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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?
The first must be that saturated solution seems to be defined as such.
Supplemental problems, not necessarily. There seems to be the opposite solution. Sometimes the temperature solubility increases.
How to judge the amount of precipitated crystals after cooling the saturated solution? Always don't understand, there is always a problem:50°C 100 g of A, B and C solution respectively when cooling to 10°C what the order of the quality of the solution size, it will give you a picture next to it, and then ask you to judge, how to judge how number of precipitated crystals After cooling the saturated solution, how to judge cooling the saturated solution? Always don't understand, there is always a problem:50°C 100 g of A, B and C solution respectively when cooling to 10°C what the order of the quality of the solution size, it will give you a picture next to it, and then ask you to judge, how to judge how number of precipitated crystals
First find out the corresponding point on the graph at 50°C, and then reduce the temperature. Move the point to the left to the corresponding temperature. If the point is above the curve, see it according to the intersection of the curve and temperature, and see it according to the actual point.
Find find out the corresponding point on the graph at 50°C, and then cool down. Move the point to the left to the corresponding temperature. If the point is above the curve, see it according to the intersection point of the curve and temperature, and see it according to the actual point.
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- 1. How do you know if the solution is cooled or heated?
- 2. 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?
- 3. Why does crystal precipitate in the evaporating dish and a small amount of liquid remain?
- 4. 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
- 5. Is it certain that crystals will precipitate from saturated solution? What is the relationship between the quality of precipitated crystals and solubility?
- 6. Is the solution after precipitation of crystals a saturated solution of a substance? Doesn't the saturated solution have crystal precipitation after cooling?
- 7. How does grain size affect the mechanical properties of metals Why How does grain size affect the mechanical properties of metals
- 8. How does grain size affect metal properties? How to refine grain?
- 9. Is NaCl crystal melting a physical or chemical change from a bond point of view? The angle of a bond: the breaking of an old bond and the formation of a new bond are called chemical reactions The angle of a bond: the breaking of an old bond and the formation of a new bond are called chemical reactions NaCl = Na ++ Cl - The ionic bond has broken, but is there any bond?
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- 11. Saturated solution. Crystallization occurs when the solution is heated or cooled.
- 12. 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,
- 13. How does the grain size affect the mechanical properties of the material?
- 14. 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?
- 15. Why does the phenomenon of calcium hydroxide saturated solution become turbid rather than crystallized when the temperature is raised
- 16. 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?
- 17. 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
- 18. 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?
- 19. How to precipitate potassium nitrate crystals from a mixed solution of potassium nitrate and sodium chloride in a mass ratio of 1:1?
- 20. 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