Multiple Choice
What is the pH of a solution at (assume complete dissociation)?
3
views
17. Acid and Base Equilibrium
pH of Strong Acids and Bases
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
What is the pH of an aqueous M HI solution at 25 °C? (Assume HI is a strong acid.)
A
B
C
D
Verified step by step guidance1
Recognize that HI (hydroiodic acid) is a strong acid, which means it completely dissociates in aqueous solution. Therefore, the concentration of H\_3O\^+ ions is equal to the initial concentration of HI.
Write down the concentration of HI given: \$8.5 \times 10^{-3}$ M. This is also the concentration of H\_3O\^+ ions in the solution.
Recall the formula for pH: \(\mathrm{pH} = -\log[\mathrm{H}_3\mathrm{O}^+]\). This formula relates the hydronium ion concentration to the pH of the solution.
Substitute the concentration of H\_3O\^+ into the pH formula: \(\mathrm{pH} = -\log(8.5 \times 10^{-3})\).
Calculate the logarithm and then the negative of that value to find the pH. This will give you the pH of the solution at 25 \degree C.
2:39mWatch next
Master pH of Strong Acids and Bases with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
pH of Strong Acids and Bases practice set
Problem sets built by lead tutorsExpert video explanations