Advertisements
Advertisements
प्रश्न
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?
पर्याय
5.08 atm
2.54 atm
4.92 atm
2.46 atm
उत्तर
2.54 atm
Explanation:
π = i1M1RT − i2M2RT
= [(1 × 0.3 mol dm−3) − (2 × 0.1 mol dm−3)] × 0.08205 atm dm3 K−1 mol−1 × 310 K
= 2.54 atm
संबंधित प्रश्न
Determine the osmotic pressure of a solution prepared by dissolving 2.5 × 10−2 g of K2SO4 in 2L of water at 25°C, assuming that it is completely dissociated.
(R = 0.0821 L atm K−1 mol−1, Molar mass of K2SO4 = 174 g mol−1)
Which of the following is not a colligative property?
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?
Determine the amount of CaCl2 (i = 2.47) dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at 27°C.
Define osmotic pressure.
Calculate the mass of NaCl (molar mass = 58.5 g mol−1) to be dissolved in 37.2 g of water to lower the freezing point by 2°C, assuming that NaCl undergoes complete dissociation. (Kf for water = 1.86 K kg mol−1)
Define the following term:
isotonic solution
Define the following term:
hypertonic solution
Define the following term:
hypotonic solution
Choose the most correct option.
The osmotic pressure of blood is 7.65 atm at 310 K. An aqueous solution of glucose isotonic with blood has the percentage (by volume)________.
Answer the following in one or two sentences.
What is osmotic pressure?
Answer the following.
What are isotonic and hypertonic solutions?
Answer the following.
A solvent and its solution containing a nonvolatile solute are separated by a semipermeable membrane. Does the flow of solvent occur in both directions? Comment giving a reason.
Answer the following.
How molar mass of a solute is determined by osmotic pressure measurement?
An aqueous solution of a certain organic compound has a density of 1.063 g mL-1 , osmotic pressure of 12.16 atm at 25 °C and a freezing point of 1.03 °C. What is the molar mass of the compound?
Which of the following statements is applicable for 0.1 M urea solution and 0.1 M sucrose solution?
Explain the osmotic pressure of a solution with the help of a thistle tube.
Explain the phenomenon of osmosis.
At constant temperature the osmotic pressure of a solution 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:
The temperature at which 10% aqueous solution of (W/V) of glucose will show the osmotic pressure of 16.4 atoms is: (R = 0.082 L atom K−1 mol−1)
At a given temperature, osmotic pressure of a concentrated solution of a substance ______.
Which of the following statements is false?
Isotonic solutions must have the same:
(i) solute
(ii) density
(iii) elevation in boiling point
(iv) depression in freezing point
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.
Discuss biological and industrial importance of osmosis.
Which of the following colligative property can provide molar mass of proteins (or polymers or colloids) with greatest precision?
Which one of the following is a colligative property?
Blood cells retain their normal shape in solution which are
In Isotonic solution
The following solutions were prepared by dissolving 10 g of glucose \[\ce{(C6H12O6)}\] in 250 ml of water (P1), 10 g of urea \[\ce{(CH4N2O)}\] in 250 ml of water (P2) and 10 g of sucrose \[\ce{(C12H22O11}\]) in 250 ml of water (P3). The right option for the decreasing order of osmotic pressure of these solutions is ______
Derive an expression to calculate molar mass of non-volatile solute by osmotic pressure measurement.
Determine the osmotic pressure of a solution prepared by dissolving 2.32 × 10−2 g of K2SO4 in 2L of solution at 25°C assuming that K2SO4 is completely dissociated.
(R = 0.082 L atm K−1 mol, Molar mass K2SO4 = 174 g mol−1)
A solution containing 10 g glucose has osmotic pressure 3.84 atm. If 10 g more glucose is added to the same solution, what will be its osmotic pressure? (Temperature remains constant)
Define osmotic pressure (π).
Prove that: M2 = `(W_2RT)/(πV)`.
Define reverse osmosis.
Name the four colligative properties that are oftently used for determination of molecular mass.
How will you determine molar mass of solute from osmotic pressure?
Write the condition of reverse osmosis.
