Step 1: Understanding the Concept:
The pH of a solution is defined as the negative base-10 logarithm of its hydrogen ion concentration \([\text{H}^+]\). Conversely, the \([\text{H}^+]\) can be found by taking the antilogarithm of the negative pH.
Step 2: Key Formula or Approach:
\[ \text{pH} = -\log_{10}[\text{H}^+] \]
\[ [\text{H}^+] = 10^{-\text{pH}} \]
Step 3: Detailed Explanation:
Given \(\text{pH} = 3.76\).
\[ [\text{H}^+] = 10^{-3.76} \]
To calculate this without a calculator, we write:
\[ [\text{H}^+] = 10^{(0.24 - 4)} = 10^{0.24} \times 10^{-4} \]
The antilog of $0.24$ is approximately $1.738$.
Thus, \([\text{H}^+] = 1.738 \times 10^{-4}\text{ moldm}^{-3}\).
Comparing with options, this matches option B.
Step 4: Final Answer:
The concentration is \(1.738 \times 10^{-4}\text{ moldm}^{-3}\).