Gravimetric Analysis
Quantitative Determination of Gravimetric Analysis
Ophelia Low Gek Suan 1311907DBT/FT/1A/01 |
SYNOPSIS
By gravimetric analysis, we are able to determine the amount of sulphate in barium sulphate quantitatively. We can do so by slowly adding dilute barium sulphate to an unknown sulphate solution that has been heated and acidified with concentrated hydrochloric acid slightly. A white precipitate will be yield from filtering the solution. It will then be washed with distilled water to rid any impurities and be put into an oven to dry. Once the precipitate has been dried, it will be taken out to be weighed as barium sulphate. The percentage of sulphate can then be obtained by calculating it from the weight of barium sulphate measured.
OBJECTIVE
The aim of this experiment is to use the gravimetric analysis to determine the amount of sulphate in a solution.
THEORY
When aqueous barium chloride and the aqueous unknown sulphate solution are added together, a solid precipitate of barium sulphate will be formed. Only a few drops of concentrated hydrochloric acid is added to water to dilute it, ensuring a low concentration for a good precipitation. The solution will be heated below boiling point for a period of time and the beaker would be covered with a watch glass to ensure no sputtering would occur and at the same time, ensure that the most number of frequent effective collisions between particles can be reached and that the speed of reaction is at its optimum. A vacuum pump is used to speed up the process of filtration to obtain the precipitate. The crucible used to contain the precipitate is porcelain and unreactive, so that it will not react with the precipitate and affect the accuracy of the experiment. It is also resistant to high heat, making it convenient for drying using an oven, effectively ridding all water content, so that an accurate mass of the precipitate can be measured.
PROCEDURES
FORMATION
Ophelia Low Gek Suan 1311907DBT/FT/1A/01 |
SYNOPSIS
By gravimetric analysis, we are able to determine the amount of sulphate in barium sulphate quantitatively. We can do so by slowly adding dilute barium sulphate to an unknown sulphate solution that has been heated and acidified with concentrated hydrochloric acid slightly. A white precipitate will be yield from filtering the solution. It will then be washed with distilled water to rid any impurities and be put into an oven to dry. Once the precipitate has been dried, it will be taken out to be weighed as barium sulphate. The percentage of sulphate can then be obtained by calculating it from the weight of barium sulphate measured.
OBJECTIVE
The aim of this experiment is to use the gravimetric analysis to determine the amount of sulphate in a solution.
THEORY
When aqueous barium chloride and the aqueous unknown sulphate solution are added together, a solid precipitate of barium sulphate will be formed. Only a few drops of concentrated hydrochloric acid is added to water to dilute it, ensuring a low concentration for a good precipitation. The solution will be heated below boiling point for a period of time and the beaker would be covered with a watch glass to ensure no sputtering would occur and at the same time, ensure that the most number of frequent effective collisions between particles can be reached and that the speed of reaction is at its optimum. A vacuum pump is used to speed up the process of filtration to obtain the precipitate. The crucible used to contain the precipitate is porcelain and unreactive, so that it will not react with the precipitate and affect the accuracy of the experiment. It is also resistant to high heat, making it convenient for drying using an oven, effectively ridding all water content, so that an accurate mass of the precipitate can be measured.
PROCEDURES
FORMATION
References: http://chemistry.tutorvista.com/analytical-chemistry/gravimetric-analysis.html