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Why does the phenomenon of calcium hydroxide saturated solution become turbid rather than crystallized when the temperature is raised
The supersaturated solution of calcium hydroxide is a turbid solution in which the turbid matter is indeed crystallized. But not all the crystals in water are as crystalline as sodium hydroxide. In the case of copper sulfate, the crystals are flocculated precipitates. This is determined by the different size of the crystalline particles and the different geometric shapes.
The supersaturated solution of calcium hydroxide is a turbid solution in which the turbid matter is indeed crystallized. However, not all the crystals in water are as crystalline as sodium hydroxide. In the case of copper sulfate, the crystals are floc-like precipitates. This is determined by the size of the crystalline particles and the geometry of the crystals.
20°C saturated salt solution 100g and 200g, each evaporating 10 water, how much crystal is precipitated Salt solubility is 36 g at 20°C
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RELATED INFORMATIONS
- 1. At 20°C,5 g of water is evaporated from 200 g of saturated sodium chloride solution, and how many g of sodium chloride crystals are precipitated?
- 2. How does the grain size affect the mechanical properties of the material?
- 3. About Crystals and Crystals What is the point in the chemical formula? I haven't learned anything about crystals. Can you tell me more about them? Such as basic cop carbonate and copper carbonate, copper hydroxide,
- 4. Saturated solution. Crystallization occurs when the solution is heated or cooled.
- 5. Is it certain that crystals will precipitate when the saturated solution cools down? Must the solution of the precipitated crystals be a saturated solution of the solute at this temperature? Tell me the reason. Is it certain that crystals will precipitate when the saturated solution cools down? Must crystals precipitate when saturated solution cools down? Must the solution of the precipitated crystals be a saturated solution of the solute at this temperature? Tell me the reason. Must crystals precipitate when saturated solution cools down?
- 6. How do you know if the solution is cooled or heated?
- 7. The crystals precipitated from saturated solution must be unsaturated solution? What happens when saturated solution cools down? What happens when the unsaturated solution heats up? When will crystals precipitate? Does the saturated solution precipitate crystals when heated? Crystals precipitated from saturated solution must be unsaturated solution? What happens when saturated solution cools down? What happens when the unsaturated solution heats up? When will crystals precipitate? Does the saturated solution precipitate crystals when heated?
- 8. Why does crystal precipitate in the evaporating dish and a small amount of liquid remain?
- 9. Similarities and differences between stopping heating when a large amount of crystals are precipitated during evaporation and... Such as title Similarities and differences between stopping heating when a large number of crystals are precipitated during evaporation and... Such as title
- 10. Is it certain that crystals will precipitate from saturated solution? What is the relationship between the quality of precipitated crystals and solubility?
- 11. In industry, how to precipitate copper sulfate crystal in low concentration copper sulfate solution (except evaporation method)? Evaporation must be too expensive, is there any most economical way? Does anyone know what methods are used in industry? How much electricity is required for evaporation of 1 kg of water?
- 12. Operation of extracting sodium chloride crystals from a sodium chloride solution containing a small amount of potassium nitrate Extraction of Sodium Chloride Crystals from a Sodium Chloride Solution Containing amount of potassium nitrate
- 13. What method is used to separate and purify sodium chloride crystals from a mixture of sodium chloride and potassium nitrate (small amount)? If there are 10g sodium chloride crystals in the original mixture, will the mass of these crystals be less than 10g after purification?
- 14. How to precipitate potassium nitrate crystals from a mixed solution of potassium nitrate and sodium chloride in a mass ratio of 1:1?
- 15. After a certain amount of M substance solution is evaporated at a certain temperature by 15 g of water,2 g of crystal is precipitated, another 15 g of water is evaporated, and another 5 g of crystal is precipitated. If another 15 g of water is evaporated, the mass of precipitated crystal is () A.2 g B.5 g C.8 g D. Inability to judge
- 16. If the temperature is not changed, when 10g of water is evaporated,4g of A crystal (excluding crystal water) will be precipitated. When 10g of water is evaporated again,6g of A crystal will be precipitated.
- 17. Does evaporative crystallization mean increasing the temperature or evaporating the solvent? NaCL is crystallized by evaporation and KNO3 is crystallized by cooling. What about Ca [OH ]2?
- 18. At t°C, the NaOH solution with a% mass fraction of solute was evaporated off mg of water and then recovered to the original temperature. At t.degree. C., the solution of NaOH with a mass fraction of solute was evaporated off mg of water and recovered to the original temperature, and the saturated solution of NaOH with a mass fraction of 2a, and the mass of the original solution was obtained At t°C, the NaOH solution with a% mass fraction of solute is evaporated off mg of water and then recovered to the original temperature. At t.degree. C., the solution of NaOH with a mass fraction of solute was evaporated off mg of water and recovered to the original temperature, and the saturated solution of NaOH with a mass fraction of 2a, and the mass of the original solution was obtained
- 19. A solution of sodium chloride at 80°C,20 g of water evaporated at constant temperature,2 g of crystals precipitated,20 g of water evaporated at constant temperature,4 g of crystals precipitated, and how many g of crystals precipitated if 35 g of water evaporated at constant temperature? At 20°C, the solubility of sodium chloride is 31 g. At present,500 g of 20% sodium chloride solution is available. If 5 g of sodium chloride crystal will be precipitated at this temperature, what is the mass of water to be evaporated?
- 20. 100 G of the solution of the substance A at 50 degrees centigrade was divided into two parts, one part evaporated at constant temperature 10 g of water with 4 g of crystals precipitated, the other part evaporated 20 g of crystals precipitated 20 g, Solubility in 50 degrees Celsius. Must have a process, thank you very much!