Collect ethyl acetate, can you use saturated NaHCO3

Classmate: Let me explain to you: Ethyl acetate is a typical reversible reaction in our middle school stage, it is a reaction that occurs under the premise of ethanol and concentrated sulfuric acid acetate as an accelerator, but in the process of collecting ethyl acetate, we know:

NaHCO3 is a weak alkali solution, he can neutralize more acetic acid, but in the alkali solution is easy to hydrolyze, hehe, I will give you a description, in the ethyl acetate group solution is acetic acid, add NaHCO3 ( Ethyl acetate is not mixed on the surface; The interface between ethyl acetate and sodium carbonate is neutralized by acetic acid.

4.What is the purpose of the ethyl acetate catheter in the experiment that is not inserted under the liquid surface?

Anti-sucking (but note that many reversible experiments are inserted).

Anti-mixed hydrolysis (as if no one has discussed this reason) is to explain later, if the acetic acid is not neutralized, then the experiment will not be successful, ethyl acetate is acidic, alkaline hydrolyzed. If you have any questions, send me an email.

Yes, the amount of solution should be more because the solubility of NaHCO3 is less than that of Na2CO3.

In fact, NaHCO3 is less alkaline, ethyl acetate is more difficult to hydrolyze, and can still absorb acetic acid.

There is no reaction when ethanol and saturated sodium bicarbonate are mixed.

Acetic acid and saturated sodium bicarbonate solution to produce carbon dioxide gas with bubbles.

Ethyl acetate has very little solubility in lily sodium bicarbonate solution, and it will stratify with saturated sodium bicarbonate.

I don't think so, I did this experiment, I didn't use saturated NaHCO3, I'm not sure if it's feasible.

The 2nd floor makes sense, but it's better to use sodium carbonate more formally.

Summary. Because the preparation method of ethyl acetate is obtained by esterification reaction of acetic acid and ethanol, and the esterification reaction between (CH3)3COOH and (CH3)3COH requires the use of stronger catalysts and stricter reaction conditions, which usually needs to be carried out in the presence of a strong base. This is because (CH3)3COOH is more acidic and requires the use of a stronger base catalyst to neutralize the acidity and facilitate the reaction.

In addition, the reaction rate of the esterification reaction between (CH3)3COOH and (CH3)3COH is relatively slow, and more stringent reaction conditions are required to facilitate the reaction to improve the yield and efficiency of the reaction. Therefore, to prepare the esterification reaction products between (CH3)3COOH and (CH3)3COH, it is necessary to adopt an esterification reaction method different from that prepared by ethyl acetate. For example, a solution reaction method in the presence of sodium hydroxide can be used, or other strong alkali catalysts and reaction conditions, such as acid ion exchange resins, can be used to facilitate the reaction.

By selecting the appropriate esterification reaction method, the esterification reaction products between (CH3)3COOH and (CH3)3COH can be efficiently prepared.

Is the method used for the preparation of ethyl acetate suitable for esterification between (CH3)3COOH and (CH3)3COH?

The esterification reaction of CH3)3COOH and (CH3)3COH can be prepared by the preparation method of ethyl acetate, because this method is prepared by the reaction of acetic acid with ethanol under acid catalysis. The esterification reaction between (CH3)3COOH and (CH3)3COH requires other esterification methods, such as the preparation of the congratulatory solution reaction in the presence of sodium hydroxide. Fight and pat the waiter.

Why do you need to use other methods to prepare it?

Because the preparation method of ethyl acetate is obtained by esterification reaction of acetic acid and ethanol, and the esterification reaction between (CH3)3COOH and (CH3)3COH requires the use of stronger catalysts and stricter reaction conditions, which usually needs to be carried out in the presence of strong bases. This is because (CH3)3COOH is more acidic and requires the use of a stronger alkali catalyst to neutralize the acidity and facilitate the reaction to abrasion. In addition, the reaction rate of the esterification reaction between (CH3)3COOH and (CH3)3COH is relatively slow, and more stringent reaction conditions are required to facilitate the reaction to improve the yield and efficiency of the reaction.

Therefore, to prepare the esterification reaction products between (CH3)3COOH and (CH3)3COH, it is necessary to adopt an esterification reaction method different from that prepared by ethyl acetate. For example, a solution reaction method in the presence of sodium hydroxide can be used, or other strong free alkali catalysts and reaction conditions, such as acid ion exchange resins, can be used to facilitate the reaction. By selecting the appropriate esterification reaction method, the esterification reaction products between (CH3)3COOH and (CH3)3COH can be efficiently prepared.

On the one hand, the saturated sodium carbonate solution can react with acetic acid mixed in ethyl acetate and can also be miscible with ethanol; On the other hand, ethyl acetate has low solubility in saturated sodium carbonate solution, which facilitates layered dispensing.

Because the solubility of ethyl acetate in water at a certain temperature is fixed, the solubility of sodium carbonate in water is reduced, but this is no longer the solubility in water, but the solubility in sodium carbonate solution.

Neutralizes unreacted acetic acid.

Dissolve the unreacted acorn ethanol.

Reduces the solubility of ethyl acetate.

Ethyl acetate is insoluble in saturated sodium carbonate.

Summary. Washing with saturated salt water is to wash off the sodium carbonate, otherwise next.

When alcohol is washed away with a saturated calcium chloride solution, flocculent carbon is produced.

Calcium acid precipitation. Why should ethyl acetoacetate be washed with NaCl when it is prepared? It is in the organic phase, so why add NaCl and let it precipitate?

Washing with saturated salt water is to wash off the sodium carbonate, otherwise next.

When alcohol is washed away with a saturated calcium chloride solution, flocculent carbon is produced.

Calcium acid precipitation. On the one hand, the solubility of ethyl acetoacetate is reduced due to the concentration of strong ions in the aqueous phase, and the solubility of ethyl acetoacetate is reduced, and secondly, the water-oil phase can be fully separated, which is the effect of demulsification.

There are three roles.

1. Absorb and dissolve volatile alcohol.

2. React to remove volatile acetic acid.

3. It is conducive to the collection of ethyl acetate (ethyl acetate is insoluble in saturated sodium carbonate, which is conducive to stratification, and ethyl acetate is in the upper layer).

Why saturation?

At a certain temperature, a certain solute is added to a certain amount of solvent, and when the solute can no longer be dissolved, the resulting solution is called a saturated solution of this solute.

At a certain temperature, a certain solute is added to a certain amount of solution, and when the solute can no longer be dissolved, the resulting solution is called a saturated solution of this solute. The solute dissolves in the solvent dissolution process, first of all, the diffusion of the solute in the solvent, the molecules or ions on the surface of the solute begin to dissolve, and then diffuse into the solvent. The dissolved molecules or ions are constantly moving in the solution, and when they collide with the solid surface, there is a possibility that they will stay on the surface, and this deposition is the reverse process of dissolution.

When the solid solute continues to dissolve and the concentration of the solution continues to increase to a certain value, the two effects of deposition and dissolution reach a dynamic equilibrium state, that is, when the number of molecules or ions dissolved in the solvent per unit time is equal to the number of molecules or ions deposited on the surface of the solute, although the dissolution and deposition are still continuous, but if the temperature does not change, the concentration of the solution has reached a stable state, such a solution is called a saturated solution, and the amount of solute contained in it is the solubility of the solute at that temperature. It can be seen that in a saturated solution, the rate of dissolution of the solute is equal to the rate at which it accumulates from the solution, in a state of dynamic equilibrium. At a certain temperature, a solution of a solute can no longer be dissolved in a certain amount of solvent (i.e., a solution that has reached the solubility of that solute).

A solution in which a solute can continue to dissolve at the same temperature (i.e., a solution that has not yet reached the solubility of the solute) is called an "unsaturated solution". If the solute is a gas, the pressure of the gas is also indicated. A saturated solution is not necessarily a concentrated solution.

Judgment: 1There are solid residues 2

The solids are completely dissolved. (Take a certain amount of solute and add it to the solution and stir it no longer dissolves) A supersaturated solution is a solution in which the amount of solute contained in the solution is greater than the amount of solute in the saturated solution at this temperature (i.e., it exceeds the normal solubility). No solid solute must be present in the solution to produce a supersaturated solution.

To prepare a supersaturated solution, it is necessary to prepare a saturated solution at a higher temperature, and then slowly filter it to remove the excess unsoluble solute and slowly reduce the temperature of the solution to room temperature. At this time, the concentration of the solution has exceeded the saturation value at room temperature and has reached a supersaturated state. The nature of a supersaturated solution (unstable), when a small solute crystal (as a "seed") is added to this solution, it can cause the crystallization of the solute in the supersaturated solution.

Because acetic acid and ethanol volatilize when preparing ethyl acetate, saturated sodium carbonate solution can dissolve ethanol, remove acetic acid, and reduce the solubility of ethyl acetate.

1. Absorb ethanol.

2. Remove acetic acid.

3. Reduce the solubility of ethyl acetate in water.

First, it can absorb unreacted acetic acid and ethanol, so some books call it washing with sodium carbonate solution;

Second, ethyl acetate has low solubility in saturated sodium carbonate solution and less loss of products.

A saturated sodium carbonate solution can reduce the solubility of ethyl acetate in water. "This statement is unscientific. Because the solubility of ethyl acetate in water at a certain temperature is fixed, the solubility of sodium carbonate in water is reduced, but this is no longer the solubility in water, but the solubility in sodium carbonate solution.

Solution: In the esterification experiment, saturated sodium carbonate is used to absorb ethanol and acetic acid. Sodium carbonate is weakly alkaline, and ethyl acetate is hydrolyzed to a very small extent. Ethyl acetate hydrolysis conditions are dilute strong acid solution or dilute strong alkali solution. ‍

Explanation: Note, it is impossible for the saturated sodium carbonate solution to absorb ethyl ethyl acetate, so you check it carefully. ‍

aEasy separation: the solubility of DAO ester in saturated sodium carbonate solution is small, which is conducive to the stratification of esters.

bEasy to purify: saturated sodium carbonate solution can dissolve ethanol, absorb the role of acetic acid saturated sodium carbonate solution: dissolve ethanol, neutralize acetic acid, and reduce ester solubility

Hehe, because there is only a saturated sodium carbonate solution in the beaker, do you understand that it is absorbed with water, and the sodium carbonate added reduces the solubility of the ester. In fact, the whole solution in the beaker is called the aqueous solution of saturated sodium carbonate.

The function of sodium carbonate: neutralizes acetic acid, dissolves ethanol, and is conducive to smelling the fragrance of ethyl acetate.

Reduce the solubility of ethyl acetate in water, and facilitate the stratification and precipitation of esters.

The effect of saturated sodium carbonate solution.

1. Absorb ethanol.

2. Remove acetic acid.

3. Reduce the solubility of ethyl acetate.

1. Absorb ethanol.

2. Remove acetic acid.

3. Reduce the solubility of ethyl acetate in water.

It should be said that at the high school level, through concentrated sulfuric acid coheated ethanol,

When ethyl acetate is prepared from acetic acid, it is used to collect the B produced by the reaction.

Ethyl ester is sodium carbonate solution...

Therefore, ethyl acetate can be collected with a saturated sodium carbonate solution.

Ethanol and acetic acid are removed at the same time).

Removal of ethanol: Ethanol will be dissolved in water in a sodium carbonate solution and will be allowed to stand for separation.

liquid, the upper layer is ethyl acetate, and the lower layer of water contains ethanol.

Removal of acetic acid: Na2CO3 solution can react with acetic acid to produce sodium acetate dissolution.

It also plays a role in removing acetic acid in water.

p, s, common types of questions, such as whether they can be collected with naoh.

Ethyl acetate, the answer is no.

Because the NaOH solution is too alkaline, it will completely hydrolyze ethyl acetate Satisfaction Don't take it to heart, prepare well for the exam, I wish you all the best.

Acetic acid was identified with saturated Na2CO3 solution to identify the formation of bubbles.

Because ethyl acetate is insoluble in Na2CO3 solution, it delaminates.

Ethanol is miscible with saturated Na2CO3 solution and does not stratify.

In this way, the three can be identified.