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)
What happens when the external pressure applied becomes more than the osmotic pressure of 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.
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?
Define osmotic pressure.
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.
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.
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?
Explain the phenomenon of osmosis.
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:
Osmotic pressure of a solution increases if
Which of the following colligative property can provide molar mass of proteins (or polymers or colloids) with greatest precision?
Isotonic solutions have same
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
Assertion (A) : Osmotic pressure is a colligative property.
Reason (R) : Osmotic pressure is proportional to the molality.
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)
Isotonic solutions are the solutions having the same ______.
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
Name the four colligative properties that are oftently used for determination of molecular mass.
Write the condition of reverse osmosis.
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]
Calculate the osmotic pressure of 0.2 M aqueous solution of nonelectrolyte at 300 K.
[R = 0.082 atm dm3 mol−1K−1]
