Multiple Choice
What is the pH of a M solution at ? (Assume is a strong acid and fully dissociates.)
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17. Acid and Base Equilibrium
pH of Strong Acids and Bases
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What is the pH of a M solution at , assuming complete dissociation?
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Verified step by step guidance1
Recognize that HCl is a strong acid and dissociates completely in aqueous solution, so the concentration of H\textsuperscript{+} ions is equal to the initial concentration of HCl, which is 0.0235 M.
Recall the definition of pH, which is given by the formula:
\(\text{pH} = -\log[\text{H}^+]\)
Substitute the concentration of H\textsuperscript{+} ions into the pH formula:
\(\text{pH} = -\log(0.0235)\)
Use logarithm properties or a calculator to find the logarithm value (do not calculate the final number here, just set up the expression).
Interpret the pH value: since the concentration is less than 1 M, the pH will be greater than 0 but less than 7, indicating an acidic solution.
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