume needed to react with another solution. Understand the principle of titration based on chemical reactions between the analyte and titrant of known concentration.