Abnormal Colligative Properties

Q.

Calculate the concentration of nitric acid in moles per litre in a sample which has a density, 1.41 g mL^–1 and the mass per cent of nitric acid in it being 69%.

Q. Sulphur forms the chlorides S2Cl2 and SCl2. The equivalent mass of sulphur in SCL2 is

Q. 20. Sodium crystallizes in a face centred cubic lattice. The approximate no of unit cells in 5 g of sodium is (Atomic mass of sodium =23u)

Q. 42. 1 mole of A, 1.5 mole of B and 2 mole of C are taken in a vessel of volume one litre . At equilibrium concentration of C is 0.5 mole/L. Equilibrium constant for the reaction A(g)+B(g) gives C(g) is (1)0.66 (2)0.066 (3)66 (4)6.6

Q. 3 What will be the mass of a 0.5 m solution of sodium acetate in water containing 0.15 mole of sodium acetate?

Q. 4 moles of PCl5 dissociates at 760 k in 2 litre flask, at equilibrium. 0.8 mole of Cl2 was present in flask. The euilibrium cons†an t would be

Q. 0.59 g of the silver salt of an organic acid(molar mass 210) on ignition gave 0.36 g of silver. The basicity of the acid is :- a. 3 b. 2 c. 1 d. 4 e. 5

Q. for the equilibrium S02Cl2=SO2+Cl2 what is the temperature at which Kp(atm)/Kc(M)=3 1.0.027K 2.0.36K 3.36.54K 4.273K

Q. 20 A sample of protein was analysed for metal content and analysis revealed that it contained magnesium and titanium in equal masses, by mass.if these are the only metallic species present in the protein and contains 0.016% metal, the minimum possible molar mass of the protein is: [ Mg=24, Ti=48]

Q. The osmotic pressure of a solution of $NaClis0.10atm$ and that of a glucose solution is $0.20atm$. The osmotic pressure of a solution formed by mixing $1L$ of the sodium chloride solution with $2L$ of the glucose solution is $x\times {10}^{-3}atm.x$ is
(JEE MAIN 2020)

Q. 71 gram of chlorine combines with a metal giving 111 gram of its chloride. The chloride is isomorphous with MgCl_2.6H_2O.Atomic mass of the metal i

Q. 36.1L of an unknown gas weighs 1.25 g at N.T.P which of the following pertains the above data 1)CO2 2)NO2 3)N2 4)O2

Q. All the N-N bond lengths are same in azide ion and hydraulic acid.true or false

Q. Which of the following setups is correct to calculate the weight (in g) of KCIO3 produced fromthe reaction of 0.150 moles of Cl2? 3CI2+6KOH-5KCI+ KCIO3 + 3H20 (a) 0.150 moles Cl2 x1 mole KCIO 3/3 moles Cl2x 122.5 g/1 mole KCIO3 (b) 0.150 moles CI2 x1 mole KCIO 3/3 moles Cl2 x 1 mole KClO3/122.5 g (c) 0.150 moles Cl2 x 3 moles Cl2/1 mole KCIO 3 x 122.5 g/1 mole KCIO3 (d) 0.150 moles Cl2x3 moles Cl2/1 mole KCIO 3 x1 mole KclO3/122.5 g

Q. 39 Starting with 100 mm (Hg) pressure of SO2Cl2 in a closed container, the following equillibrium is set up at some temperature : SO2Cl2 (g) SO2 (g) + Cl2 (g). if mole fraction of SO2Cl2 at equillibrium is 1/3, Kp for the reaction is : (a) 25 mm (b) 50 mm (c) 100 mm (d) 150 mm

Q. Moles in 10L of h2O at STP?

Q. A salt is formed due to reaction between an Oxy acid containing chlorine and a base containing monovalent metal is atomic mass X. The number of oxygen atoms in 1 molecule of the acid is more than the corresponding ic acid.Calculate the molecular mass of the salt. (A)83.5 + x/4 (b) 99.5+x (c) 83.5 +x (d) 99.5=x/2

Q. 20. Calculate the concentration of HNO3 in moles per litre in a sample which has density 1.41g/mol and mass percentage of HNO3 in it is 69%.

Q. ntQues) 3.2 moles of HI(g) were heated in a sealed bulb at 444^°C till the equilibrium was reached. Its degree of dissociation was found to be 20%. Calculate the number of moles of hydorgen iodide, hydorgen and iodine present at the equilbrium point and determine the value of equilbrium constant for the reaction 2HI(g)→H2(g) + I2(g). Considering the volume of the container 1 L. n

Q.

The observed osmotic pressure of a solution of benzoic acid in benzene is less than its expected value because

1. Benzene is a non-polar solvent

2. Benzoic acid molecules are associated in benzene

3. Benzoic acid molecules are dissociated in benzene

4. Benzoic acid is an organic compound

Q. (3) 1.25x 10-62 2g of metal carbonate is completely neutralised by100 mL of 01 N.HCI. The equivalent mass of metal4) 2.510-carbonate is(2) 300(1) 100(3) 25063. How much calcium is present in 2.5 moles of(420072

Q. Which of the following solutions will exhibit the highest boiling point?

1. $0.01mKN{O}_3$
2. $0.015m$ Glucose
3. $0.015m$ Urea
4. $0.01mN{a}_{2}S{O}_4$

Q. 28. An inorganic salt gave the following percentage composition: Na = 29.11, S = 40.51 and O = 30.38 Calculate the empirical formula and molecular formula of the salt. Given that the molecular mass of the salt is 158g

Q. Two flask x& y have capacity 1L&2L respectively & each of them contains 1 mole of a gas. The temperature of the flask are so adjusted that average speed of molecules in x is twice as those in y. The pressure in flask x would be 1) same as that in y 2)half that in y 3)twice of that in y 4) 8 times of that y

Q.

The boiling point of 0.2 mol $k{g}^{-1}$solution of X in water is greater than equimolal solution of Y in water. Which one of the following statements is true in this case?

1. Molecular mass of X is less than the molecular mass of Y.

2. Y is undergoing dissociation in water while X undergoes no change.

3. X is undergoing dissociation in water.

4. Molecular mass of X is greater than the molecular mass of Y.

Q. $3.0\times {10}^{-3}kg$ of acetic acid is added to 500 mL of water. $23\%$ of acetic acid is dissociated. If Kf and density of water are $1.86Kkgmo{l}^{-1}$ and 0.997 g/mL respectively. The depression in freezing point of acetic acid is :

1. 0.227
2. 0.229
3. 0.231
4. 0.233

Q. Pure water freezes at 273 K and 1 bar. The addition of 34.5g of ethanol to 500g of water changes the freezing point of the solution. Use the freezing point depression constant of water as 2K kg $mo{l}^{-1}$. The figures shown below represent plots of vapour pressure (V.P.) versus temperature (T). [Molecular weight of ethanol is 46g $mo{l}^{-1}$]
Among the following, the option representing change in the freezing point is

1. 
2. 
3. 
4. 

Q.

Calculate the mole fraction of ethylene glycol (C₂H₆O₂) in a solution containing 20% of C₂H₆O₂ by mass.

Q. 31.acetone in the solution is.of sIf the mole fraction of acetone in ethyl alcohol is 0.3. Then the molality o

Q. The experimental values of colligative properties of many solutes in solution resembles calculated values of colligative properties.
However in some cases, the experimental values of colligative properties differ widely than those obtained by calculations. Such experimental values of colligative properties are known as abnormal values of colligative properties. The causes for abnormal values of colligative properties are:
(i) Dissociation of solute: It increases the colligative properties.
e.g.: Dissociation of $\text{KCl, NaCl}$ etc. in $H_{2}O$.
(ii) Association of solute: It decreases the colligative properties.
e.g.: Dimerisation of acetic acid in benzene.

If the degree of dissociation of an electrolyte $A_2{B}_3$ is 25% in a solvent, then:

1. Normal boiling point = Experimental boiling point
2. Normal freezing point > Experimental freezing point
3. Normal osmotic pressure $=\frac{1}{2}$ Experimental osmotic pressure
4. Normal molecular weight $=\frac{1}{4}$ Experimental molecular weight