Question

5. Calculate the mole fraction of water a 1.8 M HNO; aqueous solution. The density of the solution is 1.027 g/mL. Also explain why this solution would have a lower vapor pressure than pure water. Hint assume you have 1.0 L of the nitric acid solution, to find the mol fraction of H.O. [8 pts.

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Answer 1

- assume 1.0L of HNO3 solution 1.8 notes of HNO3 1.8M HNO whereas dewrity of solution is 1.827 g/m2 or. 1027 kg/L mass of soluhm in Now molar mass of & moros mass of 1827 kg in 12. HNO is 63.01 9/mo ho in 18, 015re long Scanned with CamScanner

mass of 1.8 mae HNO3 in mass ( mu - m) on my man = mass = 1.84 63,0 = 113,4 18 g mass of yo = 1.027 kg - 113,418 g - 1027 g - 113, 418 g = 913,582 g motes of tho= 913,582 g - 50.7 ml 18. สุรน การ 108 +50.7 Tosal mores Now, = = 52.5 moles Now mole fraction of water in moles of tho 50.7 - = 52.5 Tosal mols си,0 when s oal it means pure water fra Px 1 when do= 0.97 Pro = px 0.97, less than po

Vapor pressure of this solution will be lower as HNO3 will not let the water vapor come out of this phase, had it been pure water no difficulties would have been there for water to come out as vapor.

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