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Henry’s law
- Henry’s Law establishes aquantitative relation betweenpressure and solubility of a gasin a solvent.
- This law is for gas-liquid solution.
- According to the law at a constant temperature, thesolubility of a gas in a liquid is directly proportional to thepressure of the gas.
- It can also be stated as - The partial pressure of the gas in vapour phase (p) is proportional to the mole fraction of the gas (x) in the solution.
Posted by Tarun Ch 6 years ago
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Yogita Ingle 6 years ago
Addition of a common ion to a slightly soluble salt solution will add up to the concentration of the common ion. According to Le Chatelier's Principle that will place a stress upon the slightly soluble salt equilibria. Thus, the equilibrium will shift so as to undo the stress of added common ion.
Posted by Tarun Ch 6 years ago
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Azeotropes
- Azeotropes are binary mixturespossessing the same synthesis in fluid, vapor stage and boiling stage at a steady temperature.
- The components of azeotropic mixtures are separated by fractional distillation.
- Azeotropes can be broadly categorized into two types-
- Minimum boiling azeotrope
The solutions showing positive deviation from Raoult’s law. For instance, solution of ethanol and water on fractional distillation results in a solution containing approximately 95% by volume of ethanol.
- Maximum boiling azeotrope.
The solutions showing negative deviation from Raoult’s law. For instance, solution of nitric acid and water has the approximate arrangement, 68% nitric corrosive and 32% water by mass, with a breaking point of 393.5 K.
Posted by Tarun Ch 6 years ago
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Meghna Thapar 6 years ago
When blood cells are placed in hypertonic solution, water will move out of these cells into the surrounding solution via the process of osmosis. This will cause the blood cells to shrink /shrivel. If the cell was placed in isotonic solution, it would be in equilibrium and nothing would happen.
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Yogita Ingle 6 years ago
The Van’t Hoff factor offers insight on the effect of solutes on the colligative properties of solutions. It is denoted by the symbol ‘i’. The Van’t Hoff factor can be defined as the ratio of the concentration of particles formed when a substance is dissolved to the concentration of the substance by mass.
The extent to which a substance associates or dissociates in a solution is described by the Van’t Hoff factor. For example, when a non-electrolytic substance is dissolved in water, the value of i is generally 1. However, when an ionic compound forms a solution in water, the value of i is equal to the total number of ions present in one formula unit of the substance.
For example, the Van’t Hoff factor of CaCl2 is ideally 3, since it dissociates into one Ca2+ ion and two Cl– ions. However, some of these ions associate with each other in the solution, leading to a decrease in the total number of particles in the solution.
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The Van’t Hoff factor offers insight on the effect of solutes on the colligative properties of solutions. It is denoted by the symbol ‘i’. The Van’t Hoff factor can be defined as the ratio of the concentration of particles formed when a substance is dissolved to the concentration of the substance by mass.
The extent to which a substance associates or dissociates in a solution is described by the Van’t Hoff factor. For example, when a non-electrolytic substance is dissolved in water, the value of i is generally 1. However, when an ionic compound forms a solution in water, the value of i is equal to the total number of ions present in one formula unit of the substance.
For example, the Van’t Hoff factor of CaCl2 is ideally 3, since it dissociates into one Ca2+ ion and two Cl– ions. However, some of these ions associate with each other in the solution, leading to a decrease in the total number of particles in the solution.
This factor is named after the Dutch physical chemist Jacobus Henricus Van’t Hoff, who won the first Nobel Prize in chemistry. It is important to note that the measured value of the Van’t Hoff factor for electrolytic solutions is generally lower than the predicted value (due to the pairing of ions). The greater the charge on the ions, the greater the deviation.
Effects of Association/Dissociation
Association is the joining of two or more particles to form one entity.
An example of the association of two particles is the dimerization of carboxylic acids when dissolved in benzene.
Dissociation refers to the splitting of a molecule into multiple ionic entities.
For example, sodium chloride (NaCl) dissociates into Na+ and Cl– ions when dissolved in water.
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Concentration of solution
- Concentration of a solution is the measure of the composition of a solution.
- A solution with relatively very large quantity of solute is called concentrated solution.
- A solution with relatively very small quantity of solute is called a dilute solution.
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Pawni Chaudhary 5 years, 5 months ago
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