Each `10^(-3)`M of following four acids are taken. Their `P^(H)` values are given in brackets. Which of the following is relatively strong acid?

Options

A. A(3.6)
B. B(4.2)
C. C(5.4)
D. D(6.8)

Answer

To determine which of the four acids is the relatively strong acid based on their given pH values, we can follow these steps:

### Step-by-Step Solution:

1. **Understand pH and H⁺ Concentration**:
The pH of a solution is defined as:
\[ \text{pH} = -\log[H^+] \]
This means that a lower pH value corresponds to a higher concentration of hydrogen ions (H⁺) in the solution.

2. **Identify the pH Values**:
Let's assume the pH values for the four acids are provided as follows (for example):
- Acid A: pH = 2.0
- Acid B: pH = 3.0
- Acid C: pH = 4.0
- Acid D: pH = 5.0

3. **Calculate H⁺ Concentration**:
Using the pH values, we can calculate the concentration of H⁺ ions for each acid:
\[ [H^+] = 10^{-\text{pH}} \]
- For Acid A:
\[ [H^+] = 10^{-2.0} = 0.01 \, M \]
- For Acid B:
\[ [H^+] = 10^{-3.0} = 0.001 \, M \]
- For Acid C:
\[ [H^+] = 10^{-4.0} = 0.0001 \, M \]
- For Acid D:
\[ [H^+] = 10^{-5.0} = 0.00001 \, M \]

4. **Compare H⁺ Concentrations**:
Now, we compare the H⁺ concentrations:
- Acid A: 0.01 M
- Acid B: 0.001 M
- Acid C: 0.0001 M
- Acid D: 0.00001 M

5. **Determine the Strongest Acid**:
The acid with the highest concentration of H⁺ ions is the strongest acid. From our calculations, Acid A has the highest concentration of H⁺ ions (0.01 M), thus it is the strongest acid among the four.

### Conclusion:
Based on the pH values provided, Acid A is the relatively strong acid.