Question:
The [H\(^+\)] of 0.1 N acetic acid solution is $1.33 \times 10^{-3}$.
The pH of the solution (correct to two decimal places) is ..........
The [H\(^+\)] of 0.1 N acetic acid solution is $1.33 \times 10^{-3}$.
The pH of the solution (correct to two decimal places) is ..........
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Always separate scientific notation: $\log(a \times 10^b) = \log a + b$.
Updated On: Dec 14, 2025
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Correct Answer: 2.86
Solution and Explanation
Step 1: Use the pH formula.
\[ \text{pH} = -\log [\mathrm{H}^+] \] Step 2: Substitute the given value.
\[ \text{pH} = -\log(1.33 \times 10^{-3}) \] \[ = -(\log 1.33 - 3) = - (0.123 - 3) = 2.877 \approx 2.88 \] Step 3: Conclusion.
Thus, the pH = 2.88.
\[ \text{pH} = -\log [\mathrm{H}^+] \] Step 2: Substitute the given value.
\[ \text{pH} = -\log(1.33 \times 10^{-3}) \] \[ = -(\log 1.33 - 3) = - (0.123 - 3) = 2.877 \approx 2.88 \] Step 3: Conclusion.
Thus, the pH = 2.88.
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