Read the given statements and mark the correct option.
Statement 1 : If a solution having pH `= 3` is diluted `100` times, its pH increases to `5`.
Statement 2 : For an acidic solution, `[H^(+)] gt 10^(-7)" mol L"^(-1)`

Options

A. Both statements 1 and 2 are true and statement 2 is the correct explanation of statement 1.
B. Both statements 1 and 2 are true but statement 2 is not the correct explanation of statement 1.
C. Statement 1 is true but statement 2 is false.
D. Both statements 1 and 2 are false.

Explanation

To solve the question, we need to evaluate the two statements provided and determine their correctness.

### Step-by-Step Solution:

**Step 1: Analyze Statement 1**
Statement 1 claims that if a solution with a pH of 3 is diluted 100 times, its pH increases to 5.
- The pH is defined as:
\[ \text{pH} = -\log[H^+] \]
where \([H^+]\) is the concentration of hydrogen ions in moles per liter.

- A solution with a pH of 3 has a hydrogen ion concentration of:
\[ [H^+] = 10^{-3} \, \text{mol/L} \]

- When this solution is diluted 100 times, the new concentration of hydrogen ions becomes:
\[ [H^+] = \frac{10^{-3}}{100} = 10^{-5} \, \text{mol/L} \]

- Now, we can calculate the new pH after dilution:
\[ \text{pH} = -\log(10^{-5}) = 5 \]

- Therefore, Statement 1 is **true**.

**Step 2: Analyze Statement 2**
Statement 2 states that for an acidic solution, \([H^+] > 10^{-7} \, \text{mol/L}\).
- The neutral pH of water is 7, which corresponds to a hydrogen ion concentration of:
\[ [H^+] = 10^{-7} \, \text{mol/L} \]

- If the concentration of hydrogen ions is greater than \(10^{-7} \, \text{mol/L}\), the solution is indeed acidic. Thus, Statement 2 is also **true**.

**Step 3: Determine the relationship between the statements**
- While both statements are true, Statement 2 does not explain Statement 1. Statement 1 is about the effect of dilution on pH, while Statement 2 simply defines what makes a solution acidic.

### Conclusion:
- Statement 1 is true.
- Statement 2 is true but does not explain Statement 1.

### Final Answer:
Both statements are correct, but Statement 2 is not the correct explanation for Statement 1.

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