100 points possible Colligative Properties and Life examples Practical applications of colligative properties in order t
Posted: Mon Jul 11, 2022 1:39 pm
100 points possible
Colligative Properties and Life examples
Practical applications of colligative properties
in order to receive full credit you are required to follow these instructions1) Original post (Your own answer your own post) should be a minimum of 1 paragraph (6-7 sentences in good details) 50 points2) Respond to 2 classmates post it should be minimum of 1 paragraph (4-5 sentences) -2×25 points 3) Be sure to proofread your posts for correct grammar, spelling, punctuation, and appropriate use of capitalization 4) Make sure your post is NOT A COPY OF SOMEONE ELSE'S POST IF IT IS THEN ITS PLAGARISM
(I will add photos of classmate so that you can answer to question no 2 which is to respond to their post please make sure everything is been made sure and looks good please
just please make sure that everything is answered all the points
O Charlie Neira Jul 1, 2022 In the kitchen we can apply practical applications of colligative properties. When cooking rice, I use a pressure cooker, which demonstrates the elevation in the boiling point of water by adding water into the cooker with the rice and putting the lid on it. As the pressure builds up inside, the boiling point of the water is increased, cooking the rice. The vapor pressure altering due to a solute being introduced to the solvent makes it a colligative property. With that being said, in the winter time up north, the temperatures tend to reach lows that can cause snow, meaning frozen water, so vehicles need 50/50 antifreeze and water put into their radiators to decrease water's freezing point, so that the motors don't lock up and can properly run in the cold weather. Edited by Charlie Neira on Jul 8 at 11:41pm Reply Ava Romero Thursday To add to your cooking example, adding salt to water increases the number of solute particles and changes many of water's colligative properties. One property affected is water's boiling point as you have mentioned. By adding salt and increasing the solutes concentration, the water will boil at a higher temperature than it normally would without the additional solute particles. The water's boiling point will continue to increase with the addition of more salt. Water boils when its molecules overcome the vapor air pressure to go undergo the needed phase transition. When salt is added, the water needs to overcome the additional pressure the salt particles are exerting on the air, meaning more energy is needed to make the phase transition. Reply
O James Giordano Thursday Colligative properties refer to the ratio between the number of solute particles compared to the number of solvent particles and not to the actual chemicals. Real world applications are everywhere including, salting icy roads. The salt decreases the melting point of ice causing roads to be less slick and more safe to drive on, this is called freezing point depression. The more impurities (salt etc..) the lower the freezing or melting point. Another example would be with osmotic pressure in medicine. Intravenous solutions must be isosmotic or isotonic before being administered into the blood stream in order to have an equilibrium with bodily fluids, the same osmotic pressure. Without this cells can lose water and shrivel or be flooded with water and burst, both are dangerous to the body. Other colligative properties include boiling point elevation and vapor pressure lowering, both widely used in cooking and some other everyday activities. Reply Ava Romero Thursday Salting icy roads works to lower the freezing point by disrupting the ordering of the hydrogen bonds present in ice. When water freezes, its bonds become more orderly, and thus the intermolecular forces become more stable and resistant to change. The addition of salt being dissolved and added to the solute, interferes with the order and stable intermolecular relationships. With this disruption, more energy will have to be continually removed in order to maintain the water in its solid, orderly state. Thus, its freezing point is lowered. The ice will melt more quickly due to it requiring less energy than what would be required to maintain its solid state. Reply Logan Sexton 2
O Ava Romero Thursday Colligative properties are those that depend on the concentration of solute particles but are not affected by the identity or nature of the solute particles themselves. A very common and important property is osmotic pressure. In biology, I learned about hypertonic, isotonic, and hypotonic solutions in various different examples. One that would be important for anyone entering the medical field is why IV's of pure water cannot be given to patients. This is because relative to the cells of the body, the waters lack of solute particles would make it a hypotonic solution (and the body's cells would thus be relatively hypertonic). This difference in solute concentration would be devastating, leading to an influx of water into the body's cells via osmosis, causing the cells to swell and eventually burst, which could lead to the death of a patient. This is why the osmolarity of IVs are changed by increasing the solute concentration of pure water. Hence most every IV is a saline solution (a combination of water and salt). Changing nothing else about the solute except the number of saline particles, IVs can successfully be given to patients without worrying about a catastrophic difference in osmotic pressure. Reply 4
Colligative Properties and Life examples
Practical applications of colligative properties
in order to receive full credit you are required to follow these instructions1) Original post (Your own answer your own post) should be a minimum of 1 paragraph (6-7 sentences in good details) 50 points2) Respond to 2 classmates post it should be minimum of 1 paragraph (4-5 sentences) -2×25 points 3) Be sure to proofread your posts for correct grammar, spelling, punctuation, and appropriate use of capitalization 4) Make sure your post is NOT A COPY OF SOMEONE ELSE'S POST IF IT IS THEN ITS PLAGARISM
(I will add photos of classmate so that you can answer to question no 2 which is to respond to their post please make sure everything is been made sure and looks good please
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O Charlie Neira Jul 1, 2022 In the kitchen we can apply practical applications of colligative properties. When cooking rice, I use a pressure cooker, which demonstrates the elevation in the boiling point of water by adding water into the cooker with the rice and putting the lid on it. As the pressure builds up inside, the boiling point of the water is increased, cooking the rice. The vapor pressure altering due to a solute being introduced to the solvent makes it a colligative property. With that being said, in the winter time up north, the temperatures tend to reach lows that can cause snow, meaning frozen water, so vehicles need 50/50 antifreeze and water put into their radiators to decrease water's freezing point, so that the motors don't lock up and can properly run in the cold weather. Edited by Charlie Neira on Jul 8 at 11:41pm Reply Ava Romero Thursday To add to your cooking example, adding salt to water increases the number of solute particles and changes many of water's colligative properties. One property affected is water's boiling point as you have mentioned. By adding salt and increasing the solutes concentration, the water will boil at a higher temperature than it normally would without the additional solute particles. The water's boiling point will continue to increase with the addition of more salt. Water boils when its molecules overcome the vapor air pressure to go undergo the needed phase transition. When salt is added, the water needs to overcome the additional pressure the salt particles are exerting on the air, meaning more energy is needed to make the phase transition. Reply
O James Giordano Thursday Colligative properties refer to the ratio between the number of solute particles compared to the number of solvent particles and not to the actual chemicals. Real world applications are everywhere including, salting icy roads. The salt decreases the melting point of ice causing roads to be less slick and more safe to drive on, this is called freezing point depression. The more impurities (salt etc..) the lower the freezing or melting point. Another example would be with osmotic pressure in medicine. Intravenous solutions must be isosmotic or isotonic before being administered into the blood stream in order to have an equilibrium with bodily fluids, the same osmotic pressure. Without this cells can lose water and shrivel or be flooded with water and burst, both are dangerous to the body. Other colligative properties include boiling point elevation and vapor pressure lowering, both widely used in cooking and some other everyday activities. Reply Ava Romero Thursday Salting icy roads works to lower the freezing point by disrupting the ordering of the hydrogen bonds present in ice. When water freezes, its bonds become more orderly, and thus the intermolecular forces become more stable and resistant to change. The addition of salt being dissolved and added to the solute, interferes with the order and stable intermolecular relationships. With this disruption, more energy will have to be continually removed in order to maintain the water in its solid, orderly state. Thus, its freezing point is lowered. The ice will melt more quickly due to it requiring less energy than what would be required to maintain its solid state. Reply Logan Sexton 2
O Ava Romero Thursday Colligative properties are those that depend on the concentration of solute particles but are not affected by the identity or nature of the solute particles themselves. A very common and important property is osmotic pressure. In biology, I learned about hypertonic, isotonic, and hypotonic solutions in various different examples. One that would be important for anyone entering the medical field is why IV's of pure water cannot be given to patients. This is because relative to the cells of the body, the waters lack of solute particles would make it a hypotonic solution (and the body's cells would thus be relatively hypertonic). This difference in solute concentration would be devastating, leading to an influx of water into the body's cells via osmosis, causing the cells to swell and eventually burst, which could lead to the death of a patient. This is why the osmolarity of IVs are changed by increasing the solute concentration of pure water. Hence most every IV is a saline solution (a combination of water and salt). Changing nothing else about the solute except the number of saline particles, IVs can successfully be given to patients without worrying about a catastrophic difference in osmotic pressure. Reply 4