Titration

Method of neutralising an acid or a base very accurately in a lab

• HCl+ NaOH - NaCl + H2O

• Reactions between Acids and Bases

  • Central Idea: Reactions between Acids and Bases

  Acids

  • Definition

    • Sour taste

    • pH less than 7

  • Examples

    • Hydrochloric acid (HCl)

    • Sulfuric acid (H2SO4)

  Bases

  • Definition

    • Bitter taste

    • pH greater than 7

  • Examples

    • Sodium hydroxide (NaOH)

    • Ammonia (NH3)

  Acid-Base Reactions

  • Neutralization Reaction

    • Acid + Base -> Salt + Water

  • Examples

    • HCl + NaOH -> NaCl + H2O

  • Importance

    • Used in various industries

    • Helps in maintaining pH balance

  Titration Experiment Outline

  • Central Idea:

    • Conducting a titration experiment to determine the concentration of an unknown solution.

  • Main Branches:

    1. Preparation:

       • Gather equipment (burette, pipette, flask).

       • Prepare standard solution of known concentration.

       • Rinse equipment with distilled water.

    2. Procedure:

       • Measure volume of unknown solution in flask.

       • Add indicator to the flask.

       • Titrate with standard solution until endpoint is reached.

    3. Calculations:

       • Determine volume of standard solution used.

       • Use stoichiometry to find moles of unknown substance.

       • Calculate concentration of unknown solution.

    4. Analysis:

       • Compare calculated concentration with expected value.

       • Analyze sources of error.

       • Draw conclusions from the experiment.

  • Sub-branches:

    • Gather Equipment:

      • Burette

      • Pipette

      • Flask

    • Prepare Standard Solution:

      • Dissolve known amount of solute in solvent.

      • Dilute to known volume.

    • Rinse Equipment:

      • Rinse with distilled water.

      • Rinse with solution being used.

    • Measure Volume:

      • Use pipette or burette to measure volume accurately.

    • Add Indicator:

      • Choose suitable indicator based on reaction.

      • Add a few drops to the solution.

    • Calculate Volume:

      • Note initial and final volume of standard solution used.

      • Calculate volume used in titration.

    • Determine Moles:

      • Use balanced chemical equation.

      • Calculate moles of unknown substance.

    • Analyze Sources of Error:

      • Parallax error in reading volume.

      • Incorrect concentration of standard solution.

      • Incomplete reaction at endpoint.

1) add 20 ml of NaOH and methyl orange to a conical flask

2) add HCl to the burette

3) slowly add the acid until a colour change is observed

4) repeat using the same measurements but without indicator

5) evaporate solution to prove it was water and salt