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1 | 1405-1408 | The resulting
Rationalised 2023-24
23
Solutions
puffiness or swelling is called edema Water movement from soil into
plant roots and subsequently into upper portion of the plant is partly
due to osmosis The preservation of meat by salting and of fruits by
adding sugar protects against bacterial action Through the process
of osmosis, a bacterium on salted meat or candid fruit loses water,
shrivels and dies |
1 | 1406-1409 | Water movement from soil into
plant roots and subsequently into upper portion of the plant is partly
due to osmosis The preservation of meat by salting and of fruits by
adding sugar protects against bacterial action Through the process
of osmosis, a bacterium on salted meat or candid fruit loses water,
shrivels and dies The direction of osmosis can be reversed if a pressure larger than the
osmotic pressure is applied to the solution side |
1 | 1407-1410 | The preservation of meat by salting and of fruits by
adding sugar protects against bacterial action Through the process
of osmosis, a bacterium on salted meat or candid fruit loses water,
shrivels and dies The direction of osmosis can be reversed if a pressure larger than the
osmotic pressure is applied to the solution side That is, now the
pure solvent flows out of the solution through the semi permeable
membrane |
1 | 1408-1411 | Through the process
of osmosis, a bacterium on salted meat or candid fruit loses water,
shrivels and dies The direction of osmosis can be reversed if a pressure larger than the
osmotic pressure is applied to the solution side That is, now the
pure solvent flows out of the solution through the semi permeable
membrane This phenomenon is called reverse osmosis and is of
great practical utility |
1 | 1409-1412 | The direction of osmosis can be reversed if a pressure larger than the
osmotic pressure is applied to the solution side That is, now the
pure solvent flows out of the solution through the semi permeable
membrane This phenomenon is called reverse osmosis and is of
great practical utility Reverse osmosis is used in desalination of sea
water |
1 | 1410-1413 | That is, now the
pure solvent flows out of the solution through the semi permeable
membrane This phenomenon is called reverse osmosis and is of
great practical utility Reverse osmosis is used in desalination of sea
water A schematic set up for the process is shown in Fig |
1 | 1411-1414 | This phenomenon is called reverse osmosis and is of
great practical utility Reverse osmosis is used in desalination of sea
water A schematic set up for the process is shown in Fig 1 |
1 | 1412-1415 | Reverse osmosis is used in desalination of sea
water A schematic set up for the process is shown in Fig 1 11 |
1 | 1413-1416 | A schematic set up for the process is shown in Fig 1 11 When pressure more than osmotic pressure is
applied, pure water is squeezed out of the sea
water through the membrane |
1 | 1414-1417 | 1 11 When pressure more than osmotic pressure is
applied, pure water is squeezed out of the sea
water through the membrane A variety of
polymer membranes are available for this
purpose |
1 | 1415-1418 | 11 When pressure more than osmotic pressure is
applied, pure water is squeezed out of the sea
water through the membrane A variety of
polymer membranes are available for this
purpose The pressure required for the reverse osmosis
is quite high |
1 | 1416-1419 | When pressure more than osmotic pressure is
applied, pure water is squeezed out of the sea
water through the membrane A variety of
polymer membranes are available for this
purpose The pressure required for the reverse osmosis
is quite high A workable porous membrane is a
film of cellulose acetate placed over a suitable
support |
1 | 1417-1420 | A variety of
polymer membranes are available for this
purpose The pressure required for the reverse osmosis
is quite high A workable porous membrane is a
film of cellulose acetate placed over a suitable
support Cellulose acetate is permeable to water
but impermeable to impurities and ions present
in sea water |
1 | 1418-1421 | The pressure required for the reverse osmosis
is quite high A workable porous membrane is a
film of cellulose acetate placed over a suitable
support Cellulose acetate is permeable to water
but impermeable to impurities and ions present
in sea water These days many countries use
desalination plants to meet their potable water
requirements |
1 | 1419-1422 | A workable porous membrane is a
film of cellulose acetate placed over a suitable
support Cellulose acetate is permeable to water
but impermeable to impurities and ions present
in sea water These days many countries use
desalination plants to meet their potable water
requirements 1 |
1 | 1420-1423 | Cellulose acetate is permeable to water
but impermeable to impurities and ions present
in sea water These days many countries use
desalination plants to meet their potable water
requirements 1 6 |
1 | 1421-1424 | These days many countries use
desalination plants to meet their potable water
requirements 1 6 5 Reverse
Osmosis and
Water
Purification
Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
1 |
1 | 1422-1425 | 1 6 5 Reverse
Osmosis and
Water
Purification
Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
1 9
Vapour pressure of pure water at 298 K is 23 |
1 | 1423-1426 | 6 5 Reverse
Osmosis and
Water
Purification
Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
1 9
Vapour pressure of pure water at 298 K is 23 8 mm Hg |
1 | 1424-1427 | 5 Reverse
Osmosis and
Water
Purification
Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
1 9
Vapour pressure of pure water at 298 K is 23 8 mm Hg 50 g of urea
(NH2CONH2) is dissolved in 850 g of water |
1 | 1425-1428 | 9
Vapour pressure of pure water at 298 K is 23 8 mm Hg 50 g of urea
(NH2CONH2) is dissolved in 850 g of water Calculate the vapour pressure
of water for this solution and its relative lowering |
1 | 1426-1429 | 8 mm Hg 50 g of urea
(NH2CONH2) is dissolved in 850 g of water Calculate the vapour pressure
of water for this solution and its relative lowering 1 |
1 | 1427-1430 | 50 g of urea
(NH2CONH2) is dissolved in 850 g of water Calculate the vapour pressure
of water for this solution and its relative lowering 1 10 Boiling point of water at 750 mm Hg is 99 |
1 | 1428-1431 | Calculate the vapour pressure
of water for this solution and its relative lowering 1 10 Boiling point of water at 750 mm Hg is 99 63°C |
1 | 1429-1432 | 1 10 Boiling point of water at 750 mm Hg is 99 63°C How much sucrose is to
be added to 500 g of water such that it boils at 100°C |
1 | 1430-1433 | 10 Boiling point of water at 750 mm Hg is 99 63°C How much sucrose is to
be added to 500 g of water such that it boils at 100°C 1 |
1 | 1431-1434 | 63°C How much sucrose is to
be added to 500 g of water such that it boils at 100°C 1 11 Calculate the mass of ascorbic acid (Vitamin C, C6H8O6) to be dissolved in
75 g of acetic acid to lower its melting point by 1 |
1 | 1432-1435 | How much sucrose is to
be added to 500 g of water such that it boils at 100°C 1 11 Calculate the mass of ascorbic acid (Vitamin C, C6H8O6) to be dissolved in
75 g of acetic acid to lower its melting point by 1 5°C |
1 | 1433-1436 | 1 11 Calculate the mass of ascorbic acid (Vitamin C, C6H8O6) to be dissolved in
75 g of acetic acid to lower its melting point by 1 5°C Kf = 3 |
1 | 1434-1437 | 11 Calculate the mass of ascorbic acid (Vitamin C, C6H8O6) to be dissolved in
75 g of acetic acid to lower its melting point by 1 5°C Kf = 3 9 K kg mol-1 |
1 | 1435-1438 | 5°C Kf = 3 9 K kg mol-1 1 |
1 | 1436-1439 | Kf = 3 9 K kg mol-1 1 12 Calculate the osmotic pressure in pascals exerted by a solution prepared
by dissolving 1 |
1 | 1437-1440 | 9 K kg mol-1 1 12 Calculate the osmotic pressure in pascals exerted by a solution prepared
by dissolving 1 0 g of polymer of molar mass 185,000 in 450 mL of water
at 37°C |
1 | 1438-1441 | 1 12 Calculate the osmotic pressure in pascals exerted by a solution prepared
by dissolving 1 0 g of polymer of molar mass 185,000 in 450 mL of water
at 37°C We know that ionic compounds when dissolved in water dissociate into
cations and anions |
1 | 1439-1442 | 12 Calculate the osmotic pressure in pascals exerted by a solution prepared
by dissolving 1 0 g of polymer of molar mass 185,000 in 450 mL of water
at 37°C We know that ionic compounds when dissolved in water dissociate into
cations and anions For example, if we dissolve one mole of KCl (74 |
1 | 1440-1443 | 0 g of polymer of molar mass 185,000 in 450 mL of water
at 37°C We know that ionic compounds when dissolved in water dissociate into
cations and anions For example, if we dissolve one mole of KCl (74 5 g)
in water, we expect one mole each of K+ and Cl– ions to be released in
the solution |
1 | 1441-1444 | We know that ionic compounds when dissolved in water dissociate into
cations and anions For example, if we dissolve one mole of KCl (74 5 g)
in water, we expect one mole each of K+ and Cl– ions to be released in
the solution If this happens, there would be two moles of particles in
the solution |
1 | 1442-1445 | For example, if we dissolve one mole of KCl (74 5 g)
in water, we expect one mole each of K+ and Cl– ions to be released in
the solution If this happens, there would be two moles of particles in
the solution If we ignore interionic attractions, one mole of KCl in
one kg of water would be expected to increase the boiling point by
2 × 0 |
1 | 1443-1446 | 5 g)
in water, we expect one mole each of K+ and Cl– ions to be released in
the solution If this happens, there would be two moles of particles in
the solution If we ignore interionic attractions, one mole of KCl in
one kg of water would be expected to increase the boiling point by
2 × 0 52 K = 1 |
1 | 1444-1447 | If this happens, there would be two moles of particles in
the solution If we ignore interionic attractions, one mole of KCl in
one kg of water would be expected to increase the boiling point by
2 × 0 52 K = 1 04 K |
1 | 1445-1448 | If we ignore interionic attractions, one mole of KCl in
one kg of water would be expected to increase the boiling point by
2 × 0 52 K = 1 04 K Now if we did not know about the degree of
1 |
1 | 1446-1449 | 52 K = 1 04 K Now if we did not know about the degree of
1 7
1 |
1 | 1447-1450 | 04 K Now if we did not know about the degree of
1 7
1 7
1 |
1 | 1448-1451 | Now if we did not know about the degree of
1 7
1 7
1 7
1 |
1 | 1449-1452 | 7
1 7
1 7
1 7
1 |
1 | 1450-1453 | 7
1 7
1 7
1 7
Abnormal
Abnormal
Abnormal
Abnormal
Abnormal
Molar
Molar
Molar
Molar
Molar
Masses
Masses
Masses
Masses
Masses
Π
Fig |
1 | 1451-1454 | 7
1 7
1 7
Abnormal
Abnormal
Abnormal
Abnormal
Abnormal
Molar
Molar
Molar
Molar
Molar
Masses
Masses
Masses
Masses
Masses
Π
Fig 1 |
1 | 1452-1455 | 7
1 7
Abnormal
Abnormal
Abnormal
Abnormal
Abnormal
Molar
Molar
Molar
Molar
Molar
Masses
Masses
Masses
Masses
Masses
Π
Fig 1 11: Reverse osmosis occurs when a
pressure larger than the osmotic
pressure is applied to the solution |
1 | 1453-1456 | 7
Abnormal
Abnormal
Abnormal
Abnormal
Abnormal
Molar
Molar
Molar
Molar
Molar
Masses
Masses
Masses
Masses
Masses
Π
Fig 1 11: Reverse osmosis occurs when a
pressure larger than the osmotic
pressure is applied to the solution Rationalised 2023-24
24
Chemistry
2 CH3COOH ⇌ (CH3COOH)2
dissociation, we could be led to conclude that the mass of 2 mol particles
is 74 |
1 | 1454-1457 | 1 11: Reverse osmosis occurs when a
pressure larger than the osmotic
pressure is applied to the solution Rationalised 2023-24
24
Chemistry
2 CH3COOH ⇌ (CH3COOH)2
dissociation, we could be led to conclude that the mass of 2 mol particles
is 74 5 g and the mass of one mole of KCl would be 37 |
1 | 1455-1458 | 11: Reverse osmosis occurs when a
pressure larger than the osmotic
pressure is applied to the solution Rationalised 2023-24
24
Chemistry
2 CH3COOH ⇌ (CH3COOH)2
dissociation, we could be led to conclude that the mass of 2 mol particles
is 74 5 g and the mass of one mole of KCl would be 37 25 g |
1 | 1456-1459 | Rationalised 2023-24
24
Chemistry
2 CH3COOH ⇌ (CH3COOH)2
dissociation, we could be led to conclude that the mass of 2 mol particles
is 74 5 g and the mass of one mole of KCl would be 37 25 g This
brings into light the rule that, when there is dissociation of solute into
ions, the experimentally determined molar mass is always lower than
the true value |
1 | 1457-1460 | 5 g and the mass of one mole of KCl would be 37 25 g This
brings into light the rule that, when there is dissociation of solute into
ions, the experimentally determined molar mass is always lower than
the true value Molecules of ethanoic acid (acetic acid) dimerise in
benzene due to hydrogen bonding |
1 | 1458-1461 | 25 g This
brings into light the rule that, when there is dissociation of solute into
ions, the experimentally determined molar mass is always lower than
the true value Molecules of ethanoic acid (acetic acid) dimerise in
benzene due to hydrogen bonding This normally happens
in solvents of low dielectric constant |
1 | 1459-1462 | This
brings into light the rule that, when there is dissociation of solute into
ions, the experimentally determined molar mass is always lower than
the true value Molecules of ethanoic acid (acetic acid) dimerise in
benzene due to hydrogen bonding This normally happens
in solvents of low dielectric constant In this case the number
of particles is reduced due to dimerisation |
1 | 1460-1463 | Molecules of ethanoic acid (acetic acid) dimerise in
benzene due to hydrogen bonding This normally happens
in solvents of low dielectric constant In this case the number
of particles is reduced due to dimerisation Association of
molecules is depicted as follows:
It can be undoubtedly stated here that if all the molecules of ethanoic
acid associate in benzene, then DTb or DTf for ethanoic acid will be half
of the normal value |
1 | 1461-1464 | This normally happens
in solvents of low dielectric constant In this case the number
of particles is reduced due to dimerisation Association of
molecules is depicted as follows:
It can be undoubtedly stated here that if all the molecules of ethanoic
acid associate in benzene, then DTb or DTf for ethanoic acid will be half
of the normal value The molar mass calculated on the basis of this DTb
or DTf will, therefore, be twice the expected value |
1 | 1462-1465 | In this case the number
of particles is reduced due to dimerisation Association of
molecules is depicted as follows:
It can be undoubtedly stated here that if all the molecules of ethanoic
acid associate in benzene, then DTb or DTf for ethanoic acid will be half
of the normal value The molar mass calculated on the basis of this DTb
or DTf will, therefore, be twice the expected value Such a molar mass
that is either lower or higher than the expected or normal value is called
as abnormal molar mass |
1 | 1463-1466 | Association of
molecules is depicted as follows:
It can be undoubtedly stated here that if all the molecules of ethanoic
acid associate in benzene, then DTb or DTf for ethanoic acid will be half
of the normal value The molar mass calculated on the basis of this DTb
or DTf will, therefore, be twice the expected value Such a molar mass
that is either lower or higher than the expected or normal value is called
as abnormal molar mass In 1880 van’t Hoff introduced a factor i, known as the van’t Hoff
factor, to account for the extent of dissociation or association |
1 | 1464-1467 | The molar mass calculated on the basis of this DTb
or DTf will, therefore, be twice the expected value Such a molar mass
that is either lower or higher than the expected or normal value is called
as abnormal molar mass In 1880 van’t Hoff introduced a factor i, known as the van’t Hoff
factor, to account for the extent of dissociation or association This
factor i is defined as:
Normal molar mass
Abnormal molar mass
i
Observed colligative property
Calculated colligative property
Total number of moles of particles after association/dissociation
Number of moles of particles before association/dissociation
i
Here abnormal molar mass is the experimentally determined molar
mass and calculated colligative properties are obtained by assuming
that the non-volatile solute is neither associated nor dissociated |
1 | 1465-1468 | Such a molar mass
that is either lower or higher than the expected or normal value is called
as abnormal molar mass In 1880 van’t Hoff introduced a factor i, known as the van’t Hoff
factor, to account for the extent of dissociation or association This
factor i is defined as:
Normal molar mass
Abnormal molar mass
i
Observed colligative property
Calculated colligative property
Total number of moles of particles after association/dissociation
Number of moles of particles before association/dissociation
i
Here abnormal molar mass is the experimentally determined molar
mass and calculated colligative properties are obtained by assuming
that the non-volatile solute is neither associated nor dissociated In
case of association, value of i is less than unity while for dissociation it
is greater than unity |
1 | 1466-1469 | In 1880 van’t Hoff introduced a factor i, known as the van’t Hoff
factor, to account for the extent of dissociation or association This
factor i is defined as:
Normal molar mass
Abnormal molar mass
i
Observed colligative property
Calculated colligative property
Total number of moles of particles after association/dissociation
Number of moles of particles before association/dissociation
i
Here abnormal molar mass is the experimentally determined molar
mass and calculated colligative properties are obtained by assuming
that the non-volatile solute is neither associated nor dissociated In
case of association, value of i is less than unity while for dissociation it
is greater than unity For example, the value of i for aqueous KCl
solution is close to 2, while the value for ethanoic acid in benzene is
nearly 0 |
1 | 1467-1470 | This
factor i is defined as:
Normal molar mass
Abnormal molar mass
i
Observed colligative property
Calculated colligative property
Total number of moles of particles after association/dissociation
Number of moles of particles before association/dissociation
i
Here abnormal molar mass is the experimentally determined molar
mass and calculated colligative properties are obtained by assuming
that the non-volatile solute is neither associated nor dissociated In
case of association, value of i is less than unity while for dissociation it
is greater than unity For example, the value of i for aqueous KCl
solution is close to 2, while the value for ethanoic acid in benzene is
nearly 0 5 |
1 | 1468-1471 | In
case of association, value of i is less than unity while for dissociation it
is greater than unity For example, the value of i for aqueous KCl
solution is close to 2, while the value for ethanoic acid in benzene is
nearly 0 5 Inclusion of van’t Hoff factor modifies the equations for colligative
properties as follows:
Relative lowering of vapour pressure of solvent,
1o
1
2
o
1
1
–
|
1 | 1469-1472 | For example, the value of i for aqueous KCl
solution is close to 2, while the value for ethanoic acid in benzene is
nearly 0 5 Inclusion of van’t Hoff factor modifies the equations for colligative
properties as follows:
Relative lowering of vapour pressure of solvent,
1o
1
2
o
1
1
–
p
p
i nn
p
Elevation of Boiling point, DTb = i Kb m
Depression of Freezing point, DTf = i Kf m
Osmotic pressure of solution, P
= i n2 R T / V
Rationalised 2023-24
25
Solutions
2 g of benzoic acid (C6H5COOH) dissolved in 25 g of benzene shows a
depression in freezing point equal to 1 |
1 | 1470-1473 | 5 Inclusion of van’t Hoff factor modifies the equations for colligative
properties as follows:
Relative lowering of vapour pressure of solvent,
1o
1
2
o
1
1
–
p
p
i nn
p
Elevation of Boiling point, DTb = i Kb m
Depression of Freezing point, DTf = i Kf m
Osmotic pressure of solution, P
= i n2 R T / V
Rationalised 2023-24
25
Solutions
2 g of benzoic acid (C6H5COOH) dissolved in 25 g of benzene shows a
depression in freezing point equal to 1 62 K |
1 | 1471-1474 | Inclusion of van’t Hoff factor modifies the equations for colligative
properties as follows:
Relative lowering of vapour pressure of solvent,
1o
1
2
o
1
1
–
p
p
i nn
p
Elevation of Boiling point, DTb = i Kb m
Depression of Freezing point, DTf = i Kf m
Osmotic pressure of solution, P
= i n2 R T / V
Rationalised 2023-24
25
Solutions
2 g of benzoic acid (C6H5COOH) dissolved in 25 g of benzene shows a
depression in freezing point equal to 1 62 K Molal depression constant
for benzene is 4 |
1 | 1472-1475 | p
p
i nn
p
Elevation of Boiling point, DTb = i Kb m
Depression of Freezing point, DTf = i Kf m
Osmotic pressure of solution, P
= i n2 R T / V
Rationalised 2023-24
25
Solutions
2 g of benzoic acid (C6H5COOH) dissolved in 25 g of benzene shows a
depression in freezing point equal to 1 62 K Molal depression constant
for benzene is 4 9 K kg mol–1 |
1 | 1473-1476 | 62 K Molal depression constant
for benzene is 4 9 K kg mol–1 What is the percentage association of acid
if it forms dimer in solution |
1 | 1474-1477 | Molal depression constant
for benzene is 4 9 K kg mol–1 What is the percentage association of acid
if it forms dimer in solution The given quantities are: w2 = 2 g; Kf = 4 |
1 | 1475-1478 | 9 K kg mol–1 What is the percentage association of acid
if it forms dimer in solution The given quantities are: w2 = 2 g; Kf = 4 9 K kg mol–1; w1 = 25 g,
DTf = 1 |
1 | 1476-1479 | What is the percentage association of acid
if it forms dimer in solution The given quantities are: w2 = 2 g; Kf = 4 9 K kg mol–1; w1 = 25 g,
DTf = 1 62 K
Substituting these values in equation (1 |
1 | 1477-1480 | The given quantities are: w2 = 2 g; Kf = 4 9 K kg mol–1; w1 = 25 g,
DTf = 1 62 K
Substituting these values in equation (1 36) we get:
M2 =
–1
–1
4 |
1 | 1478-1481 | 9 K kg mol–1; w1 = 25 g,
DTf = 1 62 K
Substituting these values in equation (1 36) we get:
M2 =
–1
–1
4 9 K kg mol
× 2 g × 1000 g kg
25 g × 1 |
1 | 1479-1482 | 62 K
Substituting these values in equation (1 36) we get:
M2 =
–1
–1
4 9 K kg mol
× 2 g × 1000 g kg
25 g × 1 62 K
= 241 |
1 | 1480-1483 | 36) we get:
M2 =
–1
–1
4 9 K kg mol
× 2 g × 1000 g kg
25 g × 1 62 K
= 241 98 g mol–1
Thus, experimental molar mass of benzoic acid in benzene is
= 241 |
1 | 1481-1484 | 9 K kg mol
× 2 g × 1000 g kg
25 g × 1 62 K
= 241 98 g mol–1
Thus, experimental molar mass of benzoic acid in benzene is
= 241 98 g mol–1
Now consider the following equilibrium for the acid:
2 C6H5COOH ⇌ (C6H5COOH)2
If x represents the degree of association of the solute then we would
have (1 – x ) mol of benzoic acid left in unassociated form and
correspondingly 2
x as associated moles of benzoic acid at equilibrium |
1 | 1482-1485 | 62 K
= 241 98 g mol–1
Thus, experimental molar mass of benzoic acid in benzene is
= 241 98 g mol–1
Now consider the following equilibrium for the acid:
2 C6H5COOH ⇌ (C6H5COOH)2
If x represents the degree of association of the solute then we would
have (1 – x ) mol of benzoic acid left in unassociated form and
correspondingly 2
x as associated moles of benzoic acid at equilibrium Therefore, total number of moles of particles at equilibrium is:
1
1
2
2
x
x
x
Thus, total number of moles of particles at equilibrium equals van’t Hoff
factor i |
1 | 1483-1486 | 98 g mol–1
Thus, experimental molar mass of benzoic acid in benzene is
= 241 98 g mol–1
Now consider the following equilibrium for the acid:
2 C6H5COOH ⇌ (C6H5COOH)2
If x represents the degree of association of the solute then we would
have (1 – x ) mol of benzoic acid left in unassociated form and
correspondingly 2
x as associated moles of benzoic acid at equilibrium Therefore, total number of moles of particles at equilibrium is:
1
1
2
2
x
x
x
Thus, total number of moles of particles at equilibrium equals van’t Hoff
factor i But
Normal molar mass
Abnormal molar mass
i
Example 1 |
1 | 1484-1487 | 98 g mol–1
Now consider the following equilibrium for the acid:
2 C6H5COOH ⇌ (C6H5COOH)2
If x represents the degree of association of the solute then we would
have (1 – x ) mol of benzoic acid left in unassociated form and
correspondingly 2
x as associated moles of benzoic acid at equilibrium Therefore, total number of moles of particles at equilibrium is:
1
1
2
2
x
x
x
Thus, total number of moles of particles at equilibrium equals van’t Hoff
factor i But
Normal molar mass
Abnormal molar mass
i
Example 1 12
Example 1 |
1 | 1485-1488 | Therefore, total number of moles of particles at equilibrium is:
1
1
2
2
x
x
x
Thus, total number of moles of particles at equilibrium equals van’t Hoff
factor i But
Normal molar mass
Abnormal molar mass
i
Example 1 12
Example 1 12
Example 1 |
1 | 1486-1489 | But
Normal molar mass
Abnormal molar mass
i
Example 1 12
Example 1 12
Example 1 12
Example 1 |
1 | 1487-1490 | 12
Example 1 12
Example 1 12
Example 1 12
Example 1 |
1 | 1488-1491 | 12
Example 1 12
Example 1 12
Example 1 12
Solution
Solution
Solution
Solution
Solution
Table 1 |
1 | 1489-1492 | 12
Example 1 12
Example 1 12
Solution
Solution
Solution
Solution
Solution
Table 1 4 depicts values of the factor, i for several strong electrolytes |
1 | 1490-1493 | 12
Example 1 12
Solution
Solution
Solution
Solution
Solution
Table 1 4 depicts values of the factor, i for several strong electrolytes For KCl, NaCl and MgSO4, i values approach 2 as the solution becomes
very dilute |
1 | 1491-1494 | 12
Solution
Solution
Solution
Solution
Solution
Table 1 4 depicts values of the factor, i for several strong electrolytes For KCl, NaCl and MgSO4, i values approach 2 as the solution becomes
very dilute As expected, the value of i gets close to 3 for K2SO4 |
1 | 1492-1495 | 4 depicts values of the factor, i for several strong electrolytes For KCl, NaCl and MgSO4, i values approach 2 as the solution becomes
very dilute As expected, the value of i gets close to 3 for K2SO4 Salt
*Values of i
van’t Hoff Factor i for complete
0 |
1 | 1493-1496 | For KCl, NaCl and MgSO4, i values approach 2 as the solution becomes
very dilute As expected, the value of i gets close to 3 for K2SO4 Salt
*Values of i
van’t Hoff Factor i for complete
0 1 m 0 |
1 | 1494-1497 | As expected, the value of i gets close to 3 for K2SO4 Salt
*Values of i
van’t Hoff Factor i for complete
0 1 m 0 01 m
0 |
1 | 1495-1498 | Salt
*Values of i
van’t Hoff Factor i for complete
0 1 m 0 01 m
0 001 m
dissociation of solute
NaCl
1 |
1 | 1496-1499 | 1 m 0 01 m
0 001 m
dissociation of solute
NaCl
1 87
1 |
1 | 1497-1500 | 01 m
0 001 m
dissociation of solute
NaCl
1 87
1 94
1 |
1 | 1498-1501 | 001 m
dissociation of solute
NaCl
1 87
1 94
1 97
2 |
1 | 1499-1502 | 87
1 94
1 97
2 00
KCl
1 |
1 | 1500-1503 | 94
1 97
2 00
KCl
1 85
1 |
1 | 1501-1504 | 97
2 00
KCl
1 85
1 94
1 |
1 | 1502-1505 | 00
KCl
1 85
1 94
1 98
2 |
1 | 1503-1506 | 85
1 94
1 98
2 00
MgSO4
1 |
1 | 1504-1507 | 94
1 98
2 00
MgSO4
1 21
1 |
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