A sulfuric acid solution containing 645.6 g of H2SO4 per liter of solution has a density of 1.329 g/cm3.
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We have the density of the solution =1.329 g/cm^3
Consider 1000ml of the solution (1Liter)
Mass of H2SO4=645.6 g
Mass of solution =density*volume =1000*1.329 g/ml =1329 g
Mass of the water=1329-645.6=683.5
a)Mass(%)=gram of solute/gram of solution *100 =(645.6/1329) *100 =48.58%(ans)
Mole of water =weight/Molecular weight =683.5/18 =37.97 mole
Mole of H2SO4=weight/Molecular weight =645.6/98=6.587
Total mole =6.587+37.97 =44.56 mole
Mole fraction =6.587/44.56 =.15 (ans)
c)Molality =moles of the solute(H2SO4)/Mass of the solvent(kg) = 6.587/.6835 =9.64 molal
d)Molarity =moles of (H2SO4)/Volume of soln =6.587/1 =6.587
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