Question

1. Determine the osmotic pressure of a solution that contains 0.020 g of a hydrocarbon solute (molar mass = 340 g/mol) dissolved in benzene to make a 350-mL solution. The temperature is 20.0°C.
A)3.1 torr
B)1.0 torr
C)2.9 torr
D)0.21 torr
E)1.4 torr
2. Which of the following solutions would have the highest osmotic pressure?
A)0.2 M C6H12O6, glucose
B)0.15 M MgBr2, magnesium bromide
C)0.2 M CH3OH, methanol
D)0.2 M C12H22O11, sucrose
E)0.15 M KBr, potassium bromide

Answer 1

1. PV=nRT
2. Osmotic pressure=molarity multiplied by the number of ionic element. Ex: NaCl has 2
\[Na ^{+}, Cl ^{-}\]
\[AlCl _{3} \] has 4 ions \[Al ^{3+},Cl ^{-},Cl ^{-}, Cl ^{-}\]

Answer 2

The equation is not working for me, but do you understand?

Answer 3

P is pressure in atm
V is volume in liters
n is the number of moles
R is a constant which is 0.082
Temperature is in Kelvin.

Answer 4

The formula for osmotic pressure is: \(\huge \sf\Pi=iMRT \)

\(\sf \Pi\) is Osmotic pressure
\(\sf i\) is the van't hoff constant
\(\sf M\) is molarity
\(\sf R\) is the gas constant
\(\sf T\) is the absolute temperature

Answer 5

Sorry, I meant to wrote osmotic pressure formula for this problem.
We do not need to know the temperature or r because they are the same.

Answer 6

For 2. you dont need it - clearly it's dependent on \(i\), but for 1. you do need to use the whole formula including the temperature.

Answer 7

Yes, I referred to 2 only since that is the one asking for osmotic pressure.

Answer 8

#1. is asking about osmotic pressure...

"1. Determine the osmotic pressure of a solution.."

Answer 9

>_>

Answer 10

Oh yea but still.
I said to use PV=nRT for problem 1 meaning temperature would be used.
I never mentioned temperature or gas constant for the problem 2 because I forgot to put it there.

Answer 11

thank you guys

Answer 12

No problem.