What will be the effect of adding solid NaHCO3 to hot concentrated H2SO4? Why should the reaction vessel containing a synthesized ester be cooled first before neutralization?

My Guess #1:
Since neutralization is an exothermic process and the ester is in equilibrium with its reactants then neutralization would put a stress on the products side and the reaction would favor the backward reaction and less of the ester will be obtained.
My Guess #2:
The neutralization of the acid will cause an increase in the temperature and this could cause slight evaporation of the ester.

PLS. I NEED HELP...

Combine guess 1 and guess 2. Guess 1 is not so much about neutralization but about containing hydrolysis. If you want to hydrolyze an ester, water and acid and heat is the way to do it. In guess #2, again, segue into the reverse direction. You are right that elevated temperatures may volatilize some of the ester (depending upon which ester we are talking about) but the main idea here is to keep the temperature down so the reverse reaction (hydrolysis) will not take place.

When solid sodium bicarbonate (NaHCO3) is added to hot concentrated sulfuric acid (H2SO4), a violent reaction occurs. This is because the reaction between NaHCO3 and H2SO4 produces carbon dioxide gas (CO2), water (H2O), and sodium sulfate (Na2SO4). The reaction is as follows:

2NaHCO3 + H2SO4 -> CO2 + H2O + Na2SO4

The reaction is highly exothermic, meaning it releases a large amount of heat. In this case, the reaction is not only exothermic but also produces a gas, which can result in a rapid increase in pressure inside the reaction vessel. The combination of the heat and pressure can cause the reaction mixture to forcefully eject from the container, potentially leading to an explosion or other safety hazards. Therefore, it is extremely important to never add solid NaHCO3 to hot concentrated H2SO4.

As for your second question, the cooling of the reaction vessel containing a synthesized ester before neutralization is done to prevent potential side reactions or loss of the ester. When an ester is synthesized, it is often done through a reaction between an alcohol and an acid, known as an esterification reaction. This reaction is typically conducted at an elevated temperature and can be reversible under certain conditions.

Neutralization involves the reaction between an acid and a base, usually an alkali. This process can release heat, potentially raising the temperature in the reaction vessel. If the ester is still in equilibrium with the reactants used in its synthesis, an increase in temperature can disrupt this equilibrium. According to Le Chatelier's principle, a change in temperature can shift the equilibrium in a direction that opposes the temperature change.

If the neutralization reaction causes an increase in temperature, it can favor the backward reaction, leading to the conversion of the ester back into its reactants (alcohol and acid). This would result in the loss of ester and a decrease in the overall yield. Cooling the reaction vessel before neutralization helps to maintain the equilibrium established during ester synthesis and prevent potential side reactions, ultimately preserving the ester product.