Chapter
stringclasses 18
values | sentence_range
stringlengths 3
9
| Text
stringlengths 7
7.34k
|
|---|---|---|
1 | 1305-1308 | 2 K = 270 95 K
1 00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the
freezing point of benzene by 0 40 K |
1 | 1306-1309 | 95 K
1 00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the
freezing point of benzene by 0 40 K The freezing point depression constant
of benzene is 5 |
1 | 1307-1310 | 00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the
freezing point of benzene by 0 40 K The freezing point depression constant
of benzene is 5 12 K kg mol–1 |
1 | 1308-1311 | 40 K The freezing point depression constant
of benzene is 5 12 K kg mol–1 Find the molar mass of the solute |
1 | 1309-1312 | The freezing point depression constant
of benzene is 5 12 K kg mol–1 Find the molar mass of the solute Substituting the values of various terms involved in equation (1 |
1 | 1310-1313 | 12 K kg mol–1 Find the molar mass of the solute Substituting the values of various terms involved in equation (1 36) we get,
M2 =
1
1
5 |
1 | 1311-1314 | Find the molar mass of the solute Substituting the values of various terms involved in equation (1 36) we get,
M2 =
1
1
5 12 K kg mol
× 1 |
1 | 1312-1315 | Substituting the values of various terms involved in equation (1 36) we get,
M2 =
1
1
5 12 K kg mol
× 1 00 g × 1000 g kg
0 |
1 | 1313-1316 | 36) we get,
M2 =
1
1
5 12 K kg mol
× 1 00 g × 1000 g kg
0 40 × 50 g
= 256 g mol-1
Thus, molar mass of the solute = 256 g mol-1
Example 1 |
1 | 1314-1317 | 12 K kg mol
× 1 00 g × 1000 g kg
0 40 × 50 g
= 256 g mol-1
Thus, molar mass of the solute = 256 g mol-1
Example 1 9
Example 1 |
1 | 1315-1318 | 00 g × 1000 g kg
0 40 × 50 g
= 256 g mol-1
Thus, molar mass of the solute = 256 g mol-1
Example 1 9
Example 1 9
Example 1 |
1 | 1316-1319 | 40 × 50 g
= 256 g mol-1
Thus, molar mass of the solute = 256 g mol-1
Example 1 9
Example 1 9
Example 1 9
Example 1 |
1 | 1317-1320 | 9
Example 1 9
Example 1 9
Example 1 9
Example 1 |
1 | 1318-1321 | 9
Example 1 9
Example 1 9
Example 1 9
Example 1 |
1 | 1319-1322 | 9
Example 1 9
Example 1 9
Example 1 10
Example 1 |
1 | 1320-1323 | 9
Example 1 9
Example 1 10
Example 1 10
Example 1 |
1 | 1321-1324 | 9
Example 1 10
Example 1 10
Example 1 10
Example 1 |
1 | 1322-1325 | 10
Example 1 10
Example 1 10
Example 1 10
Example 1 |
1 | 1323-1326 | 10
Example 1 10
Example 1 10
Example 1 10
There are many phenomena which we observe in nature or at home |
1 | 1324-1327 | 10
Example 1 10
Example 1 10
There are many phenomena which we observe in nature or at home For example, raw mangoes shrivel when pickled in brine (salt water);
wilted flowers revive when placed in fresh water, blood cells collapse
when suspended in saline water, etc |
1 | 1325-1328 | 10
Example 1 10
There are many phenomena which we observe in nature or at home For example, raw mangoes shrivel when pickled in brine (salt water);
wilted flowers revive when placed in fresh water, blood cells collapse
when suspended in saline water, etc If we look into these processes we
find one thing common in all,
that is, all these substances
are bound by membranes |
1 | 1326-1329 | 10
There are many phenomena which we observe in nature or at home For example, raw mangoes shrivel when pickled in brine (salt water);
wilted flowers revive when placed in fresh water, blood cells collapse
when suspended in saline water, etc If we look into these processes we
find one thing common in all,
that is, all these substances
are bound by membranes These membranes can be of
animal or vegetable origin
and these occur naturally
such as pig’s bladder or
parchment or can be
synthetic such as cellophane |
1 | 1327-1330 | For example, raw mangoes shrivel when pickled in brine (salt water);
wilted flowers revive when placed in fresh water, blood cells collapse
when suspended in saline water, etc If we look into these processes we
find one thing common in all,
that is, all these substances
are bound by membranes These membranes can be of
animal or vegetable origin
and these occur naturally
such as pig’s bladder or
parchment or can be
synthetic such as cellophane These membranes appear to
be continuous sheets or
films, yet they contain a
network of submicroscopic
holes or pores |
1 | 1328-1331 | If we look into these processes we
find one thing common in all,
that is, all these substances
are bound by membranes These membranes can be of
animal or vegetable origin
and these occur naturally
such as pig’s bladder or
parchment or can be
synthetic such as cellophane These membranes appear to
be continuous sheets or
films, yet they contain a
network of submicroscopic
holes or pores Small solvent
Solution
Solution
Solution
Solution
Solution
Solution
Solution
Solution
Solution
Solution
1 |
1 | 1329-1332 | These membranes can be of
animal or vegetable origin
and these occur naturally
such as pig’s bladder or
parchment or can be
synthetic such as cellophane These membranes appear to
be continuous sheets or
films, yet they contain a
network of submicroscopic
holes or pores Small solvent
Solution
Solution
Solution
Solution
Solution
Solution
Solution
Solution
Solution
Solution
1 6 |
1 | 1330-1333 | These membranes appear to
be continuous sheets or
films, yet they contain a
network of submicroscopic
holes or pores Small solvent
Solution
Solution
Solution
Solution
Solution
Solution
Solution
Solution
Solution
Solution
1 6 4 Osmosis
and Osmotic
Pressure
Rationalised 2023-24
21
Solutions
molecules, like water, can pass through these holes but the passage of
bigger molecules like solute is hindered |
1 | 1331-1334 | Small solvent
Solution
Solution
Solution
Solution
Solution
Solution
Solution
Solution
Solution
Solution
1 6 4 Osmosis
and Osmotic
Pressure
Rationalised 2023-24
21
Solutions
molecules, like water, can pass through these holes but the passage of
bigger molecules like solute is hindered Membranes having this kind
of properties are known as semipermeable membranes (SPM) |
1 | 1332-1335 | 6 4 Osmosis
and Osmotic
Pressure
Rationalised 2023-24
21
Solutions
molecules, like water, can pass through these holes but the passage of
bigger molecules like solute is hindered Membranes having this kind
of properties are known as semipermeable membranes (SPM) Assume that only solvent molecules can pass through these semi-
permeable membranes |
1 | 1333-1336 | 4 Osmosis
and Osmotic
Pressure
Rationalised 2023-24
21
Solutions
molecules, like water, can pass through these holes but the passage of
bigger molecules like solute is hindered Membranes having this kind
of properties are known as semipermeable membranes (SPM) Assume that only solvent molecules can pass through these semi-
permeable membranes If this membrane is placed between the solvent
and solution as shown in Fig |
1 | 1334-1337 | Membranes having this kind
of properties are known as semipermeable membranes (SPM) Assume that only solvent molecules can pass through these semi-
permeable membranes If this membrane is placed between the solvent
and solution as shown in Fig 1 |
1 | 1335-1338 | Assume that only solvent molecules can pass through these semi-
permeable membranes If this membrane is placed between the solvent
and solution as shown in Fig 1 9, the solvent molecules will flow through
the membrane from pure solvent to the solution |
1 | 1336-1339 | If this membrane is placed between the solvent
and solution as shown in Fig 1 9, the solvent molecules will flow through
the membrane from pure solvent to the solution This process of flow
of the solvent is called osmosis |
1 | 1337-1340 | 1 9, the solvent molecules will flow through
the membrane from pure solvent to the solution This process of flow
of the solvent is called osmosis The flow will continue till the equilibrium is attained |
1 | 1338-1341 | 9, the solvent molecules will flow through
the membrane from pure solvent to the solution This process of flow
of the solvent is called osmosis The flow will continue till the equilibrium is attained The flow of the
solvent from its side to solution side across a semipermeable membrane
can be stopped if some extra pressure is applied on the solution |
1 | 1339-1342 | This process of flow
of the solvent is called osmosis The flow will continue till the equilibrium is attained The flow of the
solvent from its side to solution side across a semipermeable membrane
can be stopped if some extra pressure is applied on the solution This
pressure that just stops the flow of solvent is called osmotic
pressure of the solution |
1 | 1340-1343 | The flow will continue till the equilibrium is attained The flow of the
solvent from its side to solution side across a semipermeable membrane
can be stopped if some extra pressure is applied on the solution This
pressure that just stops the flow of solvent is called osmotic
pressure of the solution The flow of solvent from dilute solution to
the concentrated solution across a semipermeable membrane is due to
osmosis |
1 | 1341-1344 | The flow of the
solvent from its side to solution side across a semipermeable membrane
can be stopped if some extra pressure is applied on the solution This
pressure that just stops the flow of solvent is called osmotic
pressure of the solution The flow of solvent from dilute solution to
the concentrated solution across a semipermeable membrane is due to
osmosis The important point to be kept in mind is that solvent molecules
always flow from lower concentration to higher concentration of solution |
1 | 1342-1345 | This
pressure that just stops the flow of solvent is called osmotic
pressure of the solution The flow of solvent from dilute solution to
the concentrated solution across a semipermeable membrane is due to
osmosis The important point to be kept in mind is that solvent molecules
always flow from lower concentration to higher concentration of solution The osmotic pressure has been found to depend on the concentration
of the solution |
1 | 1343-1346 | The flow of solvent from dilute solution to
the concentrated solution across a semipermeable membrane is due to
osmosis The important point to be kept in mind is that solvent molecules
always flow from lower concentration to higher concentration of solution The osmotic pressure has been found to depend on the concentration
of the solution The osmotic pressure of a solution is the
excess pressure that must be applied to a
solution to prevent osmosis, i |
1 | 1344-1347 | The important point to be kept in mind is that solvent molecules
always flow from lower concentration to higher concentration of solution The osmotic pressure has been found to depend on the concentration
of the solution The osmotic pressure of a solution is the
excess pressure that must be applied to a
solution to prevent osmosis, i e |
1 | 1345-1348 | The osmotic pressure has been found to depend on the concentration
of the solution The osmotic pressure of a solution is the
excess pressure that must be applied to a
solution to prevent osmosis, i e , to stop the
passage of solvent molecules through a
semipermeable membrane into the solution |
1 | 1346-1349 | The osmotic pressure of a solution is the
excess pressure that must be applied to a
solution to prevent osmosis, i e , to stop the
passage of solvent molecules through a
semipermeable membrane into the solution This
is illustrated in Fig |
1 | 1347-1350 | e , to stop the
passage of solvent molecules through a
semipermeable membrane into the solution This
is illustrated in Fig 1 |
1 | 1348-1351 | , to stop the
passage of solvent molecules through a
semipermeable membrane into the solution This
is illustrated in Fig 1 10 |
1 | 1349-1352 | This
is illustrated in Fig 1 10 Osmotic pressure is a
colligative property as it depends on the number
of solute molecules and not on their identity |
1 | 1350-1353 | 1 10 Osmotic pressure is a
colligative property as it depends on the number
of solute molecules and not on their identity For dilute solutions, it has been found
experimentally that osmotic pressure is
proportional to the molarity, C of the
solution at a given temperature T |
1 | 1351-1354 | 10 Osmotic pressure is a
colligative property as it depends on the number
of solute molecules and not on their identity For dilute solutions, it has been found
experimentally that osmotic pressure is
proportional to the molarity, C of the
solution at a given temperature T Thus:
P = C R T
(1 |
1 | 1352-1355 | Osmotic pressure is a
colligative property as it depends on the number
of solute molecules and not on their identity For dilute solutions, it has been found
experimentally that osmotic pressure is
proportional to the molarity, C of the
solution at a given temperature T Thus:
P = C R T
(1 39)
Here P is the osmotic pressure and R is the
gas constant |
1 | 1353-1356 | For dilute solutions, it has been found
experimentally that osmotic pressure is
proportional to the molarity, C of the
solution at a given temperature T Thus:
P = C R T
(1 39)
Here P is the osmotic pressure and R is the
gas constant P = (n2 /V) R T
(1 |
1 | 1354-1357 | Thus:
P = C R T
(1 39)
Here P is the osmotic pressure and R is the
gas constant P = (n2 /V) R T
(1 40)
Here V is volume of a solution in litres containing n2 moles of solute |
1 | 1355-1358 | 39)
Here P is the osmotic pressure and R is the
gas constant P = (n2 /V) R T
(1 40)
Here V is volume of a solution in litres containing n2 moles of solute If w2 grams of solute, of molar mass, M2 is present in the solution, then
n2 = w2 / M2 and we can write,
P V =
2
2
w
MR T
(1 |
1 | 1356-1359 | P = (n2 /V) R T
(1 40)
Here V is volume of a solution in litres containing n2 moles of solute If w2 grams of solute, of molar mass, M2 is present in the solution, then
n2 = w2 / M2 and we can write,
P V =
2
2
w
MR T
(1 41)
or M2 =
∏
w2
R T
V
(1 |
1 | 1357-1360 | 40)
Here V is volume of a solution in litres containing n2 moles of solute If w2 grams of solute, of molar mass, M2 is present in the solution, then
n2 = w2 / M2 and we can write,
P V =
2
2
w
MR T
(1 41)
or M2 =
∏
w2
R T
V
(1 42)
Thus, knowing the quantities w2, T, P and V we can calculate the
molar mass of the solute |
1 | 1358-1361 | If w2 grams of solute, of molar mass, M2 is present in the solution, then
n2 = w2 / M2 and we can write,
P V =
2
2
w
MR T
(1 41)
or M2 =
∏
w2
R T
V
(1 42)
Thus, knowing the quantities w2, T, P and V we can calculate the
molar mass of the solute Measurement of osmotic pressure provides another method of
determining molar masses of solutes |
1 | 1359-1362 | 41)
or M2 =
∏
w2
R T
V
(1 42)
Thus, knowing the quantities w2, T, P and V we can calculate the
molar mass of the solute Measurement of osmotic pressure provides another method of
determining molar masses of solutes This method is widely used to
determine molar masses of proteins, polymers and other
Fig |
1 | 1360-1363 | 42)
Thus, knowing the quantities w2, T, P and V we can calculate the
molar mass of the solute Measurement of osmotic pressure provides another method of
determining molar masses of solutes This method is widely used to
determine molar masses of proteins, polymers and other
Fig 1 |
1 | 1361-1364 | Measurement of osmotic pressure provides another method of
determining molar masses of solutes This method is widely used to
determine molar masses of proteins, polymers and other
Fig 1 10: The excess pressure equal to the
osmotic pressure must be applied on
the solution side to prevent osmosis |
1 | 1362-1365 | This method is widely used to
determine molar masses of proteins, polymers and other
Fig 1 10: The excess pressure equal to the
osmotic pressure must be applied on
the solution side to prevent osmosis Rationalised 2023-24
22
Chemistry
macromolecules |
1 | 1363-1366 | 1 10: The excess pressure equal to the
osmotic pressure must be applied on
the solution side to prevent osmosis Rationalised 2023-24
22
Chemistry
macromolecules The osmotic pressure method has the advantage over
other methods as pressure measurement is around the room
temperature and the molarity of the solution is used instead of molality |
1 | 1364-1367 | 10: The excess pressure equal to the
osmotic pressure must be applied on
the solution side to prevent osmosis Rationalised 2023-24
22
Chemistry
macromolecules The osmotic pressure method has the advantage over
other methods as pressure measurement is around the room
temperature and the molarity of the solution is used instead of molality As compared to other colligative properties, its magnitude is large
even for very dilute solutions |
1 | 1365-1368 | Rationalised 2023-24
22
Chemistry
macromolecules The osmotic pressure method has the advantage over
other methods as pressure measurement is around the room
temperature and the molarity of the solution is used instead of molality As compared to other colligative properties, its magnitude is large
even for very dilute solutions The technique of osmotic pressure for
determination of molar mass of solutes is particularly useful for
biomolecules as they are generally not stable at higher temperatures
and polymers have poor solubility |
1 | 1366-1369 | The osmotic pressure method has the advantage over
other methods as pressure measurement is around the room
temperature and the molarity of the solution is used instead of molality As compared to other colligative properties, its magnitude is large
even for very dilute solutions The technique of osmotic pressure for
determination of molar mass of solutes is particularly useful for
biomolecules as they are generally not stable at higher temperatures
and polymers have poor solubility Two solutions having same osmotic pressure at a given
temperature are called isotonic solutions |
1 | 1367-1370 | As compared to other colligative properties, its magnitude is large
even for very dilute solutions The technique of osmotic pressure for
determination of molar mass of solutes is particularly useful for
biomolecules as they are generally not stable at higher temperatures
and polymers have poor solubility Two solutions having same osmotic pressure at a given
temperature are called isotonic solutions When such solutions
are separated by semipermeable membrane no osmosis occurs
between them |
1 | 1368-1371 | The technique of osmotic pressure for
determination of molar mass of solutes is particularly useful for
biomolecules as they are generally not stable at higher temperatures
and polymers have poor solubility Two solutions having same osmotic pressure at a given
temperature are called isotonic solutions When such solutions
are separated by semipermeable membrane no osmosis occurs
between them For example, the osmotic pressure associated
with the fluid inside the blood cell is equivalent to that of
0 |
1 | 1369-1372 | Two solutions having same osmotic pressure at a given
temperature are called isotonic solutions When such solutions
are separated by semipermeable membrane no osmosis occurs
between them For example, the osmotic pressure associated
with the fluid inside the blood cell is equivalent to that of
0 9% (mass/volume) sodium chloride solution, called normal saline
solution and it is safe to inject intravenously |
1 | 1370-1373 | When such solutions
are separated by semipermeable membrane no osmosis occurs
between them For example, the osmotic pressure associated
with the fluid inside the blood cell is equivalent to that of
0 9% (mass/volume) sodium chloride solution, called normal saline
solution and it is safe to inject intravenously On the other hand, if
we place the cells in a solution containing more than 0 |
1 | 1371-1374 | For example, the osmotic pressure associated
with the fluid inside the blood cell is equivalent to that of
0 9% (mass/volume) sodium chloride solution, called normal saline
solution and it is safe to inject intravenously On the other hand, if
we place the cells in a solution containing more than 0 9% (mass/
volume) sodium chloride, water will flow out of the cells and they
would shrink |
1 | 1372-1375 | 9% (mass/volume) sodium chloride solution, called normal saline
solution and it is safe to inject intravenously On the other hand, if
we place the cells in a solution containing more than 0 9% (mass/
volume) sodium chloride, water will flow out of the cells and they
would shrink Such a solution is called hypertonic |
1 | 1373-1376 | On the other hand, if
we place the cells in a solution containing more than 0 9% (mass/
volume) sodium chloride, water will flow out of the cells and they
would shrink Such a solution is called hypertonic If the salt
concentration is less than 0 |
1 | 1374-1377 | 9% (mass/
volume) sodium chloride, water will flow out of the cells and they
would shrink Such a solution is called hypertonic If the salt
concentration is less than 0 9% (mass/volume), the solution is said
to be hypotonic |
1 | 1375-1378 | Such a solution is called hypertonic If the salt
concentration is less than 0 9% (mass/volume), the solution is said
to be hypotonic In this case, water will flow into the cells if placed
in this solution and they would swell |
1 | 1376-1379 | If the salt
concentration is less than 0 9% (mass/volume), the solution is said
to be hypotonic In this case, water will flow into the cells if placed
in this solution and they would swell 200 cm3 of an aqueous solution of a protein contains 1 |
1 | 1377-1380 | 9% (mass/volume), the solution is said
to be hypotonic In this case, water will flow into the cells if placed
in this solution and they would swell 200 cm3 of an aqueous solution of a protein contains 1 26 g of the
protein |
1 | 1378-1381 | In this case, water will flow into the cells if placed
in this solution and they would swell 200 cm3 of an aqueous solution of a protein contains 1 26 g of the
protein The osmotic pressure of such a solution at 300 K is found to
be 2 |
1 | 1379-1382 | 200 cm3 of an aqueous solution of a protein contains 1 26 g of the
protein The osmotic pressure of such a solution at 300 K is found to
be 2 57 × 10-3 bar |
1 | 1380-1383 | 26 g of the
protein The osmotic pressure of such a solution at 300 K is found to
be 2 57 × 10-3 bar Calculate the molar mass of the protein |
1 | 1381-1384 | The osmotic pressure of such a solution at 300 K is found to
be 2 57 × 10-3 bar Calculate the molar mass of the protein The various quantities known to us are as follows: P = 2 |
1 | 1382-1385 | 57 × 10-3 bar Calculate the molar mass of the protein The various quantities known to us are as follows: P = 2 57 × 10–3 bar,
V = 200 cm3 = 0 |
1 | 1383-1386 | Calculate the molar mass of the protein The various quantities known to us are as follows: P = 2 57 × 10–3 bar,
V = 200 cm3 = 0 200 litre
T = 300 K
R = 0 |
1 | 1384-1387 | The various quantities known to us are as follows: P = 2 57 × 10–3 bar,
V = 200 cm3 = 0 200 litre
T = 300 K
R = 0 083 L bar mol-1 K-1
Substituting these values in equation (2 |
1 | 1385-1388 | 57 × 10–3 bar,
V = 200 cm3 = 0 200 litre
T = 300 K
R = 0 083 L bar mol-1 K-1
Substituting these values in equation (2 42) we get
M2 =
1
1
3
1 |
1 | 1386-1389 | 200 litre
T = 300 K
R = 0 083 L bar mol-1 K-1
Substituting these values in equation (2 42) we get
M2 =
1
1
3
1 26 g × 0 |
1 | 1387-1390 | 083 L bar mol-1 K-1
Substituting these values in equation (2 42) we get
M2 =
1
1
3
1 26 g × 0 083 L bar K
mol
× 300 K
2 |
1 | 1388-1391 | 42) we get
M2 =
1
1
3
1 26 g × 0 083 L bar K
mol
× 300 K
2 57×10
bar × 0 |
1 | 1389-1392 | 26 g × 0 083 L bar K
mol
× 300 K
2 57×10
bar × 0 200 L
= 61,022 g mol-1
Example 1 |
1 | 1390-1393 | 083 L bar K
mol
× 300 K
2 57×10
bar × 0 200 L
= 61,022 g mol-1
Example 1 11
Example 1 |
1 | 1391-1394 | 57×10
bar × 0 200 L
= 61,022 g mol-1
Example 1 11
Example 1 11
Example 1 |
1 | 1392-1395 | 200 L
= 61,022 g mol-1
Example 1 11
Example 1 11
Example 1 11
Example 1 |
1 | 1393-1396 | 11
Example 1 11
Example 1 11
Example 1 11
Example 1 |
1 | 1394-1397 | 11
Example 1 11
Example 1 11
Example 1 11
Solution
Solution
Solution
Solution
Solution
The phenomena mentioned in the beginning of this section can be
explained on the basis of osmosis |
1 | 1395-1398 | 11
Example 1 11
Example 1 11
Solution
Solution
Solution
Solution
Solution
The phenomena mentioned in the beginning of this section can be
explained on the basis of osmosis A raw mango placed in concentrated
salt solution loses water via osmosis and shrivel into pickle |
1 | 1396-1399 | 11
Example 1 11
Solution
Solution
Solution
Solution
Solution
The phenomena mentioned in the beginning of this section can be
explained on the basis of osmosis A raw mango placed in concentrated
salt solution loses water via osmosis and shrivel into pickle Wilted
flowers revive when placed in fresh water |
1 | 1397-1400 | 11
Solution
Solution
Solution
Solution
Solution
The phenomena mentioned in the beginning of this section can be
explained on the basis of osmosis A raw mango placed in concentrated
salt solution loses water via osmosis and shrivel into pickle Wilted
flowers revive when placed in fresh water A carrot that has become
limp because of water loss into the atmosphere can be placed into the
water making it firm once again |
1 | 1398-1401 | A raw mango placed in concentrated
salt solution loses water via osmosis and shrivel into pickle Wilted
flowers revive when placed in fresh water A carrot that has become
limp because of water loss into the atmosphere can be placed into the
water making it firm once again Water will move into its cells through
osmosis |
1 | 1399-1402 | Wilted
flowers revive when placed in fresh water A carrot that has become
limp because of water loss into the atmosphere can be placed into the
water making it firm once again Water will move into its cells through
osmosis When placed in water containing less than 0 |
1 | 1400-1403 | A carrot that has become
limp because of water loss into the atmosphere can be placed into the
water making it firm once again Water will move into its cells through
osmosis When placed in water containing less than 0 9% (mass/
volume) salt, blood cells swell due to flow of water in them by osmosis |
1 | 1401-1404 | Water will move into its cells through
osmosis When placed in water containing less than 0 9% (mass/
volume) salt, blood cells swell due to flow of water in them by osmosis People taking a lot of salt or salty food experience water retention in
tissue cells and intercellular spaces because of osmosis |
1 | 1402-1405 | When placed in water containing less than 0 9% (mass/
volume) salt, blood cells swell due to flow of water in them by osmosis People taking a lot of salt or salty food experience water retention in
tissue cells and intercellular spaces because of osmosis The resulting
Rationalised 2023-24
23
Solutions
puffiness or swelling is called edema |
1 | 1403-1406 | 9% (mass/
volume) salt, blood cells swell due to flow of water in them by osmosis People taking a lot of salt or salty food experience water retention in
tissue cells and intercellular spaces because of osmosis 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 |
1 | 1404-1407 | People taking a lot of salt or salty food experience water retention in
tissue cells and intercellular spaces because of osmosis 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 |
Subsets and Splits
No community queries yet
The top public SQL queries from the community will appear here once available.