TS EAMCET · Chemistry · Ionic Equilibrium

The successive equilibrium constants for the stepwise dissociation of a tribasic acid are \(K_1\), \(K_2\) and \(K_3\), respectively. The equilibrium constant for the overall dissociation is

A \(\left(K_1+K_2+K_3\right)\)
B \(\sqrt[3]{\left(K_1+K_2+K_3\right)}\)
C \(\left(K_1 \times K_2 \times K_3\right)^3\)
D \(K_1 \times K_2 \times K_3\)

Verified Solution

Answer & Solution

Correct Answer

(D) \(K_1 \times K_2 \times K_3\)

Step-by-step Solution

Detailed explanation

For a tribasic acid like \(\mathrm{H}_3 \mathrm{PO}_4\) has three ionisation constant. The overall ionisation constants \((K)\) will be product of ionisation constants of three steps, i.e. \[K=K_1 \times K_2 \times K_3\]…

Apply the relevant identity from the chapter and substitute the values established in the previous step, keeping the original constraint in view.

Use the simplified expression to isolate the unknown, then plug the result back into the question setup to confirm the working is internally consistent.

Cross-check against a boundary or limiting case. Both the dimensional balance and the qualitative behaviour at the extreme should agree with the candidate answer.

Combine the steps above to identify the correct option. The remaining choices each fail at least one of the consistency, dimensional, or boundary checks.

Same subject

Explore more questions on app

From TS EAMCET

Explore more questions on app

	Column-1 Reaction		Column-2 product
A		I	Cyclohexanol
B		II	Benzyl alcohol
C		III	Toluene
		IV	Benzaldehyde
		V	Cyclohexane