Given below are two statements:
Statement (I): Aqueous solution of ammonium carbonate is basic.
Statement (II): Acidic/basic nature of salt solution of a salt of weak acid and weak base depends on \( K_a \) and \( K_b \) value of acid and the base forming it.
In the light of the above statements, choose the most appropriate answer from the options given below:
Statement (I): Aqueous solution of ammonium carbonate is basic.
Statement (II): Acidic/basic nature of salt solution of a salt of weak acid and weak base depends on \( K_a \) and \( K_b \) value of acid and the base forming it.
In the light of the above statements, choose the most appropriate answer from the options given below:
- Both Statement I and Statement II are correct
- Statement I is correct but Statement II is incorrect
- Both Statement I and Statement II are incorrect
- Statement I is incorrect but Statement II is correct
The Correct Option is A
Approach Solution - 1
The question provides two statements to analyze, and we need to determine the validity of each statement.
- Understanding Statement I: "Aqueous solution of ammonium carbonate is basic."
- Ammonium carbonate is the salt formed from a weak acid (carbonic acid, \(H_2CO_3\)) and a weak base (ammonia, \(NH_3\)).
- In aqueous solution, ammonium carbonate dissociates into ammonium ions \((NH_4^+)\) and carbonate ions \((CO_3^{2-})\).
- The carbonate ion is capable of undergoing hydrolysis to produce hydroxide ions \((OH^-)\), making the solution basic:
- Reasoning for Statement II: "Acidic/basic nature of salt solution of a salt of weak acid and weak base depends on \(K_a\) and \(K_b\) value of acid and the base forming it."
- The relative values of the acid dissociation constant \((K_a)\) for the conjugate acid and the base dissociation constant \((K_b)\) for the conjugate base determine the pH of the solution.
- If \(K_b > K_a\), the solution tends to be basic. Conversely, if \(K_a > K_b\), the solution is typically acidic.
- For ammonium carbonate, the basicity due to the carbonate ion (since it has a higher affinity for protons compared to the hydrolysis of the ammonium ion) usually prevails, leading to a slightly basic solution.
Given these considerations, both statements are accurate:
- Statement I is correct because the carbonate ion's hydrolysis makes the aqueous solution of ammonium carbonate basic.
- Statement II is correct as it appropriately describes the dependence on \(K_a\) and \(K_b\) values for salts derived from weak acids and bases.
Conclusion: The correct answer is that both Statement I and Statement II are correct.
Approach Solution -2
Statement I: Ammonium carbonate (NH4)2CO3 is basic in solution because it forms a weak acid (NH4+) and a weak base (CO32-). The carbonate ion (CO32-) can accept protons, making the solution basic.
Statement II: This statement is also correct as the pH of a salt solution formed from a weak acid and a weak base depends on the relative values of Ka and Kb.
So, Statement I and II both are correct.
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