Titration and Volumetric Analysis Terminology

Fundamental Titration Concepts

• Titration: A volumetric technique where a solution of known concentration is added to a solution of unknown concentration until the reaction is complete.
• Acidimetry: The analytical process of determining the concentration of an unknown acid by titrating it with a standard base solution.
• Alkalimetry: The analytical process of determining the concentration of an unknown base by titrating it with a standard acid solution.
• Redox Titration: A titration based on an oxidation-reduction reaction between the analyte and the titrant.

Concentration and Solution Types

• Molarity (M): The number of moles of solute dissolved per liter of solution.
• Normality (N): The number of gram equivalents of solute dissolved per liter of solution.
• Decimolar Solution (M/10): A solution containing 1/10th of a mole of solute per liter of solution.
• Decinormal Solution (N/10): A solution containing 1/10th of a gram equivalent of solute per liter of solution.
• Seminormal Solution (N/2): A solution containing half a gram equivalent of solute per liter of solution.
• g/L (Strength): The mass of solute in grams present in one liter of the solution.
• Normality Factor (f): The ratio of the actual weight of the substance taken to the calculated weight required for a specific normality.

Chemical Properties and Standards

• Acidity of a Base: The number of replaceable hydroxyl (OH^-) ions present in one molecule of a base.
• Basicity of an Acid: The number of replaceable hydrogen (H⁺) ions present in one molecule of an acid.
• Equivalent Weight: The mass of a substance which combines with or displaces 1.008 parts by mass of hydrogen, 8 parts of oxygen, or 35.5 parts of chlorine.
• Primary Standard Solution: A solution of exactly known concentration prepared by dissolving a known mass of a primary standard substance in a fixed volume of solvent.
• Secondary Standard Solution: A solution whose concentration changes over time and must be standardized against a primary standard before use.

Indicators and Measurement Accuracy

• Indicator: A chemical substance (usually a weak organic acid or base) that changes color at or near the end point to indicate the completion of a reaction.
• End Point: The point during titration at which the indicator undergoes a sharp change in color, signaling that the reaction is practically complete.
• Equivalence Point: The theoretical point in a titration where the quantity of titrant added is chemically equivalent to the quantity of analyte present.
• Titration Error: The difference between the volume of titrant required for the theoretical equivalence point and the volume used to reach the observed end point.