Given below are two statements : Statement (I) : A Buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities Statement (II) : Blood is naturally occurring buffer solution whose pH is maintained by H_2 CO_3 / HCO_3 ^\ominus concentrations. In the light of the above statements, choose the correct answer from the options given below :

Statement I is false but Statement II is true

Both Statement I and Statement II are false

Both Statement I and Statement II are true

Statement I is true but Statement II is false

Ionic Equilibrium PYQ — JEE Main 2024 · 8 Apr · Shift 2 · Q2 with Solution

View written solutionFree

Correct answer: C

Analyze Statement (I)

A buffer solution is not just any mixture of a salt and an acid or a base in any particular quantities.

A buffer is specifically:
- a weak acid + its conjugate base (salt), or
- a weak base + its conjugate acid (salt)
Also, the components must be present in suitable amounts so that the solution can resist change in pH.

Examples:
- Acidic buffer: $\mathrm{CH_3COOH + CH_3COONa}$
- Basic buffer: $\mathrm{NH_4OH + NH_4Cl}$
So Statement (I) is false because:
- it does not specify weak acid/base,
- and says any quantities, which is incorrect.
Analyze Statement (II)

Blood is a naturally occurring buffer solution.

Its pH is maintained mainly by the bicarbonate buffer system: $\mathrm{H_2CO_3 / HCO_3^-}$

This is a standard biological buffer system helping maintain blood pH near $7.4$ .

Therefore, Statement (II) is true.
Choose the correct option
- Statement (I): False
- Statement (II): True
Hence, the correct option is: $\boxed{\text{C}}$
Comparison with stored answer

Stored correct answer: C

My derived answer: C

So, they agree.

View written solutionFree

Correct answer: C

Analyze Statement (I)

A buffer solution is not just any mixture of a salt and an acid or a base in any particular quantities.

A buffer is specifically:
- a weak acid + its conjugate base (salt), or
- a weak base + its conjugate acid (salt)
Also, the components must be present in suitable amounts so that the solution can resist change in pH.

Examples:
- Acidic buffer: $\mathrm{CH_3COOH + CH_3COONa}$
- Basic buffer: $\mathrm{NH_4OH + NH_4Cl}$
So Statement (I) is false because:
- it does not specify weak acid/base,
- and says any quantities, which is incorrect.
Analyze Statement (II)

Blood is a naturally occurring buffer solution.

Its pH is maintained mainly by the bicarbonate buffer system: $\mathrm{H_2CO_3 / HCO_3^-}$

This is a standard biological buffer system helping maintain blood pH near $7.4$ .

Therefore, Statement (II) is true.
Choose the correct option
- Statement (I): False
- Statement (II): True
Hence, the correct option is: $\boxed{\text{C}}$
Comparison with stored answer

Stored correct answer: C

My derived answer: C

So, they agree.