ECAT Chemistry Online Test With Answers

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ECAT Chemistry Online Test

Sr. # Questions Answers Choice
1 The osmotic pressure of a dilute solution is directly proportional to the Diffusion rate of the solute Ionic concentration Elevation in boiling point Flow of solvent from a concentrated to a dilute solution
2 The vant Hoff factor (1) accounts for Degree of solubilisation of solute The extent of dissolution of solute The extent of dissolution of solute The degree of decomposition of solution
3 Equal volumes of ethylene glycol (molar mass = 62) and water (molar mass = 18) are mixed. The depression in freezing point of water is (given Krof water = 1.86 K mol-1kg and specific gravity of ethylene glycol is 1.11) 0.003 3.33 0.333 33.3
4 The weight of pure NaOH required to prepare 250 cm3of 0.1 N solution is 4 g 1 g 2 g 5 g
5 50 mL of 10 N H2SO4. 25mL of 12 N Hcl and 40 mL of 5N HNO3are mixed and the volume of the mixture is made 100 mL by adding water. The normality of resulting will be 1 N 2 N 3 N 9 N
6 0.5 M of H2SO4is diluted from 1 litre to 10 litre, normality of resulting solution is 1 N 0.1 N 10 N 11 N
7 The vapour pressure of two liquids 'p' and 'Q' are 80 and 60 torr respectively. The total vapour pressure of solution obtained by mixing 3 mole of P and 2 mol of Q would be 140 torr 20 torr 68 torr 72 torr
8 Ifα us the degree of dissociation of Na2SO4the vant Hoff's factor (1) used for calculating the molecular mass is 1 +<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: small;">α</span> 1 -<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: small;">α</span> 1 + 2<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: small;">α</span> 1 - 2<span style="color: rgb(34, 34, 34); font-family: arial, sans-serif; font-size: small;">α</span>
9 The weight of pure NaOH required to prepare 250 cm3of 0.1 N solution is 4 g 1 g 2 g 5 g
10 Camphor is often used in molecular mass determination because It is solvent for organic substances It is readily available It has a very high cryoscopic constant It is volatile
11 A solution contains 1.2046 x 1024hydrochloric acid molecules in one dm3of the solution. The strength of the solution is 6 N 2 N 4 N 8 N
12 Maximum freezing point falls in Camphor Naphthalene Benzene Water
13 Azeotropic mixture of HCl and water has 48% HCl 22.2% HCl 36% HCl 20.2% HCl
14 The ionic strength of a solution containing 0.1 mole/kg of KCl and 0.2 mole/kg of CuSO4is 0.3 0.6 0.9 0.2
15 Which of the statements given below concerning properties of solution, describe a colligative effect? Boiling point of pure water decreases by the addition of ethanol Vapour pressure of pure water decreases by the addition of nitric acid Vapour pressure of pure benzene decreases by the addition of naphthalene Boiling point of pure benzene increases by the addition of toluene
16 If liquids A and B form an ideal solution The enthalpy of mixing is zero The entropy of mixing is zero <div>The free energy of mixing is zero</div> The free energy as well as the entropy of mixing are each zero
17 At room temperature, the mole fraction of a solution in 0.25 and the vapour pressure of the solvent is 0.80 atm. Then the lowering of vapour pressure is 0.75 0.512 0.80 0.0512
18 When the solute is present in trace quantities the following expression is used Gram per million Milligram percent Microgram percent Parts per million
19 The solubility of a gas in water depends upon Nature of the gas Temperature Pressure of the gas All of the above
20 The depression of freezing point is directly proportional to Mole fraction of the solution Molarity of the solution Molality of the solution Molarity of the solvent
21 The temperature at which the vapour pressure of a liquid becomes equal to external pressure is Melting point Sublimation point Inversion point Boiling point
22 How much of NaOH is required to neutralize 1500 cm3of 0.1 N HCl? 60 g 6 g 4 g 40 g
23 Partial pressure of a solution component is directly proportional to its mole fraction. This statement is known as Henry's law Raoult's law Distribution law Ostwald's dilution law
24 Which substances are mixed to form a buffer solution? A strong acid and its salt of a strong base Strong acid and its salt of weak base Weak acid and its salt of strong base Weak acid and its salt of weak base
25 The osmotic pressure of 1 m solution at 27°C is 2.46 atm 24.6 atm 1.21 atm 12.1 atm
26 How many g of dibasic acid (mol. wt. 200) should be present in 100 ml of the aqueous solution to give 0.1 Normality? 1 g 2 g 10 g 20 g
27 Solutions with same osmotic pressures are called Hypertonic Hypotonic Isotonic Normal
28 The relative lowering of vapour pressure is equal to the mole fraction of the solute, This law is called Henry's law Raoult's law Ostwald's law Arrhenius law
29 Which one of the following is a colligative property? Surface tension Osmotic pressure Viscosity Refractive index
30 Which of the following will have the highest boiling point at 1 atm pressure? 0.1 M NaCl 0.1 M Sucrose 0.1 M BaCl<sub>2</sub> 0.1 M Glucose
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