Wednesday, February 13, 2019

Intensive Property Definition

Intensive properties and extensive both are class of physical properties, the intensive property is those properties that do not change as the size of substance changes. It is a bulk property, which implies it is a physical property that isn't reliant on the mass or size, it depends only on the type of matter. On the contrary, an extensive property is that which depends on the size of the sample.
Examples of intensive properties include:
Boiling Point, Chemical Potential, Color, Concentration, Density, Hardness, Molality, Pressure, Refractive Index, Specific Gravity, Specific Heat, Specific Volume, Temperature.


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Extensive Property Definition

The physical properties of the substance have different properties; they are intensive and extensive properties. An extensive property is a property of matter that changes in the quantity of the substance in sample changes, without any chemical change an extensive property can be seen and measured. various properties of the matter rely on the sample size, while others do not. The mass of an item is the calculated quantity of matter that an item contains. A small sample of a certain type of substance would have a small mass, whereas a larger sample would have more mass.
Some examples of extensive property are mass, length, volume, size, weight, and charge.
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Examples of Physical Changes

The physical changes are not similar to chemical changes; physical changes include stages of energy and matter. Physical changes take place while the substances or matter are mixed but do not react chemically. No new matter is formed during a physical change, however, the color, shape, and size of the substance can change.
Here are some examples of physical changes:
  • Alcohol vaporizes on your hands
  • Boiling of water
  • Breaking a bottle
  • Breaking a glass
  • Bursting of crackers
  • Butter melts when warm
  • Casting silver in a mold
  • Chopping of any fruits
  • Crimp paper bag
  • Crushing of any object
  • Dissolving a solute in Solvent
  • Dissolving of sugar in a solvent
  • Evaporates of water from the ocean surface
  • Evaporating of alcohol
  • Expansion of metal by heating
  • Make a shape from the clay
  • Melting of an ice cube
  • Mixing flour, sugar, and salt
  • Mixing of oil and water
  • Ripening of Fruits
  • Ripening of Fruits
  • Rusting
  • Solidification of water by freezing
  • Sublimation of dry ice
  • Wood Chopping

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Examples of Chemical Changes

The Chemical changes are different from physical changes, A chemical change is a change of matter in the other, new matter with different properties and formed one or additional new substances; it is also called as chemical reactions.
One or more matter, sometimes, react with each other or with substances that are readily obtainable in the environment. As a result, new substances are formed are called chemical changes. In a chemical change, the molecular structure of a substance changes completely and creates a new substance.
There are three types of chemical changes such as biochemical, inorganic and biological changes. Here are some examples of chemical Changes:
  • A match is lit
  • Baking a cake
  • Boiling an egg
  • Bread becomes toast
  • Burning of paper
  • Burning wood
  • Decomposition of waste
  • Digestion of food
  • Electroplating a metal
  • Heating the sugar to make caramel
  • Lightening a matchstick
  • Milk going sour
  • Mixing acid and base
  • Rotting of fruits
  • Rusting of iron
  • The explosion of fireworks
  • The reaction between the salts and acids
  • Taking an antacid to settle your stomach


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Examples of physical properties

A physical property is described by matter that can be observed and estimated without altering the identity of a substance. It can change the arrangement of the matter, but it cannot change the structure of a substance if the chemical changes occur then it is called the chemical properties.
Here are some examples of physical properties:
  • Color
  • Boiling point
  • Compressibility
  • Conductivity
  • Density
  • Density
  • Ductility
  • Elasticity
  • Electrical charge
  • Freezing point
  • Hardness
  • Luminescence
  • Luster
  • Malleability
  • Mass
  • Melting point
  • Odor
  • Opacity
  • Permeability
  • Pressure
  • Reflectivity
  • Solubility
  • Strength
  • Temperature
  • Viscosity
  • Volume

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Examples of Chemical Properties

Chemical properties can be recognized only by changing the chemical identification of a substance, and are dissimilar from the physical properties, which can be seen by touching or observing the sample.
Here are some examples of chemical properties:
  • Toxicity
  • Chemical Stability
  • Solubility
  • Flammability
  • Possible chemical bonds
  • Oxidation Number
  • The heat of combustion
  • The degree of ionization
  • Electronegativity
  • Acidity/basicity
Uses of Chemical Properties:
Scientists use chemical properties to estimate whether any sample will participate in the chemical reaction or not. Chemical properties can be used to categorize the compounds and discover applications for them. Understanding the chemical properties of a substance assists in its separation, purification from other chemicals.
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What are Chemical Properties

A chemical property is a property of a matter that is seen when a substance passes through a chemical change. A chemical change is a kind of change which identifies the substance because of the breakdown and formation of new chemical bonds.
OR
Chemical properties are that can only be observed or calculated while the substance completely passes through the change to become a different kind of substance. The difference between physical and chemical property is straight unless the phase of the material is considered.
Here are some examples of chemical properties:
Enthalpy of formation, Toxicity, Types of chemical bonds that will form, Heat of Combustion, Flammability, Solubility, Chemical stability, Reactivity with other chemicals etc.

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What are Physical Properties

A physical property is characteristic of substances which can be measured and observed without altering or changing its chemical identity of a matter. The measurement of physical property can change the arrangement of substance, but it cannot change the molecular structure. In simple words, in physical properties could involve the physical changes, but not involve the chemical changes. If there is a chemical change or reaction, then it is called the chemical properties.
The physical properties have two classes, intensive and extensive properties. An intensive property relies on the quantity of the substance; this is regardless of how much substance exists. The melting point and density are examples of intensive properties. On the other hand, the extensive property relies on the size of the sample. Shape, mass, and volume are examples of extensive properties.
Here are some examples of physical properties:
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Monday, February 11, 2019

Difference between Osmolarity and Osmolality

Osmolality and Osmolarity both are the units of measurement. The number of osmoles of solute in a kilogram of solvent is an osmolality, whereas the number of osmoles in a liter of solution is an Osmolarity.
Osmotic pressure is the pressure that is necessary to avoid osmosis and it is that concerns liquid, Osmolarity, and osmolality are associated with the osmotic pressure, both are used to calculate the osmotic pressure in terms of osmoles, it is a number of moles in a compound which contributes to osmotic pressure.
The principle difference among osmolarity and osmolality is that osmolarity is calculating the solution volume, while the osmosis is measured considering the solution mass.
Here are some of the difference between osmolarity and osmolality.

Osmolarity
Osmolality
The concentration of the solution is expressed in the form of osmoles of solute particles per liter are called as osmolarity
Osmolality is the concentration of the solution articulated as the total number of solute particles per kilogram
The osmolarity is calculating by considering the amount of solution
The osmolality is calculating by considering the mass of the solution
The unit of osmolarity is mol/L
The unit of osmolality is osmol/L
The osmolarity relies on the temperature and pressure
The osmolality don’t rely on the temperature and pressures



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Difference between Osmotic Pressure and Osmotic Potential

To prevent osmosis from occurring, the pressure that is applied against the semi-permeable called as osmotic pressure. While the osmotic potential is the concentrated solutions concealed pressure that turns out to be real, just as the solution is separated from water by utilization of a semi-permeable membrane.
Here are some of the difference between osmotic pressure and osmotic potential.

Osmotic Pressure
Osmotic Potential
It has been expressed in bars with a positive sign.
It has been expressed in bars with a negative sign.
The value of osmotic pressure increases with the increase in the solute particle concentration.
If the negative value is high of osmotic potential it means the concentration of solute particles.
If both solutions with dissimilar osmotic concentrations are separated by a semicircular membrane, after that the molecules go in the direction of a more osmotic pressure solution from the low osmotic pressure solution.
If both solutions with dissimilar osmotic concentrations are separated by a semiconductor membrane, after that the molecules go in the direction of a more osmotic pressure solution to the low osmotic pressure solution.
The Pressure which is created in an osmotic system because of the entrance of water.
Due to the presence of solute particles, the free energy of water is reduced.
This is developed in a closed system.
This is developing into an open or closed system.
The value of osmotic pressure is positive.
The value of osmotic potential is negative.



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The similarity between Diffusion and Osmosis

Diffusion:
Diffusion is a significant method by which small molecules pass across the cell membrane. This is the process in which the molecules go into areas with a high concentration from low concentration areas.
Osmosis:
Osmosis is the diffusion of a solvent such as water molecules, which occurs in the area of high solute concentration from the area of low solute concentration.
Similarities:
  • The similarity between osmosis and diffusion is that they both equal the concentration of two solutions in the membrane.
  • Both are passive processes.
  • Diffusion and osmosis happen when the molecules or substance is present in the liquid.
  • Both are reliant on concentration.
  • Both work simultaneously to move solvents or water molecules.
  • Both go through an area with high concentration to the areas of low concentration through the permeable membrane.
  • The result of both processes is an equation of the solution
  • Both diffusion and osmosis processes do not require energy.
  • Both are happening in living as well as non-living.

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Difference between osmosis and reverse osmosis

Osmosis and reverse osmosis both are techniques of water movement through a semi-permeable membrane. The semi-permeable film can be a kind of synthetic or biological membrane, which enables just certain ions or particles (molecules) to go through it by diffusion.
The principle difference among osmosis and reverse osmosis is that the osmosis is the water molecule diffusion from high water potential to lower water potential over a semi-permeable membrane, though the reverse osmosis is the diffusion of water particles over a semi-permeable membrane against the potential gradient. In addition, osmosis is a natural process, whereas reverse osmosis is an artificial process.
Here are some of the difference between osmosis and reverse osmosis.
Osmosis
Reverse osmosis
Osmosis is a kind of diffusion where the water molecules movement takes place from the area of high to lower water potential
The Reverse osmosis process in which water is purified by solutes through the semi-permeable membrane
Happens without the need for an energy
Energy is required to supply pressure
Happens from high to low water concentration
As the name reverse osmosis, the direction is the opposite of the osmosis. Happens against the concentration gradient
Occurring naturally
Applied commercial
Osmotic pressure works naturally during osmosis
More pressure than the naturally occurring pressure is applied in reverse osmosis



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Advantages and Disadvantages of Reverse Osmosis

Reverse osmosis or RO is the water or solvent separation technique used for the remove particles, molecules, and also maintained the TDS of water. It uses a filter or semi-permeable membrane, with pressure, the water is pushed from the membrane, which puts the impurities back and the cleaner allows the water to flow.
Here are some of the advantages and disadvantages of reverse osmosis (RO).
Advantages of Reverse Osmosis:
  • It keeps you away from water-related diseases.
  • Reverse osmosis is the best method to soften the water.
  • It has the ability to effectively eliminate many dissolved substances.
  • Any ion particles cannot be permitted to enter through a semi-permeable membrane.
  • RO technology has the capability to remove the total dissolved solids (TDS) along with chlorine taste and odor.
  • RO provides good taste to water.
  • RO does not put any chemicals in the water.
  • Maintenance of the RO system is simple.
  • Take minimum area to install the household RO system.
Disadvantages of Reverse Osmosis
  • The main disadvantage of RO is a high amount of water which is wasted from the process.
  • The whole process requires a lot of energy.
  • This is a costly process and the output is slow.
  • Due to decay, periodic replacement of the RO membrane is required so maintenance cost is more.



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What is reverse osmosis

Reverse osmosis is also referred to as RO, it is a technique of filtration that is utilized to expel particles, molecules, and ions from a solution or water under the pressure to the solvent or water on one side of a barrier or a semi-permeable membrane. Large solute (molecules) cannot pass the membrane or barrier, that's why they remain on one side. Solvent (Water) can pass the barrier or membrane. The outcome is that the molecules are more concentrated on one side of the membrane, as the other side’s solute molecules are diluted. 
OR
If there are impurities in water, then water flows through a membrane, but what is the other way to go? It has been found that by providing adequate pressure to overcome osmotic pressure, it is possible to force contaminated water through the same barrier this thought called reverse osmosis.


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What is osmotic pressure

To stop the water diffusing through the osmosis barrier, Osmotic pressure can be thought of as essential pressure. OR it refers to how difficult it would be to push water through a membrane to diffuse on the other side. The osmotic pressure is determined by solute concentration, water will hard to diffuse to the area of high concentrations of solutes in the low concentration area. In fact, osmotic pressure is not the desire of water, but there is an extension of the natural law that all matter will be distributed randomly over time. When the substance concentration is dissimilar in two areas and areas are interacting with each other, then due to the random motion of the particles, the matter or substance will cause the diffuse of the entire area until it becomes equal.

Through a semi-porous film, osmosis is the specific diffusion of water. So on account of osmosis, the solutes can't move since they can't go through the membrane. Be that as it may, the water can move, and it does go or pass through the film to a higher solute concentration area. It can cause the entire volume of a water change on each side of the membrane. The membrane side with additional solutes may finish up with considerably more water; it can cause problems like cell dehydration or burst.


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