Place the following solutions in order of increasing osmotic pressure.
I 10.15 M C2H602
II. 0.15 M BaCl2
III. 0.15 M Nal
Since BaCl2 and NaI are strong electrolytic compounds, hence in solution they are completely dissociate into ions. On the other hand, C2H6O2 is a covalent or non-electrolytic compound and doesn't produce ions.
Now, BaCl2 on dissociation produces three ions i.e. .
Hence, in 0.15 M BaCl2 solution, the concentration of ions = 3 * 0.15 M = 0.45 M.
Similarly, on dissociation NaI produces 2 ions i.e. .
Hence, in 0.15 M NaI solution, the concentration of ions = 2 * 0.15 M = 0.30 M.
Now, osmotic pressure is a colligative property and it is directly proportional to the the number of particles (ions or molecules) present in a solution. Since the increasing order of concentration of ions or molecules is Hence, the increasing order of osmotic pressure is or .
Place the following solutions in order of increasing osmotic pressure.
QUESTION 3 Place the following solutions in order of increasing osmotic pressure. (Hint: the solutes are l. molecule, II. a soluble ionic and III. a weak acid). I.0.15 M C2H6O2 II. 0.15 M NaCI III. 0.15 M HFQUESTION 4 Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing osmotic pressure. I. 0.011 M sucrose II. 0.0095 M glucose III. 0.0060 M glycerin
Place the following solutions in order of increasing osmotic pressure. Write a sentence or two explaining your reasoning (you can also mathematically show if you prefer). I. 0.15 M C2H6O2 II. 0.15 M BaCl2 III. 0.15 M NaI
Place the following solutions in order of increasing osmotic pressure. I. 0.15 M C2H6O2 II. 0.15 M MgCl2 III. 0.15 M CsCl II < III < I III < I < II I < II < III I < III < II II < I < III
1. Which of the following will be a consequence of ion-pairing in solution? a) higher vapor pressure b) higher boiling point c) lower melting point d) higher osmotic pressure e) none of above 2. Which of the following choices shows the correct arrangement of a given aqueous solutions in order of increasing osmotic pressure? Note "m" molality: I) 0.10m HCl II) 0.35 m HI III) 0.20 m MgCl2 IV) 0.15 m (H2N)2CO Thank you!
Consider the following set of quantum numbers and place them in order of increasing energy I. n = 4, l = 0, ml = 0, ms = -1/2 II. n = 4, l = 2, ml = -1, ms = -1/2 III. n = 5, l = 0, ml = 0, ms = +1/2 I < II < III III < II < I I < III < II II < III < I III < I < II
Determine the molarity of each of the following solutions from its osmotic pressure at 25°C. Include the van't Hoff factor for the solution when the factor is given. Part 1 II = 0.0211 atm for a solution of urea (CH4N2O): Part 2 II = 0.664 atm for a solution of KI, i=1.90:What molality of a nonvolatile, nonelectrolyte solute is needed to raise the boiling point of water by 7.35°C (K- 0.520°C/m)?
Place the following in order of increasing magnitude of lattice energy. MgO Nal Ba O
Place the solutions below in order of increasing freezing point, and explain the order: .15 m (molality) CH3OH (methanol), .10 m NaCl (sodium chloride), .18 m CH3CH2OH (ethanol), .080 m Na2SO4 (sodium sulfate)
Place the following substances in order of increasing vapor pressure. H2O N2 CO H2O < CO < N2 N2 < H2O < CO Na < CO < H2O CO < N2 < H2O CO < H2O < N2
Consider the six different solutions listed in the below. Solution Number Type of Solution: 0.90 m BaCl2, 1.20 m BaCl2, 0.30 m KCl, 0.90 m KCl, 0.30 m glucose, and 1.20 m NaNO3 (a) Arrange these six solutions in order of decreasing osmotic pressures if the temperature of all solutions is 25°C. (b) If the boiling-point elevations of these solutions were being analyzed in place of osmotic pressures, how would the order in part (a) change?