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1
Q

The elevation in boiling pt. of a solution of molal concentration of solute will be maximum if the solvent is

A

Chloroform

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2
Q

Solutions of similar osmotic pressure are known as

A

Isotonic

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3
Q

Benzene- chloroform DO NOT show ______ deviation from Raoult’s Law

A

positive

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4
Q

on dissolving common salt in water , the boiling point of water

A

Increases

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5
Q

When blood cells are kept in high osmotic pressure solution than cellsap then

A

, they shrink as the water moves from the cell (low concentration) to the outside (high concentration) This shrinkage of cells is called ‘‘plasmolysis’’

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6
Q

According to Raoult’s law , relative lowering of vapour pressure of solution of non volatile solute is equal to

A

Mole fraction of solute

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7
Q

For osmotic Pressure (P) volume (V) and temp. (T) which of the following statement is false if T is constant :
i) P proportional to 1/ V
ii) P proportional to T
iii) P proportional to V
iv) PV is constant

A

iii) P proportional to V is FALSE

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8
Q

An Ideal Soln is that which:

A

Obey’s Raoult’s Law

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9
Q

Formula for determining Osmotic pressure

A

= nRT / V

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10
Q

Ratio of observed value of colligative property to that of theoritical value is known as

A

van’t Hoff factor

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11
Q

Gram molality of a soln is

A

no. of molecules of solute per 1000 gm solvent

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12
Q

Semi permeable membrane is chemically

A

Copper ferrocyanide

in semiperemable membrane similar molar conc

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13
Q

Which among the following is a colligative property :
Surface tension
viscosity
osmotic pressure
optical inversion

A

Osmotic pressure

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14
Q

Order of osmotic pressure of BaCl2 , NaCl and glucose soln of same molarity will b

A

BaCl2 > NaCl > GLucose

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15
Q

True/False
Sum of Xa and Xb of a binary soln is more than unit

A

False

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16
Q

True/False
Molarity of a soln changes with temp.

A

True

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17
Q

True/False
All solns obey Raoult’s law

A

False

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18
Q

Magnitude of molal elevation constant adn molal depression constant are comparable

A

False

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19
Q

Berkley Hartley method cannot be used for the determination of osmotic pressure of non aqueous soln

A

False

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20
Q

Osmotic pressure of 1 M soln at 0* C is 22.4 atmosphere

A

True

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21
Q

Molarity (M) =

A

Molarity (M) = moles of solute/liters of solution

mol dm3

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22
Q

Molality (m) =

A

Molality (m) = moles of solute / kilograms of solvent.

mol/kg

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23
Q

Normality

A

Normality = Number of gram equivalents × [Volume of solution in litres]

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24
Q

An example of Soln of gas in liquid

A

Soda water

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25
Q

An example of Soln of solid in gas

A

Smoke

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26
Q

An example of non ideal soln showing positive deviation

A

CH3COCH3 + C6H6

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27
Q

An example of non ideal soln showing negative deviation

A

CHCL3 + CH3COCH3

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28
Q

At high altitudes the boiling point of water decreases because at high altitude atmospheric pressure is

A

Less

29
Q

Through semi permeable membrane only _____ molecules can pass through

A

Solvent

30
Q

Molality of water is

A

55.6 m

31
Q

Liquid mixture which boil without any change in its composition is called

A

Azeotropic liquid mixture

32
Q

Give an example of Anti-freeze compound

A

Ethylene glycol

33
Q

Value of van’t hoff factor for a solute showing normal state in the soln will be ________ to one

A

Equal

34
Q

Write the unit of representing pollution

A

ppm

35
Q

What is Raoult’s law

A

At a definite temp. , for a soln of a non volatile solute the relative lowering in vapour pressure is equal to the mole fraction of solute

36
Q

Formula of Van’t Hoff factor

A

i = Observed value of colligative property / calculated value of colligative propeerty

37
Q

Define Molarity (M)

A

i) involves total volume of solution
ii) gram moles of solute are dissolved in 1 litre of soln
iii) it changes with temp. because volume changes with temp.

37
Q

Define Molality (m)

A

i) involves mass of solvent
ii) gram moles of solute are dissolved in 1 kg of solvent. Here volume of soln is not considered
iii) it is independent of temp. as it takes mass into consideration

38
Q

Define Solution

A

Solution is a homogenous mixture of 2 or more than 2 non reactive substances whose chemical composition can be varied within certain limits. Each soln contains two components solvent and solute

39
Q

State Henry’s Law

A

According to this law, “The mass of a gas dissolved per unit volume of a solvent at constant temp. is proportional to the pressure of gas with which the solvent is in equilibrium.
Let in unit volume of solvent, mass of gas dissolved is ‘m’ and equilibrium pressure be P, then m proportional to P or m = KP where K is a constant

40
Q

Define Mole fraction

A

Ratio of the moles of a component to the total no. of moles of all the components of soln is called mole fraction.
If moles of solute is n and that of solvent is N, then
Mole fraction of solute = n / (n + N)
Mole fraction of solvent = N / (n+N)

41
Q

Define Ideal Soln

A

They obey Raoult’s Law
There is no change in enthalpy that takes place during the formation of solution
∆H mix= 0
There is no change in volume during the formation of solution
∆V mix = 0

42
Q

Define non - Ideal Soln

A

Do not obey Raoult’s law
There is change in enthalpy that takes place during the formation of solution
∆H mix ≠ 0
There is change in volume during the formation of solution
∆V mix ≠ 0

43
Q

Define Formality

A

The number of grams of formula masses of solute dissolved per litre of solution is known as the formality of a solution.
Formality = mass of ionic solvent in gm per ltr /
Formula mass of the solute

44
Q

Define parts per million

A

ppm = mass of component A / total mass of soln x 10^6

ppm = volume of component A / total volume of soln x 10^6

45
Q

What is Raoult’s Law

A

Raoult’s law states that a solvent’s partial vapour pressure in a solution (or mixture) is equal or identical to the vapour pressure of the pure solvent multiplied by its mole fraction in the solution.

Mathematically, Raoult’s law equation is written as:
Psolution = Χsolvent x Po solvent
Where,
Psolution = vapour pressure of the solution
Χsolvent = mole fraction of the solvent
Po solvent = vapour pressure of the pure solvent

46
Q

Write about Positive deviation

A

Vapour pressure of soln and partial pressure of the components are more than those expected by the Raoult’s law.
∆H mix ≠ 0 and it is positive
∆V mix = positive
Forms minimum boiling azeotrope.

47
Q

Write about negative deviation

A

Vapour pressure of soln and partial pressure of the components are less than those expected by the Raoult’s law.
∆H mix ≠ 0 and it is negative
∆V mix = negative
Forms maximum boiling azeotrope.

48
Q

what is Semi permeable membrane

A

it is a membrane which allows the movement of a few solvent molecules through it. It appears to b continuous but it has very tiny holes or pores that are semi micro in nature. Through these only the molecules of solvent can pass while those of bigger size cannot pass through.

49
Q

A soln contains 20 mole solute and total no. of moles is 80 . Mole fraction of solute will be :

A

0.25

50
Q

Write the formula of molar conductance ʎm

A

k x v / M or k x 1000 / M

51
Q

Why is CaCl2 used for clearing off snow from roads ?

A

it causes depression in freezing point so snow melts into liquid state. Water flows easily and roads get cleared.

52
Q

HOW MANY ML OF 1 M H2SO4 IS REQUIRED TO NETURALIZE 10ML OF 1N NAOH

A

5 ML

53
Q

MOLARITY OF SOLU OF H2SO4 CONTAINING 9.8GM H2SO4 DISSOLVED IN 2 L WATER

A

0.05

54
Q

WHOSE BOILING POINT IS HIGHEST AT 1 ATM PRESSURE
1]0.1M GLUCOSE
2]0.1M BACL2
3]0.1 M NACL
4]0.1 UREA

A

2] 0.1 M BACL2

55
Q

EXPERIMENTAL MOLECULAR MASS OF AN ELECTROLUTE WILL ALWAYS BE LESS THAN ITS CALCUTED VALUE BEACAUSE VALUR OF VANT HOFF FACTOR I IS EQUAL TO

A

MORE THAN 1

56
Q

IN MOLAL SOLU 1 MOLE OF SOLUTE SUBSTANCE IS DISSOLVED IN

A

IN 1000GM SOLVENT

57
Q

IF BOILING POINT OF SOLUTION IS T1 AND BOILING POINT OF SOLVENT IS T2 THEN ELEVATION IN BOILING POINT WILL BE

A

T1-T2

58
Q

A SOLUTION CONTAINS 1 MOLE OF WATER AND 4 MOLES OF ETHANOL . THE MOLE FRACTION OF WATER ETHANOL IN SOLU WILL BE

A

0.2WATER+0.8ETHANOL

59
Q

COLLIGATIVE PROPERTIES OF SOLU DEPANDS ON

A

NO OF SOLUTE PARTICLES PRESENT IN SOLU

60
Q

OSMOTIC PROPERTIES FORMULA

A

⊓=NRT/V

61
Q

6 GM UREA [MOL WT 60] DISSOLVED IN 180 GM OF WATER . THE MOLE FRACTION OF UREA WILL BE

A

0.1/10.1

62
Q

NON IDEAL SOLU OF 95.4% OF H2O + C2H5OH REPRESENTS —- DEVIATION

A

+VE

63
Q

WRITE EXAMPLE OF MINI. BOILING POINT CONSTANT SOLU

A

96.4% C2H5OH + 5% H2O

64
Q

WHAT IS AZEOTROPIC MIXTURE ??

A

An azeotropic mixture is a mixture of substances that has the same concentration of vapour and fluid phases. A zeotropic mixture basically has constant or the same boiling points, and the mixture’s vapour will also have the same composition as the liquid.

65
Q

TYPES OF AZEOTROPIC MIXTURE

A
  1. Minimum Boiling Azeotropes or Negative Azeotrope
    Azeotropic mixtures with a higher boiling point in their constitutions are maximum boiling azeotropes. Water boils at 373 K, and hydrochloric acid boil at about 188 K, while azeotropes boil at around 383 K,
  2. Maximum Boiling Azeotropes or Positive Azeotrope
    Similarly, an azeotropic mixture that has a boiling point lesser than its constituents is known as a minimum boiling azeotrope. Consider, for example, ethanol consisting of a weight concentration of approximately ninety-five per cent and four per cent of water. Water boils at 373 K, and ethanol boils at about 351.5 K, while azeotropes boil at around 351.15 K
66
Q

ISOTONIC SOLUTION

A

An isotonic solution is any external solution that has the same solute concentration and water concentration compared to body fluids. In an isotonic solution, no net movement of water will take place.

67
Q
A

chemistry (9 decks)

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