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Colligative Disaster Attitude Do you know that in cold weather countries, salt is often spilled on the road when it snows? The purpose is to prevent the road from being hard and slippery due to the formed ice. Why can salt prevent the formation of ice? Or why is water longer to boil when we add sugar to it? Well, all of this is related to the colligative disorder.
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What is a colligative? What are the colligative and how is it useful in life? Let's watch this video until the end. The colligative of a solution is a solution that only depends on the number of dissolved particles, not on the type of the substance. It means the more particles of substance are dissolved in the solution, the greater the impact on certain solutions of the solution.
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However, it should be noted that electrolyte and non-electrolyte solubility have different effects even though the concentration is the same. Why is that? In non-electrolyte solubility such as sugar, its molecules are not divided into ions. Meanwhile, in electrolyte solubility such as salt,
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its molecule is classified as an N-Hatless ion and an Ion-Telman ion. Because the coagulation nature depends on the number of particles, electrolyte melting will have a greater impact because the number of particles is more because of ionization. To calculate this ionization effect, we use the Van Hoof factor with the formula as follows:
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For example, the salt molecule is perfectly saturated, so alpha = 1 From the interaction of ionization reactions, it can be known that the number of ions produced is 1 Na+ and 1 Cl- so n = 2 After being calculated with a formula, the Van Gogh factor is obtained, the salt solution is equal to 2
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Meanwhile, for non-electrolytic solvents such as sugar, the van hoff factor is not calculated or considered the same as 1. If compared, the effect of the salt solvent is twice as big as the sugar solvent.
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There are four types of colligative solubility, namely: - pressure decrease - point decrease - increase of the point of the stem - osmotic pressure Let's discuss one by one. First, we discuss the pressure decrease. Pression is the pressure produced by a substance's vapor when it is in balance with its liquid phase.
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The more steam on the surface of the liquid, the higher the pressure of the steam. Therefore, easier to evaporate liquid will have a higher pressure of steam. When we add a dissolved substance to the solvent, for example adding sugar to water, then the pressure of the sugar solution will be lower than the pressure of the solvent or the pressure of the water.
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This pressure drop is caused by the presence of sugar particles that prevent water particles from evaporating. The pressure drop can be determined by the solution between the pure dissolved steam pressure and the dissolved steam pressure. In addition, the pressure drop is also proportional to the pure dissolved steam pressure and the fraction of dissolved matter. Next, the freezing point drop.
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Have you ever seen a road in a snowy area that is sprinkled with salt? This is an example of an application of the drop of an ice point. When an substance is dissolved like salt, added to water, the melting point will be lower than water or lower than 0 ° C. This drop in the ice point is caused by the presence of salt particles that disturb water particles to form solid crystals.
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Thus, ice or snow formation on the road can be prevented because the solution will remain liquid, although the temperature is below 0 ° C. This freezing point decrease is compared to the remaining freezing point decrease in molal and solution molality. In addition to reducing the freezing point, the liquid can also increase the boiling point of the solution.
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When the concentration of the dissolved matter is higher, the point of boiling of the solution is also higher. For example, when we cook pasta and add salt to the water, the water will boil at a temperature higher than 100 degrees Celsius. Salt contained prevents the absorption of water, so it requires energy or a higher temperature to boil.
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This increase in the point of the seed is compared to the increase in the point of the seed molal and the molality of the solution. Finally, we will discuss osmotic pressure. Osmosis is the transfer of the solvent molecule through the semi-permeable membrane from a more liquid solution to a more dense solution. Osmotic pressure is the pressure needed to stop this osmosis process.
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Osmotic pressure is straight compared to the melting molarity and influenced by temperature. Well, that's a brief explanation of the melting colligative nature and each calculation of the formula. Why is it important to study this topic? Understanding the melting colligative nature turns out to be very useful in everyday life. For example, in the process of making traditional ice cream,
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salt is added to rock ice to make the temperature colder due to the decrease in freezing points. Another example is car radiator water added with Z-ethylene glycol so that it does not freeze in the cold season because the freezing point is lower.
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On the contrary, the addition of this substance also prevents the steam so that the temperature of the machine remains stable because the steam pressure becomes lower or the boiling point is higher. Other colligative properties are infusion liquid that is inserted into the blood vessel must be isotonic or have the same osmotic pressure as blood to keep the body safe.
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Now, let's try to answer the following questions: 1. Based on the data, it can be symbolized that the decrease in the freezing point 2. If the amount of the solvent is considered the same, then the solvent that has the highest steam pressure is? 3. The comparison of the osmotic pressure of the two solvents is?
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