Ag reacts with what reaction will form a precipitate

chemical experiments] common precipitation formation.

1. Silver ions and chloride ions to generate silver-white chloride sedimentation lake;

2. Silver ions and bromide ions to generate yellowish precipitates of silver bromide;

3. Silver ions and iodide ions generate silver iodide yellow precipitate;

4. Silver and sulfur ions are formed to form sulfur branches and silver-black precipitates;

5. Silver ions and carbonate ions generate silver carbonate white precipitates;

6. Silver ions and hydroxide ions generate silver hydroxide, which is easy to decompose when seen in light and generates black precipitation of silver oxide.

1. It is insoluble in water and acid-insoluble precipitate with chloride ions, bromine ion, and iodine ions.

2. It produces white precipitate with carbonate ions, sulfate ions, and sulfite ions, and soluble orange is acidic.

3. It produces silver sulfide black precipitate with sulfide ions.

4. Silver hydroxide precipitation is produced with hydroxide ions, which is decomposed into black silver oxide and carbonate dome Hegan ions when seen by light.

Because other ions and Ag+ can also produce white precipitates, such as Ag2CO3 and Ag2SO4 are white, but these precipitates are soluble in HNo3 but Agcl is insoluble, so the purpose of adding HNo3 is to eliminate the interference of other anions and ensure the accuracy of the results.

After adding silver nitrate solution, the white precipitate cannot be determined to be silver chloride precipitate, but silver chloride is insoluble in acid, so adding nitric acid to see the precipitate can prove whether chloride ions exist in the solution. Other insoluble compounds of silver are soluble with dilute nitric acid, so dilute nitric acid acidification is added to exclude interference from other silver ions.

Inspection. Objective: To understand the method of nitrate ion detection.

Supplies: test tubes, test tube racks, test tube clamps, graduated cylinders.

Potassium nitrate, ferrous sulfate, concentrated sulfuric acid.

Principle: Nitrate ions are oxidizing, and ferrous ions can be oxidized into iron ions in an acidic solution, and they are reduced to nitric oxide. Nitric oxide can combine with many metal salts to form unstable nitroso compounds.

Summary. Hello dear, HCl is a strong acid that reacts with alkaline substances such as sodium hydroxide to produce salts and water. Sodium carbonate is an alkaline substance that reacts with HCl to produce salts (sodium chloride) and water, as well as carbon dioxide.

Why does AG+ react with HCl.

Dilute hydrochloric acid. Hello dear, HCl is a strong acid that reacts with alkaline substances such as sodium hydroxide to produce salts and water. Sodium carbonate is an alkaline substance that reacts with HCl to produce salts (sodium chloride) and water, as well as carbon dioxide.

Why do ag ions react with dilute hydrochloric acid?

Ag ions can react with dilute hydrochloric acid, because dilute hydrochloric acid contains chloride ions, and chloride ions can reversibly react with Ag ions to produce AgCl precipitate: Ag+(AQ) +Cl-(AQ) agCl(S).

Ag ions can react with dilute hydrochloric acid, because Ag ions can react with H+ ions in dilute hydrochloric acid to form Ag+ ions and Cl- ions, which makes the solution appear pale white.

There are actually quite a lot of possibilities.

Depending on the amount ratio of the reactant and the reaction temperature, there are several reactions that may occur

In the case that the reaction is carried out more thoroughly and the amount of HNO3 is relatively large, all the oxidized ones are oxidized

AG2S + 9HNO3 = = Heating == AGHso4 + AGNO3 + 8NO2 (gas) + 4H2O

This reaction seems unbelievable ... It can be a little tricky to explain.

To put it simply, Ag2SO4 is soluble in nitric acid, and after dissolving, the reaction occurs as follows:

ag2so4 + hno3====agno3 + aghso4

This is because H2SO4 has a relatively weak degree of secondary ionization, i.e., a weaker degree of HSO4- ionization (especially compared to HNO3).

However, this idea is largely ignored in secondary school chemistry.

This is also the reason why ag2so4 is deliberately avoided throughout middle school.

Moderate amount of Hno3:

3AG2S + 8HNO3 == Heating == 6AGnO3 + 3S + 4H2O + 2NO

If there is a slight amount of Hno3 at this time, then S can continue to react with Hno3.

In general, I prefer the first reaction, because the reaction may be more thorough under heating conditions.

The reaction of silver and protein depends on the type of protein and the type of silver. Normally, silver can react with proteins by binding to the teller or protein through electrostatic interactions, forming silver-protein complexes. This binding can be used to detect and measure the presence of proteins.

For example, AG can be used to detect the presence of antigens in a sample by reacting with a specific antibody. "Socks P>

There is a close connection between AG and protein. AG can be used as a catalyst for proteins, promoting protein production and activation, thereby triggering specific biological reactions. In addition, egg finch white matter can also help Ag to carry out redox reactions, which is an important positive slippery reaction between proteins and AG.

In addition, proteins can also affect the structure and properties of AG, so the relationship between AG and proteins is very close.

OK. If you have studied the precipitate dissolution equilibrium, you will know that the insoluble precipitate will transform into a more insoluble precipitate.

Sodium bromide or potassium iodide solution can be added to the silver chloride suspension, and the chlorinated jujube silver precipitation will be converted into a more insoluble pale yellow precipitate AGBR or yellow precipitate AGbr or yellow precipitate AGI in the rock suspension.

If it is recognized, hopefully!!

The ionic reaction equation for the precipitation of Ag+ is Ag+++Cl-AgCl, according to the influence of concentration on chemical equilibrium.

Hello, I am glad to answer for you: when the concentration of Ag+ increases, the reaction develops in the direction of AgCl formation, that is, the greater the concentration of Ag+, the faster the generation rate of AgCl is cleared. At the same time, when the concentration of Cl- increases, the reaction develops in the direction of AgCl formation, that is, the greater the concentration of Cl-, the faster the formation rate of AgCl.

Therefore, in the case of chemical equilibrium, the higher the concentration of both Ag+ and Cl-, the faster the rate of AgCl formation. At the same time, since the chemical equilibrium is dynamic, when the concentrations of Ag+ and Cl- change, the chemical equilibrium will also change, resulting in a corresponding change in the rate of AgCl formation. In addition, in practical applications, the influence of temperature on chemical equilibrium needs to be considered.

In general, the rate of chemical reaction increases as the temperature increases, so the rate of AgCl formation is also faster at higher temperatures, when the concentration of Ag+ and Cl- is larger.