What is titration?
Titration is a method used commonly in chemistry laboratories and classrooms, which uses a solution of a known concentration to analyze and determine the unknown concentration of a second solution. Many times, the solution whose properties are known is a base, meaning it has a pH value of more than seven, while the unknown solution is an acid, meaning its pH is below seven. A typical titration involves the gradual addition of the base to the acidic solution, until a neutral pH of 7 is reached, or until a pH indicator turns a certain color, indicating that a certain other known pH has been reached. Titration can only be done with aqueous solutions of compounds. A textbook setup for an acid-base titration involves the solution of known concentration, called the titrant, suspended in a buret above a flask containing the unknown solution, or titrand. The buret is a calibrated vertical tube with a stopcock at the bottom of it, to regulate the flow of the titrant into the flask. The stopcock
Titration is the progressive addition of one reagent to another. In acid-base chemistry, the reagents are aqueous solutions, one of which is either a strong acid or a strong base. A typical titration involves progressively adding a solution of known concentration (the titrant) from a buret to a solution of unknown concentration (the sample) situated in a container below the buret. The amount of titrant added is just enough to completely neutralize the sample. An indicator is usually added to the sample to detect the equivalence point – or the point at which chemically equivalent amounts of titrant and sample have reacted. The chosen indicator should change colour at the pH which corresponds to the equivalence point, usually somewhere between pH 5 and 9. During a titration, the point at which the indicator changes colour is called the indicator endpoint. Typically, the goal of a titration procedure is to acquire information that allows you to calculate the molar concentration of a solut
Using the neutralization reaction, you can determine the concentration of an acid or a base solution. As shown in the previous equation, one hydrogen ion from an acid reacts with exactly one hydroxide ion from a base to produce a water molecule. If adding 100 hydroxide ions to an acid solution makes it a neutral solution (only water and salt), there must be 100 hydrogen ions in the original acid solution and you can calculate the concentration of the acid solution. To titrate an unknown acid/base solution, take a certain amount of the unknown solution and add a standard reagent of the known concentration carefully until the neutralization reaction is completed. This point where the number (or mole) of hydrogen ions and hydroxide ions are equal is defined as the equivalence point. To determine the equivalence point, scientists use an indicator or a pH meter. With the data of volume of the standard reagent used, the concentration of the unknown solution can be calculated. This whole proc
