#The sample is dissolved, if it is not already in solution.
#The solution may be treated to adjust the pH (so that the proper precipitate is formed, or to suppress the formation of other precipitates).  If it is known that species are present which interfere (by also forming precipitates under the same conditions as the analyte), the sample might require treatment with a different reagent to remove these interferents.
#The precipitating reagent is added at a concentration that favors the formation of a "good" precipitate (see below).  This may require low concentration, extensive heating (often described as "digestion"), or careful control of the pH. Digestion can help reduce the amount of coprecipitation.
#After the precipitate has formed and been allowed to "digest", the solution is carefully filtered.  The filter is used to collect the precipitate; smaller particles are more difficult to filter.
#*Depending on the procedure followed, the filter might be a piece of ashless filter paper in a fluted funnel, or a filter crucible.  Filter paper is convenient because it does not typically require cleaning before use; however, filter paper can be chemically attacked by some solutions (such as concentrated acid or base), and may tear during the filtration of large volumes of solution.
#*The alternative is a crucible whose bottom is made of some porous material, such as sintered glass, porcelain or sometimes metal.  These are chemically inert and mechanically stable, even at elevated temperatures.  However, they must be carefully cleaned to minimize contamination or carryover(cross-contamination).  Crucibles are often used with a mat of glass or asbestos fibers to trap small particles.
#*After the solution has been filtered, it should be tested to make sure that the analyte has been completely precipitated.  This is easily done by adding a few drops of the precipitating reagent; if a precipitate is observed, the precipitation is incomplete.
#After filtration, the precipitate – including the filter paper or crucible – is heated, or charred.  This accomplishes the following:
#*The remaining moisture is removed (drying).
#*Secondly, the precipitate is converted to a more chemically stable form.  For instance, calcium ion might be precipitated using oxalate ion, to produce calcium oxalate (CaCO); it might then be heated to convert it into the oxide (CaO).  It is vital that the empirical formula of the weighed precipitate be known, and that the precipitate be pure; if two forms are present, the results will be inaccurate.
#*The precipitate cannot be weighed with the necessary accuracy in place on the filter paper; nor can the precipitate be completely removed from the filter paper to weigh it.  The precipitate can be carefully heated in a crucible until the filter paper has burned away; this leaves only the precipitate.  (As the name suggests, "ashless" paper is used so that the precipitate is not contaminated with ash.)
#After the precipitate is allowed to cool (preferably in a desiccator to keep it from absorbing moisture), it is weighed (in the crucible). To calculate the final mass of the analyte, the starting mass of the empty crucible is subtracted from the final mass of the crucible containing the sample. Since the composition of the precipitate is known, it is simple to calculate the mass of analyte in the original sample.