4.22M aqueous solution of zinc(II) sulfite
4.22mole/L aqueous solution of zinc(II) sulfite
1liter of solution contains 4.22moles of zinc(II) sulfite
1000ml of solution contains 4.22moles of zinc(II) sulfite
mass of solution = volume * density
                         Â
= 1000*1.01 = 1010g
mass of solute (zinc(II) sulfite) = no of moles* gram molar
mass
                                                Â
= 4.22*145.22 = 612.82g
mass of solvent
(water)Â Â Â Â Â Â Â Â Â =
1010-612.82 = 397.18g
no of moles of
H2OÂ Â Â Â Â Â Â Â Â Â Â Â Â
= 397.18/18 = 22.065moles
mole fraction of zinc(II) sulfite   = no of
moleszinc(II) sulfite/zinc(II) sulfite+ no of moles of H2O
                                               Â
= 4.22/4.22+22.065
                                                Â
= 4.22/26.285Â Â Â = 0.1605 >>>>
answer
