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 $H_2CO_3/HCO_3^-$ concentrations.
In the light of the above statements, choose the correct answer from the options given below.
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 $H_2CO_3/HCO_3^-$ 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 is true
- Both Statement I and Statement II is false
- Statement I is true but Statement II is false
The Correct Option is A
Approach Solution - 1
Let's analyze the given statements and their validity concerning buffer solutions and physiological examples such as blood.
- Statement I: "A Buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities."
- This statement is false because a buffer solution is not just any mixture of a salt and an acid or base. It specifically consists of a weak acid and its conjugate base (or a weak base and its conjugate acid) in a suitable ratio. This combination helps maintain a stable pH upon the addition of small amounts of acid or base.
- Statement II: "Blood is naturally occurring buffer solution whose pH is maintained by \(H_2CO_3/HCO_3^-\) concentrations."
- This statement is true. Blood is indeed a natural buffer system primarily maintained by a carbonic acid (\(H_2CO_3\)) and bicarbonate (\(HCO_3^−\)) buffer system. This mechanism is efficient in regulating the pH of blood around 7.4, crucial for physiological processes.
In conclusion, the correct option is that Statement I is false but Statement II is true. This correctly identifies the nature of buffers and recognizes the specific biological example of blood as a buffering system.
Approach Solution -2
To analyze the given statements, we will first understand the concept of buffer solutions and their relevance in biological systems, such as blood.
Statement (I): "A Buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities."
- A buffer solution is a solution that resists changes in its pH when small quantities of an acid or a base are added. This is typically achieved by using a weak acid and its conjugate base or a weak base and its conjugate acid.
- A common misunderstanding is that any mixture of salt and an acid/base can form a buffer solution. In reality, specific ratios and components are necessary for a buffer to be effective. For example, a buffer system involving acetic acid (\(<\text{CH}_3\text{COOH}>\)) and sodium acetate (\(<\text{CH}_3\text{COONa}>\)) works because they form a conjugate acid-base pair.
- Hence, Statement I is false because it oversimplifies and inaccurately describes the conditions under which a buffer solution can be formed.
Statement (II): "Blood is a naturally occurring buffer solution whose pH is maintained by \(H_2CO_3/HCO_3^-\) concentrations."
- Blood maintains its pH primarily through the \( \text{H}_2\text{CO}_3/\text{HCO}_3^- \) buffer system. This system helps stabilize the pH around 7.4, which is critical for physiological processes.
- Carbonic acid (\( \text{H}_2\text{CO}_3 \)) and bicarbonate (\( \text{HCO}_3^- \)) act as a conjugate acid-base pair that can neutralize excess acids or bases introduced into the bloodstream.
- Therefore, Statement II is true as it correctly describes the biological buffer system in blood.
In conclusion, after analyzing both statements:
- Statement I is false as it incorrectly describes the requirements for a buffer solution.
- Statement II is true because it accurately explains the role of the \( \text{H}_2\text{CO}_3/\text{HCO}_3^- \) system in maintaining blood pH.
Correct Answer: Statement I is false but Statement II is true
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