Concentrated aqueous sulphuric acid is 98% H2SO4 by mass and has a density of 1.80 g.mL–1. Volume of acid required to make 1 litre of 0.1 M H2SO4 solution is
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Molarity = moles of substance
volume in liters
moles of H2SO4 = mass/ molar mass
denisty = 1.8g/ml(that is 1800g/L)
mass of H2SO4 98% of 1800= 1764g(this is mass of H2SO4 in 1L)
molar mass= 2+32+64 = 98
moles = mass/molar mass = 1764/98
= 18 moles
Therefore in !liter of H2SO4 molarity= moles/volume in liters= 18/1L
= 18M
Molarity =18M
volume in liters
moles of H2SO4 = mass/ molar mass
denisty = 1.8g/ml(that is 1800g/L)
mass of H2SO4 98% of 1800= 1764g(this is mass of H2SO4 in 1L)
molar mass= 2+32+64 = 98
moles = mass/molar mass = 1764/98
= 18 moles
Therefore in !liter of H2SO4 molarity= moles/volume in liters= 18/1L
= 18M
Molarity =18M
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