Question # 1

The sum of mole fractions (X) of components of solution is equal to

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100

200

One

Zero

If 5.85 g of NaCl are dissolved in 90 g of water, the mole fraction of NaCl is

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0.1

0.01

0.2

0.0196

10% aqueous solution of NaCI has molarity

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1.7 M

2.7 M

0.17 M

3.7 M

An azeotropic mixture of two liquids boils at a lower temperature than either of them when lower temperature

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It is saturated

it shows positive deviation from Raoult's law

It shows negative deviation form Raoult's law

It is metastable

How many g of dibasic acid (mol. wt. 200) should be present in 100 ml of the aqueous solution to give 0.1 Normality?

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1 g

2 g

10 g

20 g

The vant Hoff factor (1) accounts for

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Degree of solubilisation of solute

The extent of dissolution of solute

The degree of decomposition of solution

The percentage by weight of NaCl, if 6.0 g of NaCl is dissolved in 120 g of water is

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10.5 %

5%

8.02%

11.5%

Which one of the following is used as antifreeze in the radiator

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Methanol

Ethanol

Ethylene glycol

Glycerin

When the solute is present in trace quantities the following expression is used

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Gram per million

Milligram percent

Microgram percent

Parts per million

The amount of solute present in the given amount of solvent is called

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Molarity

Molality

Concentration

Solubility

If liquids A and B form an ideal solution

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The enthalpy of mixing is zero

The entropy of mixing is zero

The free energy of mixing is zero

The free energy as well as the entropy of mixing are each zero

Which if the following has the highest freezing point at one atmosphere

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0.1 M NaCI

0.1 M sugar solution

0.1 M BaCI₂

0.1 M FeCI₂solution

Maximum freezing point falls in

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Camphor

Naphthalene

Benzene

Water

At 25°C, the highest osmotic pressure is exhibited by 0.1 M solution of

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CaCl₂

KCl

Glucose

Urea

Every sample of matter with uniform properties and a fixed composition is called a :

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Solid

Liquid.

Phase.

Gas.

The relative lowering of vapour pressure is equal to the mole fraction of the solute, This law is called

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Henry's law

Raoult's law

Ostwald's law

Arrhenius law

The concentration units independent of temperature would be

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Normality

Mass-volume precent

Molality

Molarity

The freezing point of 1 molal NaCl solution assuming NaCl to be 100% dissociated in water in

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-1.86°C

-3.72°C

+1.86°C

+3.72°C

Saturated solution of a solid is prepared at a constant temperature. 100 cm³of this saturated solution is evaporated in a china dish. The mass of the residue is called

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Azetropic mixture

Solubility

Solubility product

Equilibrium constant

Which one of the following is an ideal solution that obeys Rault's law

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Ethanol + water

Benzene + toluene

HCI + water

Acetone + chloroform

Solutions with same osmotic pressures are called

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Hypertonic

Hypotonic

Isotonic

Normal

The osmotic pressure of solution increases if

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Temperature is decreased

Solution constant is increased

Number of solute molecules are increased

Volume is increased

Which one of the following solution will have higher vapour pressure than that of water

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Aqueous solution of methanol

Aqueous solution of HCI

Aqueous solution of glucose

Aqueous solution of urea

A solution consisting of 92 grams ethyl alcohol (C₂H₅OH) 96 grams methyl alcohol (CH₃OH) 90 grams water the mole fraction and mole percent of methyl alcohol is

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0.3. 30%

0.2, 30%

0.5, 30%

0.2, 20%

The molarity of solution containing 14.5 grams urea (N₂H₄CO) dissolved in 100 cm³of the solution is

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1 molar

0.1 molar

0.2 molar

0.25 molar

Saturated solution of NaCl on heating becomes

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Super saturated

Unsaturated

Remains saturated

None

The number of moles of solute in 1000g (1 Kg) of the solvent is called :

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Molarity

Normality

Mole fraction

1.0 g pure calcium carbonate was found to require 50 ml of dilute HCl for complete reaction. The strength of HCl solution is given by

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4 N

2 N

0.4 N

0.2 N

The molar boiling point constant is the ration of elevation in boiling point to :

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Molarity

Mole fraction of solvent

Mole fraction of solute.

Which is independent of temperature

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Molarity

Molality

Normality

Mole fraction

The number of moles of NH₄CI dissolved in 500 cm³of its 15%, W/N solution is

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1 mole

1.4 mole

2.0 mole

2.4 mole

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