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1
Q

mass percentage of solute

A

mass of solute/mass of solution X 100

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2
Q

mass percentage of solute ( density)

A

mass of solute X 100/ volume of solution X density

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3
Q

mass fraction

A

mass of solute/mass of solution

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4
Q

mass percentage of solute ( mass fraction)

A

mass fraction X 100

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5
Q

percentage by vol

A

volume of solute X 100/ volume of sol

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6
Q

percentage mass by vol

A

mass of solute X 100/ volume of sol

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7
Q

strength of solution or conc of solution

A

mass of solute (in gram) /volume of solution in litre

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8
Q

parts per million

A

mass of solute X 10(power 6) / mass of soultion

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9
Q

mole fraction or fa

A

number of moles of a /total no of moles

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10
Q

no of moles of soluteor solvent

A

weight of solute or solvent/ molecular mass of solute / solvent

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11
Q

Fa + Fb + Fc=

A

1

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12
Q

molality (m)

A

no of moles of solute/ no of kg solvent

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13
Q

realation between mole fraction and molality

A

Xb X1000/ (1-Xb) molucle mass of a

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14
Q

molality (solubilty)

A

solubility X 10 / molecular mass of solute

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15
Q

solubilty

A

no of moles of solute/ no of moles of solvent

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16
Q

molarity ( M)

A

no of moles of solute/ no of litres of soultion

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17
Q

molarity ( density given)

A

(x) X d X 10 / molecular mass of solute

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18
Q

relation between molarity(M) and molality(m)

A

1/m = P/M - molecular mass of solute/ 1000

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19
Q

realtion between molarity and mole fraction

A

no of moles of solute X 1000 X density / mass of solution ( na ma + nb mb)

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20
Q

normality

A

Number of gram equivalents of solute/Number of litres of the solution

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21
Q

normality X eq mass

A

strenght of solution

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22
Q

relation of molarity and normality

A

(n=Molecular mass/ Equivalent mass)
n X molarity

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23
Q

absorption coeff

A

v/ V X P (v=volume of gas dissolved)(V= volume of solution) ( pressure in atm)

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24
Q

henrys law( solubility)

A

m= kp or s= kp

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25
henrys law
partial pressure of the gas = mole fraction X henrys const
26
which gas dont follow raoults law
ideal gas
27
raoults law
P= X partial pressure(a) + X partial pressure (b)
28
The process of separation liquid from 'a"nother liquid (binary mixture) having diffrent
boiling points
29
If a substance dissolves with absorption of heat, the, solubility _________ with rise of temperature
increase
30
if a substance dissolves with evolution of heat, the solubility __________ with rise of temperature.
decrease
31
Two solutions having same vapour pressure at same temperature are known as
isotropic solutions
32
relative lowering of vapour pressure
(Po is the vapour pressure of pure solvent) (d Ps is the vapour pressure' of the solution) Po- Ps/ Po
33
relation between lowering vp and raoults law
Po- Ps/ Po = n/n+N (n= moles of solute and N moles of solvent)
34
Variation of vapour pressure with temperature
log10 ( P2/ P1)= delta H vap X (1/T1 - 1/T2)/ 2.303 R
35
the temperature at which its vapour pressure is equal to the atmospheric pressure is called
boiling point
36
the boiling point of the solvent is elevated by the addition of _______ solute
non-volatile solute
37
Elevation of boiling point, (delta T)=
Boiling point of the solution - Boiling point of pure solvent
38
Elevation of boiling point, (delta T)=
K X no of moles of solute/ mass of solvent
39
the elevation in boiling point produed when 1 mole of the solute is dissolved in 100 g of the solvent is called
molecular elevation constant (K dash)
40
elevation in boiling point produced when 1 mole of the solute is dissolved in 1000 g of the solvent is called
molal elevation constant ( Kb)
41
relation between molal elevation const and molality
deltaT == Molality x K b
42
Raou!t's. laws of elevation of boiling point(definition )?
The elevation in boiling point of a solution of non-electrolYte is propo!tional to its molality and equimolal solutions of all the substances in the same solvent will show equal elevation in boiling points
43
Raou!t's. laws of elevation of boiling point (formula)
K b = R Tb^2/ 1000 Ly (Tb is the boiling point of the solvent on kelvin scale) and (Tb is the boiling point of the solvent on kelvin scale)
44
the temperature at which the vapour pressure of its liquid is equal to the vapour pressure of the corresponding solid is called
freezing point
45
the depression of freezing point produced when 1 mole of solute is dissolved in 1000 g of the solvent is called
K f molal depression constant
46
what solution is added to make a solution NOT FREEZE
ethylene glycol
47
what can be lowered to. the desired' extent by varying the concentration of ethylene glycoL
freezing point
48
Glycerol can also be used as anti-freeze.
its just facts (YOUR DOING GREAT :))
49
the solvent molecules from a solution of lower concentration move towards a solution of higher concentration IS called
osmosis
50
list two diff between Osmosis and Diffusion
In diffusion, solute as well as solvent molecules flow in opposite directions while in osmosis the flow of solvent molecules occurs in one direction only For osmosis, a semipermeable membrane* is required while for diffusion it is not required.
51
what is substance called if the solvent molecules to pass through it but prevents the passage of solute molecules through it
semi permeable membrane
52
semipermeable membranes name two substances
calcium phosphate and copper ferrocyanide, (ITS OKAY IF U DIDNT GET IT BUT MARK IT IMP)
53
Osmotic pressure equals
π = hdg (h = increase in level in the tube of unit cross section, d density of solution and g = acceleration due to gravity.)
54
osmotic pressure when two solutions of different concentration are separated by semipermeable membrane then
π= hdg := CRT (conc of solution= C)
55
A solution of high osmotic pressure is termed
hypertonic
56
A solution of low osmotic pressure is termed
hypotonic
57
when hypotonic solution is separated from hypertonic solution using semipermeable membrane, then osmosis takes place from hypotonic to hypertonic because solvent concentration is greater in hypotonic solution
plasmolysis
58
solutions having same osmotic pressures are termed
isotonic
59
define Boyle-van't Hoff law
The osmotic pressure (P or pi) of a solution is directly proportional to its concentration (C ) when the temperature is kept constant
60
when concentration and temperature both are changing, the osmotic pressure will be given by
PV=nST or πV=nST(S is called molar solution constant.) (no of moles of solute)
61
when is no flow of solvent molecules is observed on either side during osmosis
When two isotonic solutions are separated by a semipermeable membrane
62
DETERMINATION OF MOLECULAR MASSES by osmotic pressure
mb = Wb X S X T / PV
63
Let two solutions of same substance having different osmotic pressures 1t1 and 1t2 are mixed. Osmotic pressure of the resultant solution can be calculated as?
π1V1+ π2V2 = πr(VI + V2) [ πr= resultant osmoics pressure]
64
Let n l and n2 are the number of moles of two different solutes present in VI and V2 volumes respectively. Osmotic pressure of the mixture can be calculated as
π = (n1i1 +n2 i2 ) RT/( V1+V2) [ i1 and i 2 are van't Hoff factor for the two solutes.] ,
65
If external pressure greater than osmotic pressure is applied, the flow of solvent molecules· can be made' to proceed from solution towards pure solvent is called
reverse osmosis
66
Abnormal colligative property/ normal colligative property is called
van hoff factor i
67
van hoff factor=
Actual no. of particles in solution/ No. of particles taken
68
Total number of particles in solution=
1+ (n -l)alpha (alpha= degree of association )
69
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IIT JEE (19 decks)

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