NAME: NOSIBUSISEKO
ZULU
STUDENT NO: 2448387
MODULE: CHEM2032A
TITLE: DETERMINING
THE CONCETRATION OF
SULPHATE IN EPSOM
SALT.
, Objective
To determine the number of moles of water associated with one mole of magnesium sulphate,
MgSO4, in Epsom salt.
AIM
The aim of this experiment is to obtain the concentration of sulphate in the Epsom salt using
gravimetric method.
1. INTRODUCTION.
Epsom salts are hydrated magnesium sulphate, and their formula is sometimes written as
MgSO4.xH2O. When Epsom salts are heated, their water of crystallisation is driven off, leaving
anhydrous magnesium sulphate. Epsom salt was used because BaSO4 is not soluble in water. If the
amount of BaCl2 added to the sample is known, determining the mass of the barium sulphate
precipitate permits calculation of the amount of sulphate in the solution which can, them be related
to the concentration of MgSO4.7H2O (Epsom salt).
By weighing the hydrated and anhydrous magnesium sulphate before and after heating, it is possible
to find the mass of MgSO4 and the mass of H2O in a sample of Epsom salts. From these masses, the
number of moles of water associate with one mole of MgSO4 can be determined. This laboratory
experiment is carried out with a purpose of attaining how much concentration of sulphate does the
Epsom salt contain. The sulphate concentration of the Epsom salt was analysed gravimetrically by
converting the sulphate in the weighed Epsom salt to barium sulphate. The precipitate barium
sulphate is carefully filtered, washed with hot water, ignited at red heat, and weighed as barium
sulphate.
Ba2+(aq) + SO4(aq) BaSO4(s)……. (1)
This experiment was done using gravimetric analysis. It is of paramount importance to obtain the
concentration of sulphates. Gravimetric method is by the quantitative determination of the mass of
anhydrous Barium Sulphate precipitate. Barium sulphate precipitate is form when Barium Chloride is
added excessively to a hot given Sulphate solution slightly acidified with concentrated Hydrochloride
acid.
ZULU
STUDENT NO: 2448387
MODULE: CHEM2032A
TITLE: DETERMINING
THE CONCETRATION OF
SULPHATE IN EPSOM
SALT.
, Objective
To determine the number of moles of water associated with one mole of magnesium sulphate,
MgSO4, in Epsom salt.
AIM
The aim of this experiment is to obtain the concentration of sulphate in the Epsom salt using
gravimetric method.
1. INTRODUCTION.
Epsom salts are hydrated magnesium sulphate, and their formula is sometimes written as
MgSO4.xH2O. When Epsom salts are heated, their water of crystallisation is driven off, leaving
anhydrous magnesium sulphate. Epsom salt was used because BaSO4 is not soluble in water. If the
amount of BaCl2 added to the sample is known, determining the mass of the barium sulphate
precipitate permits calculation of the amount of sulphate in the solution which can, them be related
to the concentration of MgSO4.7H2O (Epsom salt).
By weighing the hydrated and anhydrous magnesium sulphate before and after heating, it is possible
to find the mass of MgSO4 and the mass of H2O in a sample of Epsom salts. From these masses, the
number of moles of water associate with one mole of MgSO4 can be determined. This laboratory
experiment is carried out with a purpose of attaining how much concentration of sulphate does the
Epsom salt contain. The sulphate concentration of the Epsom salt was analysed gravimetrically by
converting the sulphate in the weighed Epsom salt to barium sulphate. The precipitate barium
sulphate is carefully filtered, washed with hot water, ignited at red heat, and weighed as barium
sulphate.
Ba2+(aq) + SO4(aq) BaSO4(s)……. (1)
This experiment was done using gravimetric analysis. It is of paramount importance to obtain the
concentration of sulphates. Gravimetric method is by the quantitative determination of the mass of
anhydrous Barium Sulphate precipitate. Barium sulphate precipitate is form when Barium Chloride is
added excessively to a hot given Sulphate solution slightly acidified with concentrated Hydrochloride
acid.
