When 2.0 grams of copper (II) nitrate is added to 1000 ml of pure water, by how much is the vapor pressure of water decreased, given that at 20°C the vapor pressure of pure water is 17.535 mm Hg?(a) 3.1 x 10^-4(b) 0.303(c) 0.0333(d) 0.0033This question was addressed to me in my homework.My doubt stems from Colligative Properties and Determination of Molar Mass in portion Solutions of Chemistry – Class 12

When 2.0 grams of copper (II) nitrate is added to 1000 ml of pure wate

1.	When 2.0 grams of copper (II) nitrate is added to 1000 ml of pure water, by how much is the vapor pressure of water decreased, given that at 20°C the vapor pressure of pure water is 17.535 mm Hg?(a) 3.1 x 10^-4(b) 0.303(c) 0.0333(d) 0.0033This question was addressed to me in my homework.My doubt stems from Colligative Properties and Determination of Molar Mass in portion Solutions of Chemistry – Class 12
Answer» The correct option is (d) 0.0033 Best explanation: Given, Mass of solute, msolute = 2.0 grams Volume of solvent, Vsolvent = 1000 ml P^0water = 17.535 mm Hg Molecular mass of Cu(NO3)2 = 188 g/MOLE We know that ΔP1/P^01 = X2, where X2 is the mole fraction of the solute. We are REQUIRED to find out the difference in VAPOR pressure i.e. ΔP1. Therefore, ΔPwater= P^0water x X2 Number of MOLES of copper (II) nitrate = 2.0/188 = 0.0106 Number of moles of water = 1000g/(18g/mole) = 55.56 mole (since density of water is 1g/ml) Mole fraction of solute, X2 = 0.0106/(0.0106 + 55.56) = 1.9 x 10^-4 ΔPwater = 17.535 x 1.9 x 10^-4 = 0.0033.

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