Multiple Choice
What is the pH of a solution of , assuming it is a strong acid that dissociates completely in water?
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17. Acid and Base Equilibrium
pH of Strong Acids and Bases
Multiple Choice
What is the pH of a M solution at ? (Assume is a strong acid and fully dissociates.)
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Verified step by step guidance1
Recognize that HCl is a strong acid and fully dissociates in water, so the concentration of H\(\textsuperscript{+}\) ions is equal to the initial concentration of HCl, which is 0.00125 M.
Write the expression for pH, which is defined as the negative logarithm (base 10) of the hydrogen ion concentration: \(\text{pH} = -\log[\text{H}^+]\).
Substitute the concentration of H\(\textsuperscript{+}\) ions into the pH formula: \(\text{pH} = -\log(0.00125)\).
Calculate the logarithm value (without giving the final number here) to find the pH.
Interpret the pH value to understand the acidity of the solution; since the concentration is low but still acidic, the pH should be greater than 1 but less than 7.
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