• A laboratory method for determining the concentration of an unknown acid/base using a neutralization reaction.

 

• A method of analysis that will allow you to determine the precise endpoint of a reaction and the precise quantity of reactant in the titration flask. A buret is the used instrument to make or bring the second reactant to the flask and an indicator acid is used to detect the endpoint of the reaction.

 

• a laboratory method of determining the unknown concentration of an analyte. It is also known as volumetric analysis. A titrant is prepared as a standard solution.

 

• A laboratory analysis that uses a known solution with definite concentration and is applied to a known volume of another solution of unknown concentration until it reaches neutralization.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

• Analyte- the substance that is being tested or analyzed.

• Titrant- a solution or reagent that reacts with the analyte

 

• Equivalence point- the point at which there are stoichiometrically equivalent amounts of acid and base. [H+] = [OH-]

• Indicators- are chosen, such that they change colors at the range of the pH of interest.

 

• The solution at the endpoint may be:

1. Basic – involves Strong base and weak acid 

2. Neutral- strong acid and strong base (HCl + NaOH)

3. Acidic- strong acid + weak base

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

• Requirements:

1. Reaction must be stoichiometric.

2. Reaction must be rapid.

3. Reaction must be quantitative.

4. There should be a marked change in some property of the solution when the reaction is complete.

 

 

 

 

 

 

 

 

 

References:

http://www.dartmouth.edu/~chemlab/techniques/titration.html

http://en.wikipedia.org/wiki/Titration

 

 

 

Written By: Sydney Santiago