Advertisements
Advertisements
प्रश्न
Determine the osmotic pressure of a solution prepared by dissolving 25 mg of K2SO4 in 2 liter of water at 25°C, assuming that it is completely dissociated.
Determine the osmotic pressure of a solution prepared by dissolving 25 mg of K2SO4 in 2 liter of water at 25°C, assuming that it is completely dissociated. (mol. wt. of K2SO4 = 174 g mol−1)
Advertisements
उत्तर
Given: K2SO4 dissolved (w) = 25 mg = 0.025 g
Volume of solution (V) = 2 L
Temperature (T) = 25°C = (25 + 273) K = 298 K
R = 0.0821 L atm K−1 mol−1
When K2SO4 is dissolved in water, K+ and \[\ce{SO^{2-}4}\] ions are produced.
\[\ce{K2SO4 -> 2K+ + SO^{2-}4}\]
Total number of ions produced = 3
∴ i = 3
Molar mass of K2SO4 (M) = (2 × 39) + (1 × 32) + (4 × 16)
= 174 g mol−1
Applying the following relation,
π = `i n/V RT`
= `i xx w/M xx 1/V RT`
= `3 xx 0.025/174 xx 1/2 xx 0.0821 xx 298`
= 5.27 × 10−3 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)
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.
Define the following term:
isotonic solution
Define the following term:
Hypotonic solution
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.
The osmotic pressure of CaCl2 and urea solutions of the same concentration at the same temperature are respectively 0.605 atm and 0.245 atm, calculate van’t Hoff factor for CaCl2.
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?
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 ______.
A solution containing 10 g per dm3 of urea (molar mass 60 g mol−1) is isotonic with 5% solution of non-volatile solute, MB of solute is:
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 ______.
Isotonic solutions must have the same:
(i) solute
(ii) density
(iii) elevation in boiling point
(iv) depression in freezing point
Give an example of a material used for making semipermeable membrane for carrying out reverse osmosis.
How can you remove the hard calcium carbonate layer of the egg without damaging its semiprermiable membrane? Can this egg be inserted into a bottle with a narrow neck without distorting its shape? Explain the process involved.
Which one of the following is a colligative property?
Blood cells retain their normal shape in solution which are
The following solutions were prepared by dissolving 10 g of glucose (C6H12O6) in 250 ml of water (P1), 10 g of urea (CH4N2O) in 250 ml of water (P2) and 10 g of sucrose (C12H22O11) in 250 ml of water (P3). The right option for the decreasing order of osmotic pressure of these solutions is
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)
Name the four colligative properties that are oftently used for determination of molecular mass.
