How i can make 100 ml electrolyte solution of 0.1 M aniline & 1 M H2SO4.
i have aniline monomer of molecular weight = 93.13 and density 1.02 and concentrated H2SO4 (of 98 % grade)
For every 100 ml of solution, 0.01 mol of aniline and 0.1 mol of sulfuric acid are needed. 0.01 mole aniline = 0.9313 g 0.1 mol of sulfuric acid = 9.8 g (100%)
Because the acid is 98% you need it (100/98) * 9.8 = 10 g. Therefore pour into the beaker about 50 ml of distilled water, add 10 g of 98% sulfuric acid, add 0.9313 g aniline and make up to 100 ml with distilled water.
Unless stated otherwise, the concentration indicated in the label, should be assumed as given in wt%, i.e. (g H2SO4 / g solution)·100%. Commercial conc. H2SO4 is typically 98 wt%. The density of 98.0 wt% H2SO4 (aq.) solution is 1.836 g/cm3 (20 ºC) (*) ― likely available from the label. The molecular mass of H2SO4 is 98.079 g/mol. The molarity is: 0.98(g H2SO4 / g aq. sol.)·1.836(g aq. sol. / cm3)·(1000 cm3/dm3)/(98.079 g H2SO4/mol H2SO4) = 18.35 M (approximate).The intended dilute solution (1 M) can be then volumetrically prepared, at approx. 20 ºC, while considering the appropriate (volumetric) dilution factor. For quantitative analytical purposes the prepared solution should be standardized to accurately determine its molarity (approx. 1 M).
(*) R.H. Perry, D.W. Green, J.O. Maloney (Eds.), "Perry's Chemical Engineers’ Handbook", 7th ed., McGraw-Hill, 1997; Table 2-101.
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