l 2. Determine the mole fraction of zinc(II) sulfite in a 4.22 M aqueous solution of zinc(II)...

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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 Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â = 1000*1.01 = 1010g

mass of solute (zinc(II) sulfite) = no of moles* gram molar mass

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 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) sulfiteÂ Â Â = no of moleszinc(II) sulfite/zinc(II) sulfite+ no of moles of H2O

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â = 4.22/4.22+22.065

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â = 4.22/26.285Â Â Â = 0.1605 >>>> answer

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