explain why these three properties of water are important? melting and freezing cohesive and adhesive An excellent solvent Solution Water melting and freezing properties are important because these properties are main colligative properties useful to prepare polar biological & pharmaceutical products suitable to the internal human body environment The cohesive forces (cohesion) & adhesive forces of water molecules enable to acquire elastic tendency with considerable surface area promote solubility. This tendency is referred as surface tension. Surface tension of any fluid decreases with increasing temperature. This is due to existence of cohesive intermolecular forces between molecules of the fluid is reduced and it is based on the surrounding environment with adhesive intermolecular forces & viscosity of the fluid, molecular thermal activity at the liquid interface For example, water is a universal solvent and it has both polar because it has both positive charge (H+ or H3O+) and negative charge (OH-). This polarity enables water to make substances to dissolve in it as charged species. On the other hand, water molecules possess a higher attractive power to each other so that these forces are referred as cohesive forces responsible for “surface tension” phenomenon” and these attractions are predominantly due to hydrogen bonding. For instance, 2 to 3 drops of water between the cover slip is imparted adhesive forces (another example is capillary rise due to forces between glass and water in capillary tube) between the two glass cover slips result in adhesion instead of cohesion that potentially differentiate intermolecular forces between two different substances namely water and silicon. These intermolecular forces render glass surface as hydrophilic. These intermolecular forces are decreased as the temperature increases due to increase in molecular thermal activity of the fluid molecules ate the interface of water molecules. An excellent solvent Water is a universal polar solvent and it has hydrogen bonding associated with highest heat capacity and is referred as “specific heat capacity”. This specific heat is predominantly due to intermolecular and intermolecular hydrogen bonding. In nature on land when heat is absorbed result in breaking of hydrogen bonds specifically followed by production of heat. Normally ocean water cool little bit slower when compared to the land water because of more heat capacity. This sterile solvent has ability to dissolve a majority of biological products to prepare pharmaceutical products finally used as diluents in saline, injectables etc. Water properties and the biological importance of water: 1). Due of the presence of hydrogen bonds and strong intermolecular forces, water has high specific heat index. Specific heat capacity of water is defined as; the amount of heat (energy in joules) required for raise of temperature of water per unit mass by 10C. Our body temperature is maintained higher than the surroundin.

1. explain why these three properties of water are important?
melting and freezing
cohesive and adhesive
An excellent solvent
Solution
Water melting and freezing properties are important because these properties are main colligative
properties useful to prepare polar biological & pharmaceutical products suitable to the internal
human body environment
The cohesive forces (cohesion) & adhesive forces of water molecules enable to acquire elastic
tendency with considerable surface area promote solubility. This tendency is referred as surface
tension. Surface tension of any fluid decreases with increasing temperature. This is due to
existence of cohesive intermolecular forces between molecules of the fluid is reduced and it is
based on the surrounding environment with adhesive intermolecular forces & viscosity of the
fluid, molecular thermal activity at the liquid interface
For example, water is a universal solvent and it has both polar because it has both positive charge
(H+ or H3O+) and negative charge (OH-). This polarity enables water to make substances to
dissolve in it as charged species. On the other hand, water molecules possess a higher attractive
power to each other so that these forces are referred as cohesive forces responsible for “surface
tension” phenomenon” and these attractions are predominantly due to hydrogen bonding. For
instance, 2 to 3 drops of water between the cover slip is imparted adhesive forces (another
example is capillary rise due to forces between glass and water in capillary tube) between the
two glass cover slips result in adhesion instead of cohesion that potentially differentiate
intermolecular forces between two different substances namely water and silicon. These
intermolecular forces render glass surface as hydrophilic. These intermolecular forces are
decreased as the temperature increases due to increase in molecular thermal activity of the fluid
molecules ate the interface of water molecules.
An excellent solvent
Water is a universal polar solvent and it has hydrogen bonding associated with highest heat
capacity and is referred as “specific heat capacity”. This specific heat is predominantly due to
intermolecular and intermolecular hydrogen bonding. In nature on land when heat is absorbed

2. result in breaking of hydrogen bonds specifically followed by production of heat. Normally
ocean water cool little bit slower when compared to the land water because of more heat
capacity. This sterile solvent has ability to dissolve a majority of biological products to prepare
pharmaceutical products finally used as diluents in saline, injectables etc.
Water properties and the biological importance of water:
1). Due of the presence of hydrogen bonds and strong intermolecular forces, water has high
specific heat index. Specific heat capacity of water is defined as; the amount of heat (energy in
joules) required for raise of temperature of water per unit mass by 10C.
Our body temperature is maintained higher than the surrounding temperature. The heat of
vaporization of the water is higher (40.65 kJ/mol), this is due to the hydrogen bonds that connect
water molecules. So, due to the temperature difference, water escapes out and carry the body
heat (the specific heat capacity of the water is 5 times more than the sand). So, during the process
of vaporization of water, water releases heat into the environment and cool the body.
2). Because of the hydrogen bonding, water exhibits high surface tension. So, water molecules
on the surface are more strongly attracted to each other than to the air above. This is necessary
for the functioning of alveoli. The layer of moisture over the alveoli is necessary for the gaseous
exchange.
3). Due to the polar nature of water, water can dissolve inorganic salts that dissociate into ions in
the presence of water (like dissolves like). So, the blood can carry many of the water soluble
substances throughout the body. Water cannot dissolve nonpolar substances; they are dissolved
in non-polar solvents.
4). Plasma contains approximately 91% of water; this maintains the viscosity of the blood.