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
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Place the following solutions in order of increasing osmotic pressure. I. 0.15 M C2H6O2 II. 0.15...
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 10.15 M C2H602 II. 0.15 M BaCl2 III. 0.15 M Nal
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!
Which of the following aqueous solutions would have the lowest vapor pressure? a) 0.15 m nacl b) 0.10 m mgcl2 c) 0.30 m ch3oh d) 0.10 m li3po4 explain to me why, please
please explain why
Which of the following aqueous solutions would have the highest osmotic pressure at 298 K? O 0.5 M (NH4)2SO4 O pure H20 O 1.5 M glucose (C6H1206) O 1M MgCl2 O 1M NaNO3
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
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)
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)?
Arrange the following three bases in order of increasing base strength. NH CH3OH ОСН; II I III a. (Weakest base) I < II < III (Strongest base) b. (Weakest base) I < III < II (Strongest base) c. (Weakest base) II < I < III (Strongest base) d. (Weakest base) II < III < I (Strongest base) e. (Weakest base) III < II <I (Strongest base) f. (Weakest base) III < I< II (Strongest base)