Question

Which of the following is basic?
(A) $ {C_2}{H_5}OH $
(B) $ {H_2}{O_2} $
(C) $ OHC{H_2}C{H_2}OH $
(D) $ C{H_3}COOH $

Answer 1

Hint :A base is a chemical entity in aqueous solution that gives electrons, receives protons, or releases hydroxide ( $ O{H^ - } $ ) ions. Bases have specific distinguishing characteristics that may be utilised to assist identify them. They have a slick texture (like soap), have a harsh taste, combine with acids to create salts, and accelerate specific processes. Arrhenius bases, Bronsted-Lowry bases, and Lewis bases are examples of base types. Alkali metal hydroxides, alkaline earth metal hydroxides, and soap are examples of bases.

Complete Step By Step Answer:
For the sake of this discussion, an acid will be defined as "a substance that distributes hydrogen ions (protons) to other objects." We'll look at how quickly acids release hydrogen ions to water molecules while they're in solution in water to get a gauge of this.
Ethanol, $ {C_2}{H_5}OH $ , is so weakly acidic that it isn't even considered acidic. An ethoxide ion is generated when the hydrogen-oxygen link breaks, releasing a hydrogen ion: $ {C_2}{H_5}{O^ - } $ This has absolutely nothing going for it. The negative charge, which is securely attached to the oxygen atom, cannot be delocalized. The ethanol will rapidly re-form due to the powerful negative charge's strong attraction to hydrogen ions. Because ethanol has a difficult time releasing hydrogen ions, it is neither acidic nor basic in nature.
 $ C{H_3}COOH $ Is a weak acid. The hydrogen that is linked to the oxygen is acidic. When ethanoic acid ionises, the ethanoate ion, $ CH3CO{O^ - } $ is formed. The structure of the ethanoate ion would appear to be as follows, however bond length studies reveal that the two carbon-oxygen bonds are similar and are somewhere between a single and a double bond in length. The more charge you can distribute, the more stable an ion becomes. In this situation, delocalizing the negative charge over numerous atoms makes it less appealing to hydrogen ions, reducing the likelihood of re-forming ethanoic acid.
Because of the electron-withdrawing capacity of the terminal hydroxyl group, glycolic acid is somewhat stronger than acetic acid. Hydrogen peroxide is a weak acid that reacts with several metals to generate hydroperoxide or peroxide salts.
Hence option A is correct.

Note :
The organic acids are weak in terms of ionisation since it is relatively incomplete. The majority of the acid will be present in the solution as unionised molecules at any one moment. In the case of dilute ethanoic acid, for example, the solution contains around 99 percent ethanoic acid molecules, but only approximately 1% have ionised at any one time. As a result, the equilibrium point is well to the left.