What is the pH of a 0.01 M solution of hydrochloric acid (HCl)?
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For strong acids, the pH is calculated directly from the concentration of the acid since they dissociate completely. Use the formula \( \text{pH} = -\log [\text{H}^+] \).
Step 1: Characterize the acid.
Hydrochloric acid (HCl) is classified as a strong acid. This indicates that it undergoes complete dissociation in aqueous solution:
\[
\text{HCl} \rightarrow \text{H}^+ + \text{Cl}^-
\]
Step 2: Determine the hydrogen ion concentration.
Due to the complete dissociation of HCl, the molar concentration of hydrogen ions \( [\text{H}^+] \) is equivalent to the initial molar concentration of the acid:
\[
[\text{H}^+] = 0.01 \, \text{M}
\]
Step 3: Apply the pH definition.
The pH of a solution is mathematically defined as:
\[
\text{pH} = -\log [\text{H}^+]
\]
By substituting the calculated hydrogen ion concentration:
\[
\text{pH} = -\log (0.01) = 2
\]
Answer: The resultant pH of the solution is 2.
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