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|Acids/Bases - Titration|
Titration is a laboratory method used to determine the unknown concentration of a reactant. This is a delicate procedure that requires patience and a good observation skills. Usually, an indicator is used in titration to determine the endpoint of the reaction. Once the endpoint volume is found, mathematics can be used to determine the concentration of the unknown. This procedure is commonly used in the field of analytical chemistry.
Indicators must be chosen carefully, or else they will not be helpful in a titration. They must be chosen on the basis of pH at the equivalence point of the two reagents.
Color in Acid
Color in Base
pH at color change
Explore the discoverer's biography, including general facts about his life and anecdotes regarding how he made this particular discovery. Also see other significant scientific discoveries built largely on this concept and other real-world applications in history that may not still be relevant.
Titration can be traced to the origins of volumetric analysis, which began in the late eighteenth century. Study of analytical chemistry began in France and the first burette was made by Francois Antoine Henri Descroizilles. The field began to spread to neighboring countries. The first book containing titration was titled Lehrbuch der chemisch-analytischen Titrirmethode (Instructional Book of Titration Methods in Analytical Chemistry) and was published in 1855 in Germany. The author of this book, Karl Freiderich Mohr, is also responsible for advancing the burette from a graduated cylinder- type instrument to a tool with a clamp at the bottom that is still used today.
Study the primary definition of this concept, broken into general, basic, and advanced English definitions. Also see the mathematical definition and any requisite background information, such as conditions or previous definitions.
The gradual addition of one solution to another until the chemical amount of one reactant being added matches stoichiometrically the amount of another reactant in the solution initially present.
An operation, used in volumetric analysis, in which a measured amount of one solution is added to a known quantity of another solution until the reaction between the two is complete. If the concentration of one solution is known, that of the other can be calculated.
Real World Application
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Titration is used in laboratory medicine to determine unknown concentrations of chemicals of interest in blood and urine. Pharmacists also use titration in the development of new pharmaceuticals.
Titration may also be used to determine the amount of a certain chemical in food. Often, titration is used to determine fat content, water content, and concentrations of vitamins. Titration is also used to tell if cheeses and wines have aged enough for distribution to supermarkets and shops.
Of course, the main use of titration is in the laboratory. However, titrations are not limited to the field of chemistry. Scientists of different disciplines use titrations for a variety of different reasons.
Learn important vocabulary for this concept, including words that might appear in assessments (tests, quizzes, homework, etc.) that indicate the use of this concept.
Browse relevant videos from the Journal of Chemical Education's (JCE) Chemistry Comes Alive! library and other video sources.
This video shows the procedure near and at the endpoint of a titration.
This quick animation allows the teacher to narrate about different points of the titration curve as a reaction runs.
This video shows an example of a rough titration, that would be perfect for introducint titration.
This video shows the titration of hydrochloric acid and sodium hydroxide. It is a great video for beginning a titration lesson.
NaOH + HCl → NaCl + H2O
During this animated titration, the narrator explains precisely what is occurring during the titration.
This video shows a complete titration, explaining the steps along the way. It is good to show to students before they attempt their first titration.
This video shows the colors expected when various indicators are placed in acidic solution and basic solution.
Experience computer simulators or animations that illustrate the concept discussed here. Many simulators or animations come with worksheets for use in class.
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Titration is widely used when the concentration of a reagent or certain chemical in a solution is unknown. Students should know how to determine the concentration of the unknown after a titration as well as the reactions involved. Indicators are often used to determine the endpoint of the reaction.
Explore sample problems from the JCE QBank and other sources.
A 25.0 mL aliquot of a 1.44M solution of ammonia (Kb = 1.8 x 10-5) is titrated with 1.50M HCl. Use the Indicator Table below to decide which of the indicators listed would most accurately signal the equivalence point for this titration.
Write the letter corresponding to your choice of indicator in the box.