Osmotic Pressure

Q. Two solutions of $KN{O}_3$ and $C{H}_{3}COOH$ are prepared separately having the same molar concentration.
The correct relationship between the osmotic pressures is

1. $P_2>P_1$
2. $P_1=P_2$
3. $P_1>P_2$
4. $\frac{P_1}{P_1+P_2}=\frac{P_2}{P_1+P_2}$

Q. What is the pH of the solution when 0.2 mole of hydrochloric acid is added to one litre of a solution containing 1 M acetic acid and acetate ion? Assume that the total volume is one litre. $K_a$ for ${\text{CH}}_3\text{COOH}=1.8\times {10}^{-5}$

1. 4.58
2. 7
3. 2.37
4. 9.16

Q. The slope of $\pi$ versus $\text{C}$ was made against insulin concentration $\text{c}$. in ${\text{gmL}}^{-1}$ and temperature $27{}^{\circ }\text{C}$. If $\text{C}$ is in ${\text{litre}}^{-1}$ and the slope of line obtained is $4.65\times {10}^{-3}\frac{g}{mL}$, which of the following are not the molar mass $\left({\text{in g mol}}^{-1}\right)$ of insulin?

1. $9\times {10}^5$
2. $3\times {10}^5$
3. $4.5\times {10}^5$
4. $5.30\times {10}^6$

Q.

Osmotic pressure is 0.0821 atm at a temperature of 300 K. Find concentration in mole/litre.

1. 0.033

2. 0.066

3. 

4. 3

Q.

A solution of sucrose (molar mass = 342 g/mol) is prepared by dissolving 68.4 g of it per litre of the solution. What is its osmotic pressure (R = 0.082 lit. atm.k^-1mol^-1) at 273 K?

Q.

Which of the following colligative properties can provide molar mass of proteins (or polymers or colloids) with greater precision

1. Relative lowering of vapour pressure
2. Elevation of boiling point
3. Depression in freezing point
4. Osmotic pressure

Q.

The average osmotic pressure of human blood is 7.8 bar at 37⁰C. What is the concentration of an aqueous NaCl solution that could be used in the blood stream

1. 0.16 mol/L

2. 0.32mol/L

3. 0.60mol/L

4. 0.45mol/L

Q. The osmotic pressure of the solution is given by the relation :
where,
$\pi \text{is osmotic pressure}$
$T\text{is temperature}$
$R\text{is ideal gas constant}$
$n\text{are number of moles}$
$V\text{is volume}$
All quantites are in their SI units

1. $\pi =\frac{V}{n\times R\times T}$
2. $\pi =\frac{n\times R\times T}{V}$
3. $\pi =\frac{n\times V}{R\times T}$
4. $\pi =\frac{V\times R\times T}{n}$

Q.

The vapour pressure of water at 23^°C is 19.8 mm. 0.1 mole of glucose is dissolved in 178.2 g of water. What is the vapour pressure (in mm) of the resultant.

1. 19
2. 19.602
3. 19.402
4. 19.202

Q. A solution of glucose ($C_6{H}_{12}{O}_6$) is isotonic with 4 g of urea $(H_{2}N-CO-N{H}_2)$ per litre of solution. The concentration of glucose is:

1. $4g/L$
2. $3g/L$
3. $12g/L$
4. $14g/L$

Q.

The ratio of the value of any colligative property for KCl solution to that of sugar solution is

1. 1.0

2. 2.0

3. 0.5

4. 2.5

Q.

Which of the following shows maximum osmotic pressure in solution?

1. AgNO₃

2. MgCl₂

3. (NH₄)₃PO₄

4. Na₂SO₄

Q. $x\%\left(w/v\right)$ aqueous solution of $HCHO$ and $y\%\left(w/v\right)$ aqueous solution of glucose are isotonic with each other. The ratio $x:y$ will be:

1. $1:3$
2. $1:6$
3. $1:1$
4. $1:4$

Q.

The osmotic pressure at 17°C of an aqueous solution containing 1.75 g sucrose per 150 ml solution is

1. 0.8 atm

2. 0.08 atm

3. 8.1 atm

4. 9.1 atm

Q. Which of these solutions has the maximum osmotic pressure at a given temperature $\text{T}$?

1. $100\text{mL}$ of $\text{1 M}$ urea solution
2. $300\text{mL}$ of $\text{1 M}$ glucose solution
3. A mixture of $100\text{mL}$ of $\text{1 M}$ urea solution and $300\text{mL}$ of $\text{1 M}$ glucose solution
4. All of these are isotonic

Q.

A solution is obtained by dissolving 0.2 moles of urea in a litre of water. Another solution is obtained by dissolving 0.4 moles of cane sugar. The lowering of vapour pressure of the first solution is

1. same as that of the second solution
2. half of that of second solution
3. double to that of second solution
4. Cannot be predicted

Q. The following solutions were prepared by dissolving 10g of glucose $\left(C_6{H}_{12}{O}_6\right)$ in 250ml of water $\left(P_1\right)$ 10g of urea $\left(C{H}_4{N}_{2}O\right)$ in 250ml of water $\left(P_2\right)$ and 10g of sucrose $\left(C_{12}{H}_{12}{O}_{11}\right)$ in 250ml of water $\left(P_3\right)$. The right option for the decreasing order of osmotic pressure of these solutions is:

(NEET-2021)

1. $P_2>P_3>P_1$
2. $P_1>P_2>P_3$
3. $P_2>P_1>P_3$
4. $P_3>P_1>P_2$

Q.

The osmotic pressure of which solution is maximum (consider that deci-molar solution of each is 90% dissociated)

1. Aluminium sulphate

2. Barium chloride

3. Sodium sulphate

4. A mixture of equal volumes of (b) and (c)

Q.

Which of the following colligative properties is best suited for finding the molar mass of a substance?

1. Relative lowering of V.P.

2. Depression of M.P.

3. Elevation of B.P.

4. Osmotic presure.

Q.

Osmotic pressure of 0.1 M solution of NaCl and Na₂SO₄ will be

1. Same

2. Osmotic pressure of NaCl solution will be more than Na₂SO₄ solution

3. Osmotic pressure of Na₂SO₄ solution will be more than NaCl

4. Osmotic pressure of Na₂SO₄ will be less than that of NaCl solution

Q. Which statement comparing solutions with pure solvent is not correct?

1. A solution containing a non-volatile solute has a lower freezing point than pure solvent
2. A solution containing a non-volatile solute has a lower vapour pressure than pure solvent
3. None of the above
4. A solution containing a non-volatile solute has a lower boiling point than pure solvent

Q. Two isotonic solutions must have ----

1. Same solute and solvent
2. Same solute but different solvent
3. Same solvent but different solute
4. Both Solute and solvent may be different.

Q. A solution of urea contains 8.6 gm/litre (mol. Wt. 60.0). It is isotonic with a 5% (W/W) solution of a non-volatile solute having density 1 g/cc. The molecular weight of the solute will be

1. 348.8
2. 34.88
3. 3488
4. 861.2

Q.

The osmotic pressure of which solution is maximum (consider that deci-molar solution of each is 90% dissociated)

1. Aluminium sulphate

2. Barium chloride

3. Sodium sulphate

4. A mixture of equal volumes of (b) and (c)

Q.

Which of the following plots doesnot represent the behaviour of an ideal binary liquid solution ?

1. Plot of P_A Versus X_A (molefraction of A in liquid phone) is linear

2. Plot of P_B Versus X_B is linear

3. Plot of P_total X_A Versus (Or X_B)X_A is linear

4. Plot of P_total Versus X_A is non- linear

Q.

The density of a 9.5% by mass solution of fructose $\left(C_6{H}_{12}{O}_6\right)$ is $1.036g/c{m}^3$ at 293k. Calculate the osmotic pressure of solution.

1. 13.16 atm
   

2. 16.13 atm
   

3. 11.36 atm
   

4. 13.61 atm

Q. A container is partitioned by a semipermeable membrane (SPM), open from the top as shown in the figure. Initially, the left partition has 1 mole of $NaCl$ (non-volatile) in 90 g of water while the right partition has 1 mole of glucose (non-volatile) in 72 g of water at room temperature. After a long time, when steady state is reached by the transfer of some liquid water from the one partition to the other, which of the following options is true?

1. 18 g water is transferred from $NaCl$ solution to glucose solution
2. 18 g water is transferred from glucose solution to $NaCl$ solution
3. 9 g water is transferred from $NaCl$ solution to glucose solution
4. 9 g water is transferred from glucose solution to $NaCl$ solution

Q.

If 3 gm of glucose (mol. wt. 180) is dissolved in 60 gm of water at 15⁰C. Then the osmotic pressure of this solution will be

1. 0.34 atm

2. 0.65 atm

3. 6.57 atm

4. 5.57 atm

Q. $0.1M$ aqueous solution of $MgC{l}_2$ is at 300K and 4.92 atm. What will be the percentage of ionization of the salt?

1. $59\%$
   
2. $69\%$
3. $79\%$
   
4. $49\%$

Q.

The density of a 9.5% by mass solution of fructose $\left(C_6{H}_{12}{O}_6\right)$ is $1.036g/c{m}^3$ at 293k. Calculate the osmotic pressure of solution.

1. 13.16 atm
   

2. 16.13 atm
   

3. 11.36 atm
   

4. 13.61 atm