Multiple Choice
Calculate the concentration of OH⁻ in a 0.01 M HCl solution at 25 °C, and classify the solution as acidic or basic.
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17. Acid and Base Equilibrium
pH of Strong Acids and Bases
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Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Calculate the pH of a 0.012 M solution of HCl, a strong acid.
A
2.08
B
3.00
C
1.92
D
0.92
Verified step by step guidance1
Understand that HCl is a strong acid, meaning it completely dissociates in water. Therefore, the concentration of hydrogen ions [H⁺] is equal to the concentration of HCl.
Identify the concentration of HCl given in the problem, which is 0.012 M. This is also the concentration of hydrogen ions [H⁺] in the solution.
Recall the formula for calculating pH: \( \text{pH} = -\log[\text{H}^+] \). This formula is used to find the pH from the concentration of hydrogen ions.
Substitute the concentration of hydrogen ions [H⁺] into the pH formula: \( \text{pH} = -\log(0.012) \).
Use a calculator to evaluate the logarithm and find the pH value. Remember that the pH scale is logarithmic, so even small changes in concentration can lead to significant changes in pH.
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