Experimental Report on the Reaction of Metal and Compound Solution
The following is an example of an experimental report on the reaction of a metal and a compound solution: ** 1. Purpose of the experiment ** 1. To explore the law of the reaction between metals and compound solutions. 2. Comparing the order of activity of different metals. ** 2. Experiment Principle ** The more active metal could replace the less active metal from its compound solution. By observing the reaction phenomenon (such as whether there is a new metal separation, the color change of the solution, etc.) to determine whether the reaction occurred, and then determine the order of metal activity. ** 3. Laboratory supplies ** 1. ** Instrument **: Test tube, test tube rack, tweezers, etc. 2. ** Pharmaceuticals **: aluminum sheet, iron sheet, copper sheet, copper sulfuric acid solution, aluminum sulfuric acid solution, silver nitrates solution, etc. ** 4. Experimental Steps ** 1. Reaction of aluminum and copper sulfuric acid solution - He took a test tube and added a suitable amount of copper sulfuric acid solution. - He used a pair of tweezers to pick up a piece of aluminum and put it into the copper sulfuric acid solution. - Observation: There is a red substance on the surface of the aluminum sheet, and the color of the solution gradually lightens. The reaction equation is: 2AI + 3CuSO = Al2 (SO)+ 3Cu. 2. Reaction of iron and copper sulfuric acid solution - He took out another test tube and added the copper sulfuric acid solution. - He used a pair of tweezers to pick up a piece of iron and put it into the solution. - Red substances were observed on the surface of the iron sheet, and the color of the solution became lighter. The reaction equation was: FeSO2 + CuSO2 = FeSO2 + Cu2. 3. Reaction of Copper with Aluminium-Sulphate Solution - He took out a test tube and added the solution. - He placed a piece of copper. - Observed phenomenon: No obvious phenomenon, indicating that copper cannot replace the aluminum in the aluminum sulfuric acid solution, and the mobility of copper is weaker than that of aluminum. 4. Reaction of Copper with Silver Nitrate Solution - He took out a test tube and added the silver nitrates solution. - Put in the copper plate. - A silver-white substance was seen on the surface of the copper plate, and the color of the solution changed. The reaction equation was: Cu + 2AgNO = Cu(NO) 2 + 2AG. ** 5. Experimental results and analysis ** 1. Through the reaction between aluminum and copper sulfuric acid solution, and the reaction between iron and copper sulfuric acid solution, it could be seen that aluminum and iron were more mobile than copper. 2. Copper did not react with the aluminum sulfuric acid solution, further indicating that the mobility of aluminum was stronger than copper. 3. Copper reacted with silver nitrates, which meant that copper was more mobile than silver. Based on the above experimental results, the order of metal activity was as follows: Al > Cu > Ag, Fe > Cu> ** 6. Experiment conclusion ** 1. The order of metal activity affects the reaction between the metal and the compound solution. The more active metal can replace the less active metal. 2. When describing the reaction phenomenon between metal and metal compound solution, it was necessary to pay attention to the attachment of new metal to the surface of the original metal and the change in color of the solution. 3. This kind of reaction must be carried out in a solution. The metal compound must be water-dissolved, and the metal compound that is not water-dissolved generally does not react with the metal. Read more exciting novels for free
Reaction equation and phenomenon of solution and metal
1. **金属与酸的反应** - **反应方程式及现象（以常见金属镁、铁、锌、铝与稀硫酸反应为例）** - 镁与稀硫酸反应：\(Mg + H_{2}SO_{4}=MgSO_{4}+H_{2}\uparrow\)，现象为反应剧烈，有大量气泡产生。 - 铁与稀硫酸反应：\(Fe + H_{2}SO_{4}=FeSO_{4}+H_{2}\uparrow\)，现象是有气泡产生，溶液由无色变为浅绿色（因为生成了亚铁离子）。 - 锌与稀硫酸反应：\(Zn + H_{2}SO_{4}=ZnSO_{4}+H_{2}\uparrow\)，反应较剧烈，产生气泡。 - 铝与稀硫酸反应：\(2Al+3H_{2}SO_{4}=Al_{2}(SO_{4})_{3}+3H_{2}\uparrow\)，产生气泡。 - **反应规律及图像问题（针对初中化学常见考点）** - 当等量的金属分别和足量的酸反应（酸过量）时，反应中最终产生氢气的多少由金属决定。在金属化合价相同的情况下，对于相同质量的金属，金属的相对原子质量越大，生成的氢气越少;生成的氢气越多，金属的相对原子质量越小。 - 当等量的酸分别和足量的金属反应（金属过量）时，反应产生氢气的量由酸的量决定，最终产生氢气的量相等。 - 两种或多种金属与稀酸反应时，反应的快慢（即相同时间内产生氢气的多少）由金属的活动性决定，在温度、金属颗粒大小和稀酸溶液溶质质量分数一定的条件下，金属的活动性越强，生成氢气就越快;生成氢气越快，说明金属的活动性就越强。在图像中，纵坐标通常为产生氢气的量，横坐标可能为时间、消耗酸的质量或消耗金属的质量。 2. **金属与盐溶液的反应** - **反应方程式及现象（以铁丝浸入硫酸铜溶液为例）** - 反应方程式：\(Fe + CuSO_{4}=FeSO_{4}+Cu\)，现象为浸入溶液中的铁钉表面覆盖红色物质（铜），溶液由蓝色逐渐变为浅绿色。 - **反应条件及规律** - 金属（钾、钙、钠除外）的活动性强于盐中金属阳离子对应的金属;盐必须可溶于水。当多种金属和多种盐溶液反应时，最活泼的金属先与最不活泼的金属盐反应，再轮到较活泼的金属或金属盐反应。例如向一定量的硝酸银和硝酸亚铁混合溶液中加入锌粉，金属活动性顺序为锌>铁>银，锌先与硝酸银反应，硝酸银完全反应后，若锌还有剩余，则锌再与硝酸亚铁反应。 3. **金属与酸性溶液中的氢离子反应（以酸性溶液与金属反应为例）** - 酸性溶液中的氢离子（\(H^{+}\)）会与金属发生反应，如形成氢气，同时金属逐渐溶解，但未明确具体金属时无法给出确切方程式。 4. **特殊金属与溶液反应（如金属铋与稀硝酸反应）** - 放入金属铋，加入稀硝酸，加热试管，冷却后加水稀释，反应方程式为\(Bi + 4HNO_{3}=Bi(NO_{3})_{3}+NO\uparrow+2H_{2}O\)（根据给出的后续反应推测铋与稀硝酸反应的可能方程式），现象未明确提及，可能有气体产生等现象。 5. **金属与水反应（以金属钾与水反应为例，虽然未明确要求，但属于金属与溶液相关反应类型）** - 金属钾与水反应：\(2K + 2H_{2}O = 2KOH+H_{2}\uparrow\)，现象是反应剧烈，可能有燃烧、爆炸等危险现象（因为反应放出大量热和氢气）。 <a href="/?from=ask_words" style="color:red" target="_blank">点击前往免费阅读更多精彩小说</a>
What is the reaction equation of solution and metal?
The reaction equation between a solution and a metal used chemical symbols and chemical formulas to represent the chemical reaction between the solution and the metal. It described the process of transforming the reagents (solute and metal in the solution) into products. It followed the law of conservation of mass, which meant that the type and number of atoms would not change in a chemical reaction. For example, in the chemical equation,[2Na +2H ^O = 2Na +2H ^O + H ^^], it means that the metal, Na, will react with water to form Na ions, Ox ions, and hydrogen. The reaction equation not only indicated what the reagents and products were, but it could also express the ratio of the number of particles (the ratio of the number of molecules or atoms) between the substances through the stoichiometric-number (the coefficient in the equation). At the same time, the mass relationship between the reagents and products could be determined according to the relative atomic mass or relative molecular mass. This helped to predict the outcome of the reaction, calculate the amount of reagents and products, and understand the nature of the reaction. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Experimental Report on the Effect of Sulfur Sulphate on Iodine Reaction
#Experimental Report on the Effect of Sulfur Sulphate on Iodine Reaction ** I. Introduction ** The reaction between iodines and thiothiosulfates was of great significance in the field of chemical analysis, especially in the process of iodoscopic titrations. The purpose of this experiment was to investigate the effect of the reaction of sulfur dioxide on the reaction of sulfur dioxide, including the reaction principle, reaction phenomenon, and the mechanism behind it. ** 2. Experiment Principle ** 1. ** Reaction equation ** - The chemical equation of the reaction between sulfur dioxide (Na2S2O3) and sulfur dioxide (I2) is: 2Na2S2O3 + I2 = Na2S4O6 + 2NaI. This reaction was an oxido-reduction reaction, in which the reducing agent was thiothiosulfuric acid, and the oxidiser was iodinate. 2. ** Reaction process ** - In the reaction system, the iodines were oxidiser, while the sulfur in the thionate was in an intermediate state and had a reducing property. When the two were mixed, the sulfur atom in the sulfur dioxide was oxided by the iodate, and the iodate itself was reduced to the iodate ion (I^-). ** 3. Experiment Materials and Methods ** 1. ** Experiment Materials ** - Iodine solution (known concentration), solution of thiothiosulfuric acid (known concentration), starch indicator, conical flask, buret, pipet, etc. 2. ** Experiment Method ** - Weigh a certain volume of the solution and place it in a conical flask. Use a pipet to accurately add a certain amount of the solution. At the same time, shake the conical flask to mix the solution thoroughly. When the reaction was approaching the end point, a starch indicator was added to observe the color change of the solution. The experiment was repeated by changing the amount of the solution of thiothiosulfuric acid, and the reaction phenomena and related data under different conditions were recorded. ** 4. Experiment result ** 1. ** Reaction Phenomenon ** - At the beginning of the reaction, the solution did not change color because the reaction between the sulfur and the sulfur was colorless. As the reaction progressed, when there was a small amount of remaining uranium, the solution would turn blue after adding the starch indicator. If he continued to add the solution, the blue color would gradually fade until the solution became colorless. 2. ** Data Record ** - Through many experiments, the corresponding time of the color change of the solution, as well as the change in the concentration of the solution before and after the reaction, were recorded. For example, when adding x ml of the solution of thiothiosulfuric acid, the color of the solution completely faded after the reaction for t seconds. The concentration of the solution before the reaction was C1, and the concentration of the solution after reaction was C2. ** 5. Analysis of the results ** 1. ** Effect on reaction rate ** - It could be seen from the experimental results that the concentration and dosage of the solution had a significant effect on the reaction rate. With the increase of the concentration or the addition of the amount of the Thiosulfuric acid, the reaction rate increased, and the time required for the color change of the solution shortened. This was because in the reaction system, the probability of collision between the molecules of sulfur dioxide and the molecules of sulfur dioxide increased with the increase of the concentration or amount of sulfur dioxide, which made the reaction proceed more quickly. 2. ** Impact on the reaction end point ** - The reaction end point was determined by the color change of the starch indicator. When the iodines were completely reacted with the thiothioates, the starch-iodines in the solution decomposed and the blue color disappeared. If the amount of thionate added was insufficient, the solution would show a blue color, indicating that there was still unreacted iodate; if the amount was too much, the solution would be colorless after the reaction, and the accuracy of subsequent measurement of iodate content might be affected. ** 6. conclusion ** The experiment showed that the effect of the thiothiosulfuric acid on the reaction of the iodines was significant. Its concentration and amount of addition affected the reaction rate and the determination of the reaction end point. In practical applications, such as the operation of the iodoxy method, the dosage of the thionate needed to be precisely controlled to ensure the accuracy of the experimental results. At the same time, this experiment also deepened the understanding of the principle and characteristics of the oxido-reduction reaction between sulfur dioxide and sulfur dioxide. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Experimental process of the reaction between the silver solution and the carbolic group
The reaction between silver and an aromatic group (using an example of this) was as follows: 1. ** The preparation of the silver solution: - In a clean test tube, add 1 - 2ml of 2% - 3% silver nitrates solution, then add a drop of 5% solution of soda, and then add 2% diluted aqua solution drop by drop while shaking the test tube, until the initial deposit just dissolved, to produce the silver solution. The reaction equations were: [AgNO3 + NH3·H2O = AgOx + NH4NO3],[AgOx +2NH3·H2O = AgOx +2H2O]. 2. ** Silver Mirror Reaction Operation **: - Add 3 - 5 drops of 40% potassium ether to the silver solution, shake it gently, and then immediately heat the test tube in a water bath at 60 - 70 ° C. - During the heating process, the color of the solution would change from colorless to milky white, dark red, colorless, and finally to silver-white. Then, a bright silver mirror would appear on the inner wall of the test tube. 3. ** Note **: - The solution must be used immediately and must not be left for a long time. Otherwise, it would form a black and explosive silver tri-nitrogen deposit (Ag3N). - The test tube used must be very clean. If the test tube was not clean, most of the restored silver would be loose and grainy, and the bright silver mirror would not be obtained. It can be washed with hot sulfuric acid, 10% NaClO solution, and then rinsed with distilled water. - Do not shake the test tube again when the solution of silver and amine is evenly mixed with the dripped potassium ether. Otherwise, it will form a black, loose silver deposit instead of a bright silver mirror. - The reaction must be heated in a water bath. Do not heat it directly with a flame, or it may explode. During the water bath heating process, do not shake the test tube, nor stir the solution. The water bath temperature should be 60 - 70 ° C. Because the boiling point of jumped ether is low, too high a temperature will cause a large amount of jumped ether to evaporate and the reaction effect will be poor. It is difficult to obtain a bright silver mirror, but only black fine silver particles can be obtained. - The dosage of Zhang Tie's alcohol should not be too much. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Experimental Report on the Reaction of Dilute Sulfuric Acid and Natrium Hydride
|experimental procedure| experimental phenomenon| experiment conclusion| |--|--|--| |continuously dripping the sulfuric acid into a solution of sulfuric acid in the presence of phenothalin.| The red color of the solution gradually disappeared| The diluted sulfuric acid reacted with the soda, and the equation was as follows: HC1 + NaOx = NaCl2 + H2O. When the red color just disappeared, it meant that the added sulfuric acid had completely reacted with the solution of sulfuric acid. This was because the combination of the Oh in the solution of sulfuric acid and the H in the solution of sulfuric acid formed H O, causing the solution to gradually weaken until it was neutral.| |continuously dropping the solution of the solution| If a solution of NaH was added to the solution of NaH, the initial solution would have a pH-value of <7, and the pH-value would gradually increase with the addition of NaH. If a solution of NaH was added to the solution of NaH, the initial pH-value of the solution would be <7, and the pH-value would decrease with the addition of acid. When the reaction was complete and formed NaCl-water, the pH-value would be <7. When the acid was excessive, the pH-value would be <7.| By measuring the change of the pH-value, one could directly see the change of the pH-value of the solution during the reaction between diluted sulfuric acid and the solution of the solution of| <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Will the reaction of acid and base solution change color? What is the experimental principle?
The reaction between acid and base solution may change color, which can be judged by the different colors of the acid, base, and neutral solutions. The principle of the color change of the alkali-base indicator was that the alkali-base indicator was some organic weak acid or organic weak base. In the solution, they could be partially dissociated into the indicator's ions and hydrogen ions (or hydrogen ions). Due to the change in structure, the molecules and ions had different colors, so they would display different colors in different alkali-base solutions. For example, when the sulfuric acid concentration in the solution was reduced, it would turn red when the sulfuric acid concentration increased. When acid and base react, the solution's pH-value will change, which will cause the acid and base indicator to gain a proton and transform from basic to the conjugated acid, or lose a proton and transform from acid to the conjugated base. Due to the change of its structure, the color will change. This color change is a chemical change, because the acid and base indicator is generally an organic weak acid or weak base. They are weakly ionised in water. The added acid or base will be ionised to produce H or Oh, which will cause the combination of the two to move to the equilibrium of ionisation and dehydration. It caused the ratio of ions to substances in the original solution to change and present different colors. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Reaction of the solution with the solution
There were different opinions on whether or not the reaction between the two substances occurred. One view was that silver chloride-soda would react to produce silver-white silver silver precipitations and NaCl2, and the silver-white precipitations could easily be converted to brown silver oxide-soda. The other view was that the reaction could not be carried out because the reaction between base and salt required the salt to be dissolved, while AgCl2 was difficult to dissolve. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
How to write the experimental report on the reaction of carbon dioxide and carbon dioxide
Reaction equation of the solution of the saturated solution of the solution of
There was no reaction between the saturated solution of NaCl2 and the solution of NaOx. This was because it did not meet the conditions for a metathesis reaction (forming a deposit, gas, or water). <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
What are the reaction phenomena of the solution of the solution of the iron of the solution of the solution of the
Ferrocyanide could react with the reaction of the acid to form a deposit of the acid. This deposit could carry away or absorb interfering substances. It had a strong ability to remove protein, but its ability to remove color was poor. The main reaction phenomenon was the formation of the precipitations of the metal. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>