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 HF
QUESTION 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
Question-3 :
since NaCl is soluble as well as ionic in nature so it fully dissociate to give Na+ and Cl- ion so concentration gets high also osmotic pressure .
while HF is weak acid so it will less dissociate so it's osmotic pressure is less than NaCl.
while glycol is non dissociating so it's osmotic pressure is too low .
so order is
I < III < II
Question : 4
among all of them all are non volatile non dissociating compounds so it's concentration matters only which gets high has high pressure as
π = cRT where π c
so , order is
I > II > III
Place the following solutions in order of increasing osmotic pressure.
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
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
Calculate the osmotic pressure at 298 K of the solutions that contain: 10.5 g of MgCl_2 in 150 mL of solution. 0.650 M NaCI solution. 7.5 % glucose (non-electrolyte) by mass in water. Density of solution is 1.01 g mL^-1
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)?
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 four liquids and/or solutions. pure water a 0.3 m solution of glucose in water a 0.2 m solution of lithium bromide in water a 0.1 m solution of magnesium bromide in water Place the liquids and/or solutions in order of (a) lowest freezing point to highest freezing point (b) lowest boiling point to highest boiling point (c) lowest osmotic pressure to highest osmotic pressure
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!
Number 1a,1b,1c,1d 1. Given the following three aqueous solutions at 25°C and 1 atm I. 0.100 m NaNO3 II. 0.100 w glucose (C6H1200) III. 0.100 m CaCl2 I II III (Please CIRCLE your choice) (2.5 points) a) Which solution has the highest osmotic pressure? I II III (Please CIRCLE your choice) (2.5 points) b) Which solution has the lowest boiling point? I II III (Please CIRCLE your choice) (2.5 points) c) Which solution has the highest freezing point? I II...
12.59 Place the following solutions in order of increasing [H3O+]. Please explain your reasoning. 0.10 M HF, 0.10 M NH3, 0.10 M HNO3 0.10 M HCN, 0.20 M HCN, 0.20 M HClO4 0.10 M NH3, 0.10 M NaOH, 0.10 M Ca(OH)2