Biochemistry deals with the study of chemistry of life and living processes. It is important for understanding basic biological functions, disease mechanisms, and conducting laboratory tests. A solution is a mixture of substances composed of a solute dissolved in a solvent. The concentration of solutions can be expressed as normal, molar, or percent solutions. Osmosis is the movement of solvent through a semipermeable membrane from lower to higher concentration. Diffusion is the movement of solute molecules from higher to lower concentration. Dialysis is a process used to remove waste and excess water from the blood, serving as an artificial replacement for lost kidney function.

1. Biochemistry
for
B.Sc.Nursing
Introduction
Definition, Scope
Solution & Its
Types
Osmosis Diffusion
Dialysis
NOTES TO PRINT

2. Definition, Scope & Importance of Biochemistry
in Health Science
 Biochemistry deals with the study of
chemistry of life and living process. The
name Biochemistry was introduced by Carl
Neuberg in 1903.
Scope
 The scope of biochemistry is as huge as life
itself. Every aspect of life birth, growth,
reproduction, age and death involves
biochemistry.

3. Importance of Biochemistry in Health Science
 To understand:
 Basic knowledge of Biochemistry and its
application in Medical science.
 The role of non-living matters for development,
growth and death of biological system.
 The role of biomolecules and their metabolism
for survival of life.
 And develop basic skill to conduct biochemical
and immunological laboratory test.
 The mechanism of developing disease.
 And analyze the problem developed during
analysis, understanding and controlling disease.

4. Solution & Its Types
 Solution is defined as mixture of substances
which is composed of two parts, solute &
solvent. The part which is dissolved is known
as solute and which dissolves the solute is
known as solvent.
 The relative concentration in solution is
expressed in several ways:
 Normal solution
 Molar solution
 Percent solution

5. Normal Solution:
 Normal solution is defined as the gram
equivalent weight of a substances dissolved
in 1000 ml of solvent. One gram of
equivalent weight of an element or
compound represents its capacity to replace
or combine 1 mole of hydrogen.

6. Equivalent Weight:
 The equivalent weight of an element is the number
of parts of it by weight, which combine with or
displace from a compound, 8 parts by weight of
oxygen or its equivalent i.e. 1.008 parts by which of
hydrogen or 35.5 parts by weight of chlorine.
 Equivalent Weight of a element = Atomic weight / Valency
 Equivalent Weight of an acid = Molecular weight of acid /
Replaceable hydrogen
 Equivalent Weight of a base = Molecular weight of base / No. of
hydroxyl group
 Equivalent Weight of a salt =Molecular weight of salt / No. of
metal ions or radicals

7. Element
Symbol Atomic Weight Valency
Equivalent
Weight
Carbon C 12.010 4 3.003
Chlorine Cl 35.457 1 35.457
Hydrogen H 1.008 1 1.008
Nitrogen N 14.008 3 4.669
Oxygen O 16.000 2 8.000
Phosphorus P 30.975 3 10.325
Potassium K 39.100 1 39.100
Silver Ag 107.880 1 107.880
Sodium Na 22.997 1 22.997
Sulphor S 32.006 2 16.003
Acid Formulae Molecular Weight
Replaceable
Hydrogen
Equivalent
Weight
Sulphuric Acid H2SO4 98.082 2 49.041
Hydrochloric Acid HCl 36.468 1 36.468
Acetic Acid CH2COOH 60.08 1 60.08
Alkali Formulae Molecular Weight Hydroxyl Group
Equivalent
Weight
Sodium Hydroxide NaOH 40.005 1 40.005
Calcium Hydroxide Ca(OH)2 91.104 2 45.552
Salt Formulae Molecular Weight No. of cations
Equivalent
Weight
Sodium Chloride NaCl 58.454 1 58.454
Sodium Carbonate Na2CO3 106.004 2 53.002

8. Molar Solution:
 Molar solution is defined as the gram
molecular weight of a substances dissolved in
1000 ml of solvent. One gram of molecular
weight of an element or compound is
calculated by adding together the atomic
weight of various atoms in the compound.

9. Percent Solution:
 Percent solution is defined as a part of a
solute dissolved in 100 parts of a final
solution. The most frequently used in weight
per volume (w/v). e.g. 9% saline (9 gram
/100 ml).
 There are 3 ways of expressing % solution:
 W/W (Weight by Weight)
 W/V (Weight by Volume)
 V/V (Volume by Volume)

10. Osmosis
 Osmosis is defined as the movement of solvent through a semi permeable
membrane. The movement of solvent takes place from the lower
concentration to a higher concentration solution when it is separated by
semi permeable membrane. It is due to osmotic pressure.
 Osmotic pressure is defined as the excess pressure that must be applied
to a solution to prevent the passage of solvent into the solution on
separation with semi permeable membrane.
 Application of Osmosis:
 Blood volume & fluid balance
 RBC and fragility
 Transfusion
 Osmotic dieresis
 Edema due to hypoalbuminemia
 Cerebral edema
 Irrigation of wounds
 Action of purgatives

11. Diffusion
 Diffusion is defined as the movement of solute
molecule from higher concentration to lower
concentration. The smaller particles diffuse
faster than the larger molecules hence gas
diffuses more rapidly than liquids. Diffusion
occurs in gases as well as in colloidal solution.
 Application of diffusion:
 Gases exchanges in lungs
 Absorption of nutrients from Gastero Intestinal
tracts.
 Passes of waste products in the renal tubules.

12. Dialysis
 Dialysis is a process for removing waste and
excess water from the blood.
 Primarily as an artificial replacement for lost
kidney function.
 Dialysis may be used for those with an acute
disturbance in kidney function or progressive but
chronically worsening kidney function (chronic
kidney disease).
 The latter form may develop over months or
years, but in contrast to acute kidney injury is
not usually reversible, and dialysis is regarded as
a "holding measure" until a kidney transplant can
be performed, or sometimes as the only
supportive measure in those for whom a
transplant would be inappropriate.