Advertisements
Advertisements
प्रश्न
At 300 K, 36 g of glucose present in a litre of its solution has an osmotic pressure of 4.98 bar. If the osmotic pressure of the solution is 1.52 bars at the same temperature, what would be its concentration?
Advertisements
उत्तर
Given: Temperature (T) = 300 K
R = 0.083 bar L K−1 mol−1
π V = `w/(M') RT`
For the first case,
Osmotic pressure for the first case (π) = 4.98 bar
4.98 × 1 = `36/(M') xx R xx T` ...(i)
For the second case,
Osmotic pressure for the second case (π) = 1.52 bar
1.52 × 1 = `w/(M') xx R xx T` ...(ii)
Dividing eq. (i) by eq. (ii), we get,
`4.98/1.52 = 36/w`
or `w = (1.52 xx 36)/4.98`
= 10.99 g
∴ Moles of solute present in 1 L of solution = `10.99/180`
= 0.061
Hence, the molarity of the solution is 0.061 M.
संबंधित प्रश्न
What happens when the external pressure applied becomes more than the osmotic pressure of solution?
Blood cells are isotonic with 0.9% sodium chloride solution. What happens if we place blood cells in a solution containing
(i) 1.2% sodium chloride solution?
(ii) 0.4% sodium chloride solution?
A solution containing 15 g urea (molar mass = 60 g mol–1) per litre of solution in water has the same osmotic pressure (isotonic) as a solution of glucose (molar mass = 180 g mol–1) in water. Calculate the mass of glucose present in one litre of its solution.
Calculate the osmotic pressure in pascals exerted by a solution prepared by dissolving 1.0 g of polymer of molar mass 185,000 in 450 mL of water at 37°C.
Which of the following 0.1 M aqueous solutions will exert the highest osmotic pressure?
Calculate the mass of a compound (molar mass = 256 g mol−1) to be dissolved in 75 g of benzene to lower its freezing point by 0.48 K (Kf = 5.12 K kg mol−1).
Choose the most correct option.
A living cell contains a solution which is isotonic with 0.3 M sugar solution. What osmotic pressure develops when the cell is placed in 0.1 M KCl solution at body temperature?
Answer the following.
What are isotonic and hypertonic solutions?
Answer the following.
Explain reverse osmosis.
Answer the following.
How molar mass of a solute is determined by osmotic pressure measurement?
What are hypertonic solutions?
Which of the following is a colligative property?
Two solutions have different osmotic pressures. The solution of higher osmotic pressure is called ____________.
At constant temperature the osmotic pressure of a solution is ____________.
20 g of a substance were dissolved in 500 mL of water and the osmotic pressure of the solution was found to be 600 mm of mercury at 15°C. The molecular weight of the substance is ______.
The average osmotic pressure of human blood is 7.8 bar at 37°C. What is the concentration of an aqueous NaCl solution that could be used in the blood stream?
Osmotic pressure of a solution is 0.0821 atm at a temperature of 300 K. The concentration in moles/litre will be:
In isotonic solutions:
(i) Solute and solvent both are same.
(ii) Osmotic pressure is same.
(iii) Solute and solvent may or may not be same.
(iv) Solute is always same solvent may be different.
Give an example of a material used for making semipermeable membrane for carrying out reverse osmosis.
Discuss biological and industrial importance of osmosis.
The vapour pressure of water is 12.3 k pa at 300 k. Calculated the vapour pressure of molal solution in it.
Assertion (A) : Osmotic pressure is a colligative property.
Reason (R) : Osmotic pressure is proportional to the molality.
Arrange the following solutions in the order of increasing osmotic pressure (π) assuming complete ionization.
- 0.5M Li2 SO4
- 0.5M KCl
- 0.5M Al2 (SO4)3
- 0.1 M BaCl2
Calculate the osmotic pressure of 0.03 mole of non electrolyte solute dissolved in 0.1 dm3 of water at 300 K. [R = 0.082 dm3 atm mol-1 K-1]
The plot of osmotic pressure (π) vs concentration (mol L−1) for a solution gives a straight line with slope 25.73 L bar mol−1. The temperature at which the osmotic pressure measurement is done is ______.
(Use R = 0.083 L bar mol−1 K−1)
