Titration-finding the concentration of a solution of sulphuric acid

Finding aside the accurate concentrain of sulphuric venereal infection Aim The point of this investigation is to dockage up out the absorption of the sulphuric acid in my experiment. I ordain do this by titrating the sulphuric acid with atomic number 11 change. H2SO4 + Na2CO3 à Na2SO4 + H2O + CO2 Acid + Alkali à brininess + Water + Carbon dioxide Ratio of sulphuric acid to atomic number 11 change: H2SO4 : Na2CO3 1 : 1 Concentration of sulphuric acid: H2SO4 is closely 0.05 - 0.15 moldm-3 The average concentration of the sulphuric acid is: 0.05 + 0.15 = 0.1 moldm-3 2 Concentration (moldm-3) = concentration (g dm-3) Molar clinch (g mol-1) Mr of Na2CO3 = (23 x 2) + ( 16 x 3) = 106 g mol-1 250cm3 x 0.1moldm-3 x 106 gmol-1 = 2.650g 1000cm3 I depart use 2.650g of Na2CO3 in 250cm3 of distilled water. Apparatus ·         Weighing store ·         Clamp stand ·          dulcify rod ·         250cm3 volumetric flask ·          fine cone-shaped flask ·         50cm3 burette ·         100cm3 beaker ·         25cm3 pipette ·         Pipette filler ·         Plastic pipette ·          diminished filter funnel ·         Balance ·         Distilled water ·         Sulphuric acid ·         2.

650g of sodium carbonate ·         Spatula ·         White tile ·         Methyl orange indicator Method ·         I will turn a solution where the solute will be the sodium carbonate and the solvent will be distilled water. ·         I will prototypic measure the pondering bottlefulful on its own without the lid on. ·         I will thusly make the weight of the bottle equal to 0.00g on the balance. ·         I will add 2.650g of sodium carbonate using a spatula. ·         I will then(prenominal) pour the sodium carbonate into a beaker, which has been washed out with distilled water to remove casteless compounds. ·         I will weigh the mass of the weighing bottle without... If you want to get a full essay, order it on our website: Ordercustompaper.com

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