Home
Class 12
CHEMISTRY
CH(3)COOH(2)^(+) , is present in the sol...

`CH_(3)COOH_(2)^(+)` , is present in the solution of acetic acid in

A

`NH_(3)`

B

water

C

Benzene

D

HCI

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question regarding the presence of the ion \( CH_3COOH_2^+ \) in a solution of acetic acid, we can follow these steps: ### Step-by-Step Solution 1. **Identify the Structure of Acetic Acid**: - Acetic acid has the molecular formula \( CH_3COOH \). It is a weak acid that partially dissociates in solution. 2. **Understand the Concept of Protonation**: - The ion \( CH_3COOH_2^+ \) indicates that acetic acid has gained an additional proton (H⁺). This means that acetic acid is being protonated. 3. **Determine the Role of the Solvent**: - For \( CH_3COOH_2^+ \) to form, a strong proton donor (acid) must be present in the solution. This is because acetic acid, being a weak acid, does not provide enough protons on its own to create the \( CH_3COOH_2^+ \) ion. 4. **Identify a Suitable Proton Donor**: - A strong acid like hydrochloric acid (HCl) can provide protons. HCl dissociates completely in solution to give \( H^+ \) and \( Cl^- \). 5. **Protonation Reaction**: - When acetic acid is dissolved in a strong acid like HCl, the \( H^+ \) ions from HCl can be abstracted by the oxygen atom in acetic acid. This results in the formation of \( CH_3COOH_2^+ \): \[ CH_3COOH + H^+ \rightarrow CH_3COOH_2^+ \] 6. **Conclusion**: - Therefore, the solvent in which \( CH_3COOH_2^+ \) is present is hydrochloric acid (HCl). ### Final Answer The solvent in which \( CH_3COOH_2^+ \) is present is **HCl**. ---
Promotional Banner

Similar Questions

Explore conceptually related problems

If degree of dissociation of 2M CH_3 COOH is 10% then degree of dissociation of this acetic acid in 3 Molar CH_3 COONa solution will be

When strong base (NaOH) is added to the weak (acid , CH_3COOH ) , then dissociation of acetic acid increase, this effect is known as

Calculate the degree of ionisation and [H_3O^(+) ] of a 0.15 M CH_3COOH solution. The dissociation constant of acetic acid is 1.8 xx 10^(-5)

Enthalpy of neutralisation of acetic acid by NaOh is -50.6 kJ mol^(-1) . Calculate DeltaH for ionisation of CH_(3)COOH . Given. The heat of neutralisation of a strong acid with a strong base is -55.9 kJ mol^(-1) .

Enthalpy of neutralisation of acetic acid by NaOH is -50.6 kJ mol^(-1) . Calculate DeltaH for ionisation of CH_(3)COOH . Given. The heat of neutralisation of a strong acid with a strong base is -55.9 kJ mol^(-1) .

0.1 M CH_(3) COOH solution is 1.0% ionized. In another diluted solution acetic acid is 10% ionised. In other solution concentration of acetic acid is

CH_(3)COOH is titrated with NaOH solution. Which of the following statements is true ?

Acetic acid dissociates as CH_(3) "COOH" hArr CH_(3) "COO"^(-) + H^(+) . If a little amount of sodium acetate is added to its aqueous solution

Let us consider the inonisation of HCl in the aqueous solution of CH_(3)COOH CH_(3)COOH + HCl hArr CH_(3)COOH_(2)^(+) +Cl^(-) Select the correct statement (s) among the following :

A solution contains 0.09 HC1, 0.09 M CHC1_(2)COOH , and 0.1M CH_(3)COOH . The pH of this solution is one. Calculate K_(a) for CHC1_(2)COOH . (Given K_(a)CH_(3)COOH = 10^(-5))