13.9: Freezing Point Depression And Boiling Point ~ Just News

Freezing point = 0 - 17.6 = -17.6 oC A solution that contains 55.0 g of ascorbic acid (Vitamin C) in 250 g of water freezes at - 2.34°C. Calculate the approximate molar mass (in units of g/mol) of the solute. Kf of water is 1.86°C/m.Which solution would have the lowest freezing point, 0.500 M NaCl or 0.500 M CaCl2? chemistry. calculate the freezing point of an aqueous solution of 15.5 grams of glucose dissolved in 150 grams of water . Chemistry. Solutions are made that contain 0.1 moles of each of the following compounds below in 100g of H20.Option B: ionic Mg Br2. Because the depression of freezing point is proportional to the number of moles of solute per kg of solvent, and given that 1 mol Mg Br2 dissociates into three moles of ions, the solution of Mg Br2 will have more moles of particles and exhibit the largest reduction in the freezing point.Depression in freezing point is a colligative property which depends upon the amount of the solute. Δ T f = i × k f × m. where T f is the change in freezing point, i is Vant Hoff factor, m is molality and k is freezing point constant. 1% glucose will have Vant Hoff factor 1, 1% sucrose will have Vant Hoff factor 1.When I do an internet search for the densest-by-mass aqueous solution, I get the answer almost instantly: Clerici's solution. But, for some reason, when I search for the solution (of a salt - I'm querying only solutions of salts here) that has the lowest freezing-point, I find nothing but examples of multiple-choice questions - ie, which solution from a given short list has the lowest freezing

3. Which aqueous solution would you expect to have the

Answer: (d)1%CaCl2. Explanation: Depression in freezing point is a colligative property which depend upon the amount of the solute. where, = change in freezing point. i= vant hoff factor = freezing point constant. m = molality (a) 1% glucose: For non electrolytes like glucose, vant hoff factor is 1.Which of the following aqueous solutions h... | Clutch Prep Problem: Which of the following aqueous solutions has the lowest freezing point?a. 0.18 m KClb. 0.15 m Na 2SO4c. 0.12 m Ca (NO3)2d. pure watere. 0.20 m C2H6O2 (ethylene glycol)Which of the following aqueous solutions has the lowest freezing point? A. 0.10 M CaCl2 B. 0.15 M NaCl C. 0.15 M CaCl2 D. 0.20 M Na Cl Answer: The magnitude of the freezing point depression is proportional to the concentration of particles in the solution. The solution with the lowest freezing point is the one with the highest concentration of particles.Which of the following aqueous solutions has the lowest freezing point? A) 0.1m Na2SO4 B) 0.1m glucose C) 0.1m NaCl D) 0.1m NaHSO4 E) 0.1m CH3COOH the answer is A but thought it was glucose??

Which of the following aqueous solutions has the lowest

Given the Kf of water is 1.86° C/m, which of the following aqueous solutions has the lowest freezing point? a) 0.18 m KCl. b) 0.15 m Na 2 SO 4. c) 0.12 m Ca(NO 3) 2. d) pure water. e) 0.20 m C 2 H 6 O 2 (ethylene glycol)Get the detailed answer: 12. Which of the following aqueous solutions would be expected to have the lowest freezing point? A) 0.400 m K2SO4 B) 0.400 m NaCl C) 0.400 m C6H12O6 (glucose) D) 0.040 m K2SOcolligative properties like depression in freezing point and elevation in boiling point directly depends over no. of particles of solute.but freezing point &boiling point are not colligative properties.so in this question lowest freezing point is of 0.1 M Al 2 (SO 4) 3 due to greater no. of particles & hence greater deppression in freezing point takes place.and in case of boiling point ,valueD)higher boiling point and a lower freezing point 3.Compared to a 2.0 M aqueous solution of NaCl at 1 atmosphere, a 3.0 M aqueous solution of NaCl at 1 atmosphere has a A)higher freezing point and a lower boiling point than water B)higher freezing point and a higher boiling point than water C)lower freezing point and a higher boiling point thanWhich aqueous solution (i.e., water is the solvent) has the lowest freezing point? (The Kf for water is 1.86 degC/m; the freezing point of pure water is 0degC)

(A) 0.2 m NaCl (B) 0.2 m CaCl2 (C) 0.2 m H2SO4 (D) 0.2 m NH3 (E) 0.2 m Al(NO3)3 Answer and Explanation:Freezing point of a natural solvent is dependent upon the amount of solute that gets dissolved in it. In order to decide which solution has the lowest freezing point, we wish to have a look at the molality as well as whether the solute is ionic or covalent. Since the molality is equivalent for all of the solution choices, we want to look at what sort of solutes are present. Choice A: NaCl is ionic since it has a metal and a nonmetal. NaCl dissociates into 2 ions: Na+ and Cl - Choice B: CaCl2 is ionic because it has a metal and a nonmetal. CaCl2 dissociates into 3 ions: one Ca 2+ and two Cl- ionsChoice C: H2SO4 is a sturdy acid, and dissociates into 3 ions: two H+ and one SO4 2-Choice D: NH3 is a covalent compound since it's composed of 2 nonmetals, and subsequently does not dissociate when it's in waterChoice E: Al(NO3)3 is an ionic compound and will dissociate into 4 ions when it dissolves in water: one Al3+ and three NO3 - ions. Thus, since Al(NO3)3 dissociates into the most ions, the solution with it will have lowest freezing point.

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