Osmotic Pressure

Q.

Calculate(a)molality (b)molarity and (c)mole fraction of KI if the density of 20% (mass/mass) aqueous KI is1.202 g mL^-1.

Q.

Calculate the mass of a non-volatile solute (molar mass 40 g mol⁻¹) which should be dissolved in 114 g octane to reduce its vapour pressure to 80%.

Q.

Define Isotonic, hypertonic and hypotonic solutions

Q.

What is an isotonic solution?

Q. Find out the solubility of $Ni(OH{)}_2$ in $0.1MNaOH$. Given that the ionic product of $Ni(OH{)}_2$ is $2\times {10}^{-15}$.

1. $2\times {10}^{-8}M$
2. $1\times {10}^{-13}M$
3. $1\times {10}^{8}M$
4. $2\times {10}^{-13}M$

Q.

QUESTION 2.22

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 bar at the same temperature, what would be its concentration?

Q. $25.3g$ of sodium carbonate, $N{a}_{2}C{O}_3$ is dissolved in enough water to make $250mL$ of solution. If Sodium carbonate dissociates completely, molar concentration of sodium ion, $N{a}^{+}$ and carbonate ions, $C{O}_3^{2-}$ are respectively $(\text{molar mass of}N{a}_{2}C{O}_3=106gmo{l}^{-1})$

1. $\text{0.477 M and 0.477 M}$
2. $\text{0.955 M and 0.910 M}$
3. $\text{1.910 M and 0.955 M}$
4. $\text{1.90 M and 0.910 M}$

Q.

Calculate the mass percentage of Aspirin (${\mathrm{C}}_9{\mathrm{H}}_8{\mathrm{O}}_4$) in Acetonitrile (${\mathrm{CH}}_3\mathrm{CN}$) when$6.5\mathrm{g}$ of ${\mathrm{C}}_9{\mathrm{H}}_8{\mathrm{O}}_4$ is dissolved in $450\mathrm{g}$of ${\mathrm{CH}}_3\mathrm{CN}$.

Q.

Insulin (C₂H₁₀O₅)_n is dissolved in a suitable solvent and the osmotic pressure (π) of solutions of various concentrations (g/cm³) C is measured at 20℃. The slope of a plot of π against C is found to be 4.65 × 10^-3. The molecular weight of insulin is

Q. A solution containing $10gd{m}^{-3}$ of urea (Molecular weight 60 g/mol) is isotonic with a $5\%\left(w/V\right)$ solution of a non - volatile solute at the same temperature. The molecular mass of this non volatile solute is :

1. $30gmo{l}^{-1}$
2. $50gmo{l}^{-1}$
3. $111.1gmo{l}^{-1}$
4. $300gmo{l}^{-1}$

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 bloodstream

1. 0.45mol/L

2. 0.60mol/L

3. 0.15 mol/L

4. 0.32mol/L

Q.

An aquase solution of 2% non volatile solute exerts a pressure of 1.004 bar at normal boiling point of solvent. What is the molecular mass of solute (vapour pressure of pure water is 1.013bar

Q.

Which of the following solutions has highest osmotic pressure?

1. 1 M sucrose

2. 1 M NaCl

3. 1 M urea

4. 1 M glucose

Q.

Raoult's law becomes a special case of Henry's law when

1. K_H > p₁⁰

2. K_H < p₁⁰

3. K_H = p₁⁰

4. ^{all of the above}

Q.

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.

Q.

QUESTION 2.41

Determine the osmotic pressure of a solution prepared by dissolving 25 mg of $K_{2}S{O}_4$ in 2L of water at ${25}^{\circ }C$, assuming that it is completely dissociated.

Q.

What is Sahils method?

Q. A decimolar solution of potassium ferrocyanide at $300K$ is $50\%$ dissociated. Calculate the osmotic pressure of the solution.
$R=0.082Latmmo{l}^{-1}{K}^{-1}$.

1. $\pi =14.18atm$
2. $\pi =7.38atm$
3. $\pi =1.45atm$
4. $\pi =21.91atm$

Q. At $10{}^{\circ }\text{C}$, the osmotic pressure of urea solution is $500\text{mm}$. The solution is diluted and the temperature is raised to $25{}^{\circ }\text{C}$, and the osmotic pressure is found to be $105.3\text{mm of Hg}$. Determine the extent of dilution.

1. 3 times
2. 10 times
3. 5 times
4. 2 times

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.

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

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

Q.

The osmotic pressure of a 5% (wt/vol) solution of cane sugar at 150⁰C is

1. 4 atm

2. 2.45 atm

3. 5.078 atm

4. 3.4 atm

Q.

The osmotic pressure of blood is $7.65\text{atm}$ at $310\text{K}$. An aqueous solution of Glucose that will be isotonic with blood is what wt/vol?

Q. 24. 200ml of an aqueous solution of a protein contains its 1.26g.The osmotic pressure of this solution at 300K is found to be 2.57×10-3bar. The molar mass of protein will be (R=0.083Lbar mol-1 K-1) 1. 31011 g mol-1 2. 61038 g mol-1 3. 51022 g mol-1 4. 122044 g mol-1

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. 3488
2. 861.2
3. 348.8
4. 34.88

Q. $0.004gNaOH$ is dissolved in $250mL$ of solution.
Then choose the correct statement:

1. $\text{Molarity}=4\times {10}^{-4}M$
2. $2\times \text{Normality}=\text{Molarity}$
3. $\text{Concentration of}NaOH\text{solution}is16\text{ppm (w/V)}$
4. Both (a) and (c)

Q. Calculate the boiling point of solutions when 2 g of $N{a}_{2}S{O}_4(M=142gmo{l}^{-1})$ is dissolved in 50 g of water, assuming $N{a}_{2}S{O}_4$ undergoes complete ionization. ( $K_b$ for water = 0.52 K kg $mo{l}^{-1}$ )

Q. The relationship between osmotic pressure at 273 K when 10 g glucose, 10 g urea and 10 g sucrose are dissolved in 250 mL of water to form separate solutions is:
[$P_1,P_2$ and $P_3$ are osmotic pressure of glucose, urea and sucrose solution respectivitely]

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

Q. In 0.1 m aqueous solution of urea, the mole fraction of urea is

Q.

Which one of the following statements is FALSE:

1. The correct order of osmotic pressure for 0.01 M aqueous solution of each compound is BaCl₂>KCL>CH₃COOH sucrose.
2. The osmotic pressure (π) of a solution is given by the equation π=MRT where M is the molarity of the solution.
3. Raoult's law states that the vapour pressure of a component over a solution is proportional to its mole fraction
4. Two sucrose solutions of same molality prepared in different solvents will have the same freezing point depression.