Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

IIT JEE > solutions > Flashcards

solutions Flashcards

1
Q

mass percentage of solute

A

mass of solute/mass of solution X 100

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

mass percentage of solute ( density)

A

mass of solute X 100/ volume of solution X density

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

mass fraction

A

mass of solute/mass of solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

mass percentage of solute ( mass fraction)

A

mass fraction X 100

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

percentage by vol

A

volume of solute X 100/ volume of sol

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

percentage mass by vol

A

mass of solute X 100/ volume of sol

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

strength of solution or conc of solution

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

parts per million

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

mole fraction or fa

A

number of moles of a /total no of moles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

no of moles of soluteor solvent

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Fa + Fb + Fc=

A

1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

molality (m)

A

no of moles of solute/ no of kg solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

realation between mole fraction and molality

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

molality (solubilty)

A

solubility X 10 / molecular mass of solute

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

solubilty

A

no of moles of solute/ no of moles of solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

molarity ( M)

A

no of moles of solute/ no of litres of soultion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

molarity ( density given)

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

relation between molarity(M) and molality(m)

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

normality

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

normality X eq mass

A

strenght of solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

relation of molarity and normality

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

absorption coeff

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

henrys law( solubility)

A

m= kp or s= kp

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

henrys law

A

partial pressure of the gas = mole fraction X henrys const

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

which gas dont follow raoults law

A

ideal gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

raoults law

A

P= X partial pressure(a) + X partial pressure (b)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

The process of separation liquid from ‘a”nother liquid
(binary mixture) having diffrent

A

boiling points

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

If a
substance dissolves with absorption of heat, the, solubility
_________ with rise of temperature

A

increase

30
Q

if a
substance dissolves with evolution of heat, the solubility
__________ with rise of temperature.

A

decrease

31
Q

Two solutions having same vapour pressure at same temperature are known as

A

isotropic solutions

32
Q

relative lowering of vapour pressure

A

(Po is the vapour pressure of pure solvent)
(d Ps is the
vapour pressure’ of the solution)
Po- Ps/ Po

33
Q

relation between lowering vp and raoults law

A

Po- Ps/ Po = n/n+N (n= moles of solute and N moles of solvent)

34
Q

Variation of vapour pressure with temperature

A

log10 ( P2/ P1)= delta H vap X (1/T1 - 1/T2)/ 2.303 R

35
Q

the temperature at which its
vapour pressure is equal to the atmospheric pressure is called

A

boiling point

36
Q

the boiling point of the solvent is elevated by the addition of
_______ solute

A

non-volatile solute

37
Q

Elevation of boiling point,
(delta T)=

A

Boiling point of the solution - Boiling point of pure
solvent

38
Q

Elevation of boiling point,
(delta T)=

A

K X no of moles of solute/ mass of solvent

39
Q

the
elevation in boiling point produed when 1 mole of the solute
is dissolved in 100 g of the solvent is called

A

molecular elevation constant (K dash)

40
Q

elevation in boiling point produced when 1 mole of the solute
is dissolved in 1000 g of the solvent is called

A

molal elevation constant ( Kb)

41
Q

relation between molal elevation const and molality

A

deltaT == Molality x K b

42
Q

Raou!t’s.
laws of elevation of boiling point(definition )?

A

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
Q

Raou!t’s.
laws of elevation of boiling point (formula)

A

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
Q

the temperature at which the vapour pressure of its liquid is equal to the vapour pressure of the corresponding solid is called

A

freezing point

45
Q

the depression of freezing point produced
when 1 mole of solute is dissolved in 1000 g of the solvent is called

A

K f molal depression constant

46
Q

what solution is added to make a solution NOT FREEZE

A

ethylene glycol

47
Q

what can be lowered to. the desired’ extent by varying the concentration of ethylene glycoL

A

freezing point

48
Q

Glycerol can also
be used as anti-freeze.

A

its just facts (YOUR DOING GREAT :))

49
Q

the solvent molecules
from a solution of lower concentration move towards a solution
of higher concentration IS called

A

osmosis

50
Q

list two diff between Osmosis and Diffusion

A

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
Q

what is substance called if the solvent molecules to pass
through it but prevents the passage of solute molecules through it

A

semi permeable membrane

52
Q

semipermeable
membranes name two substances

A

calcium phosphate and copper ferrocyanide, (ITS OKAY IF U DIDNT GET IT BUT MARK IT IMP)

53
Q

Osmotic pressure equals

A

π = hdg (h = increase in level in the tube of unit cross section, d density of solution and g = acceleration due to gravity.)

54
Q

osmotic pressure when
two solutions of different concentration are separated by
semipermeable membrane then

A

π= hdg := CRT (conc of solution= C)

55
Q

A solution of high osmotic
pressure is termed

A

hypertonic

56
Q

A solution of low osmotic
pressure is termed

A

hypotonic

57
Q

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

A

plasmolysis

58
Q

solutions having same osmotic pressures are termed

A

isotonic

59
Q

define Boyle-van’t Hoff law

A

The osmotic pressure (P or pi)
of a solution is directly proportional to its concentration (C )
when the temperature is kept constant

60
Q

when concentration and
temperature both are changing, the osmotic pressure will be
given by

A

PV=nST or πV=nST(S is called molar solution constant.) (no of moles of solute)

61
Q

when is no flow
of solvent molecules is observed on either side during osmosis

A

When two isotonic
solutions are separated by a semipermeable membrane

62
Q

DETERMINATION OF MOLECULAR
MASSES by osmotic pressure

A

mb = Wb X S X T / PV

63
Q

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?

A

π1V1+ π2V2 = πr(VI + V2) [ πr= resultant osmoics pressure]

64
Q

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

A

π = (n1i1 +n2 i2 ) RT/( V1+V2) [ i1 and i
2 are van’t Hoff factor for the two solutes.]
,

65
Q

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

A

reverse osmosis

66
Q

Abnormal colligative property/ normal colligative property is called

A

van hoff factor i

67
Q

van hoff factor=

A

Actual no. of particles in solution/
No. of particles taken

68
Q

Total number of particles in solution=

A

1+ (n -l)alpha (alpha= degree of association )

69
Q
A
70
Q
A

IIT JEE (19 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions