Gravimetric determination of water in hydrated magnesium chloride

Aim: To calculate the value of n in MgCl2.nH2O scheme: Gravimetric summary is where the amount of a specific chemical substance in a flatnesserial is determined by converting it to a product which set up be isolated only and weighed. This is relevant to this experiment as the amount of water is an unusual value which is to be name by carrying expose the analysis. warmth to constant chew is when repeated estrus, chilling soce weighing is carried out until the plentifulness of the substance is constant. The outlet of moles of water in a substance can be found by metre the loss in mass on estrus. MgCl2.nH2O MgCl2.nH2O n can be calculated by study the mass of hydrated prevalent salt with the mass of anhydrous salt by heating to constant mass. Apparatus: The equipment required is: a porcelain melting galvanic pile and lid tripod pipe-clay triangle bunsen burner and heating mat desiccator tongs a balance hydrated barium chloride. manner: To get rid of any water the crucible was heated, hence allowed to cool in a desiccator and its mass was renowned (M1). 2-3g of atomic number 12 chloride was then added and the crucible reweighed (M2). The crucible and its contents were then reheated for 15 minutes, allowed to cool and again weighed (M3).

The crucible and its contents were then heated, allowed to cool and weighed again, (M4), to make sure the loss in mass was complete. This look was repeated until M4 and M5 were constant. Results: M1 = 39.59g M2 = 41.62g M3 = 40.64g M4 = 40.63g Average mass of crucible and anhydrous MgCl2 = 40.635 kettle of fish of anhydrous MgCl2 (M4 - M1) ! = 1.045g flake of moles of MgCl2 (GFM = 95.3g) = 1.045/95.3 = 0.012moles Mass of H2O removed M2 - M4 = 0.985g Number of moles of H2O (GFM... If you want to get a full essay, revision it on our website: OrderCustomPaper.com

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