Question:
Calculate the pH of a \(0.001\,\text{M}\) solution of \(HNO_3\).
Calculate the pH of a \(0.001\,\text{M}\) solution of \(HNO_3\).
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For strong acids, assume complete dissociation. If \([H^+] = 10^{-n}\), then \(pH = n\).
Updated On: Apr 22, 2026
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The Correct Option is C
Solution and Explanation
Concept:
The pH of a solution is defined as the negative logarithm of the hydrogen ion concentration in the solution. :contentReference[oaicite:0]{index=0} Nitric acid (\(HNO_3\)) is a strong acid and completely dissociates in water, producing hydrogen ions.
Step 1: Write the concentration of hydrogen ions. Since \(HNO_3\) is a strong acid, \[ [H^+] = 0.001 = 10^{-3} \]
Step 2: Substitute into the pH formula. \[ pH = -\log(10^{-3}) \]
Step 3: Calculate the value. \[ pH = 3 \] Hence, \[ \boxed{pH = 3} \]
The pH of a solution is defined as the negative logarithm of the hydrogen ion concentration in the solution. :contentReference[oaicite:0]{index=0} Nitric acid (\(HNO_3\)) is a strong acid and completely dissociates in water, producing hydrogen ions.
Step 1: Write the concentration of hydrogen ions. Since \(HNO_3\) is a strong acid, \[ [H^+] = 0.001 = 10^{-3} \]
Step 2: Substitute into the pH formula. \[ pH = -\log(10^{-3}) \]
Step 3: Calculate the value. \[ pH = 3 \] Hence, \[ \boxed{pH = 3} \]
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