Statement-1: pH value of acidic buffer solution changes , If buffer solution is diluted upto very large extent.
Statement-2: `[H^(+)]` decreases due to change in concentration as well as `alpha` increases and decreases in concentration is more as compared to increases in `alpha` .

Options

A. If both the statements are TRUE and STATEMENT-2 is the correct explanation of STATEMENT-1
B. If both the statements are TRUE AND STATEMENT-2 is NOT the correct explanation of STATEMENT-1
C. If STATEMENT-1 is TRUE and STATEMENT-2 is FALSE
D. If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Answer

To solve the question, we need to analyze both statements and determine their validity and relationship.

### Step 1: Analyze Statement 1
**Statement 1:** "pH value of acidic buffer solution changes if buffer solution is diluted up to very large extent."

- **Explanation:** An acidic buffer solution is typically made from a weak acid and its salt. The pH of a buffer solution is given by the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pKa} + \log\left(\frac{[\text{Salt}]}{[\text{Acid}]}\right) \]
- When the buffer solution is diluted, the concentrations of both the weak acid and its salt decrease. However, the ratio of salt to acid concentration may remain relatively constant if both are diluted equally.

- However, if the dilution is extreme, the weak acid may dissociate more, leading to an increase in the concentration of H⁺ ions, but this increase is minimal compared to the overall decrease in concentration due to dilution.

- Therefore, the pH will change upon significant dilution. Thus, Statement 1 is **true**.

### Step 2: Analyze Statement 2
**Statement 2:** "[H⁺] decreases due to change in concentration as well as α increases and decrease in concentration is more as compared to increase in α."

- **Explanation:** The degree of dissociation (α) of a weak acid is very small. When the buffer is diluted, the concentration of the weak acid decreases, which leads to a decrease in the concentration of H⁺ ions.

- Although dilution can cause an increase in α (the degree of dissociation), this increase is not sufficient to offset the decrease in concentration of H⁺ ions due to dilution.

- Therefore, the overall concentration of H⁺ ions decreases, leading to an increase in pH. Thus, Statement 2 is also **true**.

### Step 3: Relationship Between Statements
- Statement 2 provides an explanation for Statement 1. The decrease in [H⁺] due to dilution and the weak acid's low degree of dissociation (α) explains why the pH of the buffer changes upon dilution.

### Conclusion
Both statements are true, and Statement 2 is the correct explanation for Statement 1.

### Final Answer
Both statements are true, and Statement 2 is the correct explanation of Statement 1.

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