Question:
Calculate the pH of a \(0.01\,M\) \(HCl\) solution.
Calculate the pH of a \(0.01\,M\) \(HCl\) solution.
Show Hint
For strong acids, assume complete dissociation.
Thus, the hydrogen ion concentration equals the molarity of the acid.
Updated On: Apr 29, 2026
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The Correct Option is B
Solution and Explanation
Concept:
The pH of a solution is defined as
\[
pH = -\log[H^+]
\]
For strong acids like \(HCl\), the acid completely dissociates in water.
Step 1: Determine the hydrogen ion concentration. Since \(HCl\) is a strong acid, \[ [H^+] = 0.01\,M \] \[ [H^+] = 10^{-2} \]
Step 2: Apply the pH formula. \[ pH = -\log[H^+] \] \[ pH = -\log(10^{-2}) \]
Step 3: Evaluate the value. \[ pH = 2 \]
Step 1: Determine the hydrogen ion concentration. Since \(HCl\) is a strong acid, \[ [H^+] = 0.01\,M \] \[ [H^+] = 10^{-2} \]
Step 2: Apply the pH formula. \[ pH = -\log[H^+] \] \[ pH = -\log(10^{-2}) \]
Step 3: Evaluate the value. \[ pH = 2 \]
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