Editing Titration (section)

==Procedure==
[[File:Titration for Soil.JPG|thumb|Analysis of soil samples by titration.]]
A typical titration begins with a [[beaker (glassware)|beaker]] or [[Erlenmeyer flask]] containing a very precise amount of the analyte and a small amount of [[PH indicator|indicator]] (such as [[phenolphthalein]]) placed underneath a calibrated [[burette]] or [[Pipette|chemistry pipetting syringe]] containing the titrant.<ref>{{cite journal |doi=10.1016/j.aca.2006.04.048 |title=Digital image-based titrations |year=2006 |last1=Gaiao |first1=Edvaldo da Nobrega |last2=Martins |first2=Valdomiro Lacerda |last3=Lyra |first3=Wellington da Silva |last4=Almeida |first4=Luciano Farias de |last5=Silva |first5=Edvan Cirino da |last6=Araújo |first6=Mário César Ugulino |journal=Analytica Chimica Acta |volume=570 |issue=2 |pages=283–290 |pmid=17723410 }}</ref> Small volumes of the titrant are then added to the analyte and indicator until the indicator changes color in reaction to the titrant saturation threshold, representing arrival at the [[equivalence point|endpoint]] of the titration, meaning the amount of titrant balances the amount of analyte present, according to the reaction between the two. Depending on the endpoint desired, single drops or less than a single drop of the titrant can make the difference between a permanent and temporary change in the indicator. 

===Preparation techniques===
Typical titrations require titrant and analyte to be in a liquid (solution) form.  Though solids are usually dissolved into an aqueous solution, other solvents such as [[Acetic acid|glacial acetic acid]] or [[ethanol]] are used for special purposes (as in [[petrochemistry]], which specializes in petroleum.)<ref>
{{Cite book
  | last = Matar
  | first = S.
  |author2=L.F. Hatch
   | title = Chemistry of Petrochemical Processes
  | publisher = Gulf Professional Publishing
  | edition = 2
  | year = 2001
  | isbn = 0-88415-315-0
}}</ref>  Concentrated analytes are often diluted to improve accuracy.

Many non-acid–base titrations require a constant [[pH]] during the reaction.  Therefore, a [[buffer solution]] may be added to the titration chamber to maintain the pH.<ref>
{{Cite book
  | last = Verma
  | first = Dr. N.K. |author2=S.K. Khanna |author3=Dr B. Kapila
  | title = Comprehensive Chemistry XI
  | publisher = Laxmi Publications
  | location = New Delhi
  | pages = 642–645
  | isbn = 81-7008-596-9
}}</ref>

In instances where two reactants in a sample may react with the titrant and only one is the desired analyte, a separate [[Masking agent|masking solution]] may be added to the reaction chamber which eliminates the effect of the unwanted ion.<ref>
{{Cite book
  | last = Patnaik
  | first = P.
  | title = Dean's Analytical Chemistry Handbook
  | publisher = McGraw-Hill Prof Med/Tech
  | edition = 2
  | year = 2004
  | pages = 2.11–2.16
  | isbn = 0-07-141060-0
}}</ref>

Some reduction-oxidation ([[redox]]) reactions may require heating the sample solution and titrating while the solution is still hot to increase the [[reaction rate]]. For instance, the oxidation of some oxalate solutions requires heating to {{convert|60|C|F}} to maintain a reasonable rate of reaction.<ref>
{{Cite book
  | last = Walther
  | first = J.V.
  | title = Essentials of Geochemistry
  | publisher = Jones & Bartlett Learning
  | year = 2005
  | pages = 515–520
  | isbn = 0-7637-2642-7
}}</ref>