Transcript Document

医学基础化学（1）
刘洛生
82378
[email protected]
课本（英文、中文
CHAPTER 1
2
顺序 3
5
6
10
11
12
共48学时）
Solution ( 4h)
Electrolyte solution (5h)
Buffer solution (4h)
Rates of chemical reaction(4h)
Electrochemistry (6h)
Titrimetry (4h)
Spectrophotometry(2h)
The colloidal system and
surface phenomena (5h)
7 Atomic Structure (4h)
8 Molecular Structure (4h)
9 Coordination Compounds (6h)
学习方法：
• 先中文，再英文 记忆英文的词汇和相关定义
• 正确理解基本概念、基本原理及适用范围
抽象→联系实际，勤思考，理解，推理。
预习自学 记笔记，及时复习、消化、答疑。
重视作业
适当做习题。
每章要求的作业：summary（上交）
CHAPTER ONE
SOLUTION
1-1 Basic Terms of Solution
1-2 Solubility of Solution
1-3 Solution Concentration
1-4 Colligative Properties of Solutions
问题：
生理盐水？（0.9%NaCl）
等渗溶液？（5%GS、50%GS）
肾脏衰竭的治疗方法——血液透析原理？
溶液浓度、渗透及渗透压概念有关
1-1
Basic Terms of Solution
• A solution is a homogeneous mixture of
two or more substances evenly distributed
in each other.
• When one of these substances is a liquid
and the others are so1ids or gases, we tend
to think of the liquid as the substance that
dissolves the solid or gas. The liquid is
referred to as the solvent and the solids and
gases as the solutes.
• Solvent is the substance in a solution
that dissolves another substance; it is
the substance in the solution that is in
greater amount.
• Solute is either a substance in a
solution considered to have been
dissolved by a solvent, or else a
substance in a solution that is in smaller
amount.
• Two liquids that mix completely in one
another to form a solution, no matter what
the proportions of liquids, are said to be
miscible.
Water – alcohol
• Two liquids that do not mix together or
dissolve in one another in significant
amounts, but rather tend to separate into
two distinct layers, are said to be
immiscible .
Water – oil
Solution Process
• What happens when a substance like NaCl
dissolves in water?
When NaCl is added to water, the water
molecules orient themselves on the surface of
the NaCl crystals.
The positive end of the water dipole is
oriented towards the Cl- ions, while the
negative end of the water dipole is oriented
toward the Na+ ions.
• The dipole-ion( 偶 极 离 子 ) attractions between
water molecules and Na+ and Cl- ions are
sufficiently strong to pull these ions from
their positions in the crystal.
• Once removed from the crystal, the Na+ and
Cl- ions are surrounded by water molecules.
• Such interactions between solute and solvent
molecules is known as solvation(溶剂化).
• When the solvent is water it is known as hydration.
（水合）
1-2 Solubility of Solution
• Solubility is the maximum amount of substance
that dissolves in a given volume of solvent at a
specified temperature.
• Suppose you add 60 g of sodium thiosulfate to 100 ml of
water contained in a flask at 20℃.
• After stirring vigorously, you find that 50g of the
crystalline compound dissolves, leaving 10g at the bottom
of the flask.
• Thus, the solubility of sodium thiosulfate at 20℃ is 50 g
in 100 ml of water.

The solution you obtain after you have
dissolved the maximum amount of solute in a
solvent at a given temperature is said to be a
saturated solution.
•
Thus, the solution of 100ml water containing
50g of sodium thiosulfate at 20℃ is a saturated
solution of sodium thiosulfate.
• Any solution that contains less solute in a given
volume of solvent than is contained in the
saturated solution is said to be an unsaturated
solution.
• supersaturated solution, which is a
solution that contains more of a solute
than is contained in the saturated solution.
• How do you know whether a solution is
saturated or supersaturated? (P5)
Factors That Affect Solubility
1. Nature of Solute / Solvent.
2. Temperature i) Solids/Liquids: Solubility increases with temperature
increase .
ii) Gas : Solubility decreases with temperature increase .
3. Pressure Factor i) Solids/Liquids : Very little effect
Solids and Liquids are already close together, extra pressure will not
increase solubility.
ii) Gas: Solubility increases with Pressure.
Solubilities of Solids vs Temperature
MOST salts have greater
solubility in hot water.
A few salts have negative
heat of solution,
(exothermic(放热) process)
and they become less
soluble with increasing
temperature.
Temperature & the Solubility of Gases
The solubility of gases DECREASES at higher temperatures
1-3 Solution Concentration
1-3.1 Amount-of-substance and Molar Mass
1-3.2 Mass Percent of Solute
1-3.3 Mole fraction (Amount-of-substance
Fraction)
1-3.4 Molality
1-3.5 Amount-of-substance Concentration
ways of expressing concentration:
Mass percent: (mass solute / mass of solution) x 100%
Molarity(c): moles solute / Liter solution
Molality* (mB) ： moles solute / Kg solvent
Mole Fraction(x) : moles solute / total moles solution
* Note that molality is the only concentration
unit in which denominator（分母） contains
only solvent information rather than solution.
1-3.2
Mass percent of solute (p11)
mass solute
% (m/m) =
mass solution
x 100
mass solute
% (m/v) =
volume solution
x 100
volume solute
volume solution
x 100
% (v/v) =
Example
3.5 g of CoCl2 is dissolved in 100mL solution.
Assuming the density of the solution is 1.0 g/mL,
what is concentration of the solution in % mass?
% = 3.5 g CoCl2
100g H2O
= 3.5% (m/m)
1-3.3 Mole fraction
(Amount-of-substance Fraction)
Mole fraction of A =
or
xA =
Moles of A (Amount-of-substance of A)
Sum of moles of all components
nA
nA + nB
Example1-1 A chemist prepared a solution by adding 200.4g
of pure ethanol (C2H5OH) to 143.9g of water. Calculate the
mole fraction of these two components?
The mol masses of ethanol and water are 46.02g and 18.02g,
respectively.
Solution:
The Amount-of-substance of C2H5OH and H2O present are :
Amount-of-substance of C2H5OH =
Amount-of-substance of H2O =
200.4g C2H5OH
= 4.355mol
46.02g/mol
143.9g H2O
= 7.986 mol
18.02g/mol
Using equation we can write the mole fraction of ethanol and water as
4.355mol
xC2H5OH =
= 0.3529
(4.355mol+7.986mol)
7.986mol
xH2O =
= 0.6471
(4.355mol+7.986mol)
1-3.4 Molality _____moles solute / kg solvent
• Molality is a concentration unit equal to the
amount-of-substance of solute dissolved in a
kilogram of solvent.
amount-of-substance of solute (nB)
Molality (mB)=
kilograms of solvent (mA)
or
nB
mB =
mA
若将58.5gNaCl溶于1kg水，
所得溶液的质量摩尔浓度是
1.00 mo1·kg ―1
Molarity (c):
_____moles solute / Liter solution
If 0.435 g of KMnO4 is dissolved in enough water to give
250. mL of solution, what is the molarity of KMnO4?
As is almost always the
case, the first step is to
convert the mass of
material to moles.
0.435 g KMnO4 • 1 mol KMnO4 = 0.00275 mol KMnO4
158.0 g KMnO4
Now that the number of moles of substance is known, this can be
combined with the volume of solution — which must be in liters
— to give the molarity. Because 250. mL is equivalent to 0.250 L .
Molarity KMnO4 = 0.00275 mol KMnO4 = 0.0110mol/L
0.250 L solution
1-3.5
Amount-of-substance Concentration
• Amount-of-substance Concentration
is a concentration unit equal to the amount-ofsubstance of solute dissolved in a liter of solution
Amount-of-substance of solute
Amount-of-substance Concentration =
liters of solution
nB
or
cB =
V
实验室常用——物质的量浓度
• 如50ml，18 mo1· L ―1的浓硫酸中所含
H2SO4的物质量(mol) 。
nH 2 SO4
50
 18 
 0.90 (mol)
1000
Solutions By “Parts”
• Parts per million is the number of particles of
solute per one-million particles of solution.
Fluoridated drinking water contains ~ 1 ppm of
fluoride ion.
1 ppm = 1 mg/L (10-3)
• Parts per billion （十亿） is the number of
particles of solute per one-billion particles of
solution.
1 ppb = 1 µg/L (10-6)
• Parts per trillion（万亿） is the number of
particles of solute per one-trillion particles of
solution.
1 ppt = 1 ng/L (10-9)
等物质的量的反应规则
aA + tT
dD + eE
n(aA)  n(tT )  n(dD)  n(eE)
• 关于浓度，细读中文书 p8-10
1-4
Colligative Properties of Solutions
1-4.1 Vapor Pressure Lowering
1-4.2 Boiling Point Elevation
1-4.3 Freezing Point Depression
1-4.4 Osmosis and Osmotic Pressure
1-4.5 The Colligative Properties of Electrolyte Solution
1-4.6 Isotonic(等), Hypotonic (低), Hypertonic (高) Solution
1-4.7 Osmolarity
1-4.8 Crystalloid Osmotic Pressure and Colloidal
Osmotic Pressure
1-4
Colligative Properties of Solutions
• The properties of a solution are differ from
the properties of solute and solvent
•Two kinds of properties :
The first depends on the nature of solute
eg. color 、 electric and the volume change
The second not depend on the nature of solute is called
colligative property
eg. vapor pressure、 boiling point 、freezing point and
osmotic pressure
• colligative property:
All these properties depend on the collective
effect of the number of dissolved particles
(molecules or ions) rather than on the nature
of the particular particles involved
• (1) the lowering of the vapor pressure of the
solution relative to that of the pure solvent,
•(2) the elevation of the boiling point,
•(3) the depression of the freezing point,
•(4) the phenomenon of osmotic pressure.
1-4.1 Lowering of Vapor Pressure
• Evaporation is the process by which
water is converted from its liquid form to its
vapor form.
Evaporation
is a surface
phenomenon some molecules
have enough
kinetic energy to
escape.
1-4.1 Lowering of Vapor Pressure
Condensation is the change of
water from its gaseous form (water vapor)
into liquid water.
If the container is
closed, an equilibrium
is reached where
an equal number of
molecules return to
the surface.
Saturated Vapor Pressure
Equilibrium:
V evaporation = V condensation .
• At this point the vapor is said to be saturated,
and the pressure of that vapor (usually
expressed in mmHg) is called the saturated
vapor pressure.
• The pressure of this equilibrium is called the
saturation vapor pressure .
Lowering of Vapor Pressure
Solvent molecule
solute molecule
(nonvolatile)
(a)vapor pressure of pure solvent (b) vapor pressure of solution
po
p
• The presence of a non-volatile（非挥发性的） solute
means that fewer solvent particles are at the solution’s
surface, so less solvent evaporates!
Δp = po- p
• Vapor pressure of a dilute solution that containing
nonvolatile, nonelectrolyte is directly proportional
to the amount-of-substance fraction of the solvent.
p∝ xA
.
p is the vapor pressure of solution
xA is amount-of-substance fraction of solvent
The constant is the vapor pressure of pure solvent p°
p = p°xA
比例系
数
……（经验公式）
xA+ xB =1
p= po xA = po(1- xB)= po - po xB
∴ p o- p = p o x B
Δp Vapor Pressure Lowering
Δp = po xB
Δp≥0
Raoult’s law :
Vapor pressure lowing of a dilute solution that containing
nonvolatile, nonelectrolyte is directly proportional to the
amount-of-substance fraction of the solute and has
nothing to do with the nature of solute.
Suppose: solvent is 1000g:
For a dilute solution
1000 g
nA 
MA
nA>> nB， (nA+nB≈nA)
nB
nB
xB 

nA  nB nA
MA
p  p xB  p
nm
B
1000 B
Δp=
Δp=KKbbBmBB
若以水为溶剂，
1kgH2O中含有nB
在数值上mB≈nB
(1-9)
• Raoult’s law :
• Vapor pressure lowing of a dilute
solution that containing nonvolatile,
nonelectrolyte is directly proportional to
the molality of the solute and has
nothing to do with the nature of solute.
Δ p = K mB
Raoult’s law : Δ p = K mB
p
T
[例1-6] 已知20℃时水的饱和蒸气压为2.33kPa，将17.1g蔗
糖(C12H22O11)与3.00g尿素[CO(NH2)]2]分别溶于100g水。
计算这两种溶液的蒸气压各是多少？
解：蔗糖的摩尔质量M＝342 g·mol－1，所以溶液的
质量摩尔浓度
mB 
17.1 1000

 0.500
342 100
H2O的摩尔分数 x H O
2
蔗糖溶液的蒸气压
(mol  kg 1 )
1000
55.5
18
.
0


 0.991
1000
00
55.5  0.5
 0.500
18.0
p  pH0 2O  xH 2O
 2.33 0.991 2.31 (kPa)
• 尿素的摩尔质量M＝60.0 g·mol－1，溶液的
质量摩尔浓度
3.00 1000
mB 

 0.500
60.0 100
x H 2O
(mol  kg -1 )
1000
55.5
18.0


 0.991
1000
55.5  0.5
 0.500
18.0
所以尿素溶液中蒸气压
p＝2.31kPa，
这两种溶液的质量分数不同，但溶剂的摩尔分数相
同，蒸气压也就相等。
Application of Vapor Pressure Lowering
• Describe what is happening in the pictures below.
• Use the concept of vapor pressure lowering to
explain this phenomenon.
1-4.2 Elevation of Boiling Point
•Why is responsible for increasing the boiling
point of water with the addition of anti-freeze（防
冻剂） (or salt)?
•Evaporation occurs when molecules have
sufficient energy to escape the interface of a
liquid substance.
Normal Boiling Point:
Temperature at which the vapor
pressure of the liquid is equal to
the atmospheric pressure.
PH2O=P外=101.3 kPa
T=1000C
When a solute contaminates the
solvent, the surface area is
reduced because of the attraction
between solute and solvent, thus the physical
properties (i.e., vapor pressure) are altered.
•Boiling Point Elevation
Δ Tb = (Tb -Tb°)
Tb°_ b.p. of pure solvent
Tb _ b.p. solvent in solution
Δ Tb _ b.p. Elevation
Raoult’s law :
Boiling Point Elevation of a dilute solution that
containing nonvolatile, nonelectrolyte is directly
proportional to the amount-of-substance fraction of the
solute and has nothing to do with the nature of solute.
ΔTb= Kb mB
for water Kb = 0.512
Kb is different for different solvent
•Table 1- 1 Boiling-Point elevation and FreezingPaint Depression Constants
Solvent
Formula
Acetic acid CH3COOH
Benzene
C6H6
Carbon tetrachloride CCl4
Diethyl ether二乙醚C4H 10O
Ethanol
C2H5OH
Naphthalene
C10H8
萘
Water
H2 O
Tb(℃)
Kb
118.1
3.07
80.1
2.53
76.7
5.03
34.7
2.02
78.4
1.22
100.0
0.512
Tf(℃) Kf
17
3.9
5.5
4.9
-22.9
32
- 116.2 1.8
- 114.7
80.5
6.8
0.0
1.86
Example 1-3 （P17）
• When 5.50 g of biphenyl (C12H 10), a nonvolatile
compound, is dissolved in 100.0 g of benzene, the
boiling point of the solution exceeds the boiling point of
pure benzene by 0.903℃. What is Kb for benzene?
• Solution
Because the molar mass of biphenyl is 154 g ·mol-1, 5.50
g of biphenyl contains
5.50g /154g ·mol-1 =0.0357 mol biphenyl
The molality of the biphenyl in the solution is
0.0357 mol
mB = ---------------- = 0.357 mol ·kg-1
0. 1000 kg
ΔTb
0.903 K
Kb = -------- = ----------------- - =2.53 K · kg ·mol-1
mB
0.357 mol /kg
Example 1- 4
（p9）
• When 6.30 g of a nonvolatile
hydrocarbon（烃） of unknown molar
mass is dissolved in 150.0 g of benzene,
the boiling point of the solution is
80.696℃. The boiling point of pure
benzene is 80.099℃. What is the molar
mass of the hydrocarbon?
Exercise
1. What would the boiling point of a
solution be if 60 g of NaCl were dissolved
on 1000g of H2O?
1-4.3 Depression of Freezing Point
• Freezing Point, temperature at which a
liquid congeals(凝结) into the solid state
at a given pressure.
• The temperature at which the solid and
liquid states of the substance are in
equilibrium.
凝固点 是物质的固相与它的液相平衡共存的温度。
•
Water
0 0C
P固相 = P液相（固-液两相共存）
0 0C以上 P固相 〉P液相 （冰溶化）
0 0C以下 P固相 〈 P液相 （水转化为冰）
Freezing point depression
• The depression of the freezing point of a
solution with respect to the pure solvent is
analogous（相似的） to boiling point elevation.
• Here, we consider only the case that only
solvent crystallizes out of solution.
凝固点
是溶剂的固相与液相平衡
共存的温度。
solution：
0 0C
P溶液 〈 P冰
（冰吸收热量融化，使体系温度降低）
Since the solution vapor pressure curve lies below
that of the pure liquid solvent due to Raoult‘s law,
the point of intersection（交点） gives rise to a
lower freezing point for the solution.
•
ΔTf = Kf mB
(1-11)
Tf is subtracted from the normal freezing point of
the solvent.
Kf is the molal freezing point depression constant
of the solvent. Kf is different for different solvent
for water Kf = 1.86
[例1-9]
乙二醇CH2(OH)CH2(OH)是一种常用的汽车防冻剂，它溶于水并
完全是非挥发性的（b.p.197℃）。
计算在2505g水中溶解651g该物质的溶液的凝固点。 夏天能否将它
用于汽车散热器中？
乙二醇的摩尔质量是62.01g/mol。
解：溶液的质量摩尔浓度
mB 
651 1000

 4.19 mol / kg
62.01 2505
ΔTf ＝Kf·mB＝1.86×4.19＝7.79(K)
因为纯水的凝固点是273K，
该溶液凝固点
Tf ＝ 273-7.79 ＝ 265.21K
沸点升高 ΔTb ＝ 0.52×4.19＝2.2（K）
此溶液在375.2K沸腾，所以夏天它能用于汽车散热器中防止
溶液沸腾。
Determining Molecular Weight (p21)
•Dissolves 2.06 g of an unknown solid
substance in 164 g of cyclohexane (C6H12环己烷)
and determines that the freezing point of this
solution is 4.76℃.The freezing point of pure
cyclohexane is 6.47℃; the Kf is 20.0K kg/mol.
What is the molecular weight of the unknown
solid, (Assume that it is nonionizable and
nonvolatile.)
Solution:
The freezing-point depression is
ΔTf =freezing point of pure solvent - freezing point of
solution
= 6.47℃ - 4.76℃ = 1.71 ℃
according to ΔTf = Kf mB
mB =ΔTf / Kf = 1.71 / 20.0 =0.0855 (mol / kg)
Amount-of-substance of solute
(nB)= 0.164kg×0.0855 mol / kg
=0.0140 mol
n = m/M
Molar mass unknown =2.06g /0.0140mol = 147 g/mol
1-4.4 Osmotic Pressure
• Osmosis:
• the process of solvent flow
through a semipermeable
membrane from a pure solvent
or from a dilute solution to a
more concentrated solution in
order to equalize the
concentrations of solutes on the
two sides of the membrane.
Figure : An experiment in osmosis.
达平衡状态时，半透膜两侧
的水位差所表示的静压大小
反映出溶液渗透能力的大小
，溶液的渗透能力用渗透压
表示。
• Osmosis is the spontaneous movement (自发运动)of
water across a semi-permeable membrane from an area
of low solute concentration to an area of high solute
concentration
1-4.4 Osmotic Pressure
•Osmotic Pressure The Pressure that
must be applied to
stop osmosis.
渗透压的定义是：将纯溶剂与溶液以半透膜隔开时，为了
阻止溶剂分子向溶液渗透所需要加给溶液的额外压力。
一定温度下，溶液越浓，
渗透压也越大。
• 实验证明：
在一定温度下，溶液的渗透压与它的浓度成正比；
在一定浓度时，溶液的渗透压与绝对温度成正比。
1886年荷兰物理化学家范托夫（van’t Hoff）综合上述实
验结果，指出了非电解质的稀溶液的渗透压与温度、
浓度的关系：
•
πV ＝ nRT
• osmotic pressure:
Π= cRT
• For a dilute solution, the amount-of-substance
concentration is approximately equal to the molality
of solution,
so
Π= mBRT
公式的意义在于：一定温度下，溶液的渗透压与溶液的质量
摩尔浓度成正比，也就是说，与溶液中所含溶质质点的数目
成正比，而与溶质的本性无关。
Problem
• What would the boiling point of a solution be
if 18.0g of glucose were dissolved on 1000g
of H2O?
• What would the boiling point of a solution be
if 5.85g of NaCl were dissolved on 1000g of
H2O?
freezing point ?
Osmotic Pressure？
1-4.5 The Colligative Properties of
Electrolyte Solution
• Δ p = i K mB
• ΔTb = i Kb mB
• ΔTf = i Kf mB
• Π = i RT mB
i - Van’t Hoff factor
i For sucrose, i =1; for KNO3 , i =2 ; for MgCl2, i = 3
1- 4.6 Isotonic, Hypotonic, Hypertonic Solution
Osmosis —is important in many biological processes
A cell might be thought of as an aqueous
solution surrounded by a semipermeable
membrane.
The solutions surrounding cells must have
the same osmotic pressure.
Otherwise, water will either leave the cell,
dehydrating （脱水）it ,
or enter the cell, causing it to burst（溶胀）.
Osmosis and Blood Cells
(a) A cell placed in an isotonic solution. The net movement of
water in and out of the cell is zero because the concentration of
solutes inside and outside the cell is the same. (5%C6H12O6)
(b) In a hypertonic solution, the concentration of solutes
outside the cell is greater than that inside. There is a net flow
of water out of the cell, causing the cell to dehydrate, shrink,
and perhaps die. (50% C6H12O6)
(c) In a hypotonic
水、电解质紊乱
solution, the
Isotonic
Hypertonic
Hypotonic
concentration of solutes
outside of the cell is less
than that inside. There is
a net flow of water into
the cell, causing the cell
to swell and perhaps to
burst. (1 % C6H12O6)
1-4.7 Osmolarity（渗透物质的量浓度）
Osmolarity （osmol/L or Osm/L).
is the measure of solute concentration,
defined as the number of osmoles (Osm)
of solute per liter of solution
渗量浓度 __指1L溶液中能产生渗透效应的各种溶质
微粒（分子或离子）的总物质的量。
1-4.7 Osmolarity
number of particles
• osmolarity = molarity×------------------------- = molarity × i
molecule of solute
the unit of osmolarity is the Osm/L
• For nonionizable solute: Osm/L ≈ mol/L ,
but for the electrolyte:
Osm/L ≈ mol/L × i
•For example: 1 mole of glucose dissolved in 1 litre
of water has an osmolarity of 1 osmole (Osm/L ).
If 1 mole of another sugar, such as sucrose（蔗糖）
were added to the same litre of water, the osmolarity
would be 1 Osm/L.
For example:
If 1 mole of NaCl were dissolved in 1 litre of water
it would produce a 1 mol/LNaCl solution with an
osmolarity 2 osm/L because NaCl dissociates into
Na+ and Cl- (two particles)
in solution.
Na2SO4
i=3
For dilute solutions, osmolarity is expressed in
milliosmols per liter (m Osm/L).
• What is the osmolarity of a 0.9% NaCl solution?
osmolarity = molarity × i
1000
= 0.9%×----------------- ×2 = 0.308 Osm/L
100×M(58.5)
( 308mOsm/L)
•Body fluids have an osmolarity of about 300 mOsm/L.
(280-320 mOsm/L)
• What is the osmolarity of a 5% glucose
solution?
Solution:
• Glucose is a nonelectrolyte;
number of particles
osmolarity = molarity ×------------------------- = molarity × i
molecule of solute
1000
=5%×----------------- × 1 = 0.277 Osm/L
100×M(180)
= 277mOsm/L
1-4.8 Crystalloid Osmotic Pressure and
Colloidal Osmotic Pressure
• Crystalloid Osmotic Pressure (772KPa)
by NaCl, NaHCO3, glucose,0.75% regulate
balance of fluid and electrolyte on the two side of
cell wall
Colloidal Osmotic Pressure (2.93~4.00KPa)
by large molecular colloidal substances
(Protein),7% regulate balance of fluid and
electrolyte on the two side of blood capillary wall.
水、电解质紊乱
（Interstitial fluid）
fluid）
（Plasma）
（ICF）
（ECF）
ECF）
Crystalloid Osmotic Pressure
If lack of water in the body, the outside fluids of
cells become hypertonic, can lead to dehydratio
If water Crystalloid
intake is too
much,Pressur
the outside fluids of cells
Osmotic
?
becomeColloidal
hypotonic,
can lead
to hemolysis,
Osmotic
Pressure
水、电解质紊乱
（Interstitial fluid）
fluid）
（Plasma）
（ICF）
（ECF）
ECF）
If the protein in plasma become less because some
disease, Colloidal Osmotic Pressure become
less,small crystal molecules osmosis to the outside
of blood capillary wall,so the edema（水肿） occur
•
edema occur
透析是指溶质通过半透膜，从高浓度溶液向低浓度方向运动。
Dialysis
血液透析包括溶质的移动和水的移动，即血液和透析液在透析器（人工肾）
• Process of cleaning blood
内借半透膜接触和浓度梯度进行物质交换，使血液中的代谢废物和过多的电
解质向透析液移动，透析液中的钙离子、碱基等向血液中移动。
Process of cleaning blood
A solution, called the dialysate（ 透 析 液 ） , circulates
outside of the cellophane tube. This dialysate is very
carefully prepared not only to be isotonic with blood but
also to have the same concentrations of all the essential
substances that should be left in solution in the blood.
When these concentrations match, the rate at which such
solutes migrate(迁移) out of the blood equals the rate at
which they return. In this way several key equilibria are
maintained, and there is no net removal of essential
components.