Multiple Choice
Calculate the concentration of H3O+ in a 0.01 M solution of HCl at 25°C, and classify the solution as acidic or basic.
331
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
Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)₂.
A
pH = 0.70
B
pH = 12.00
C
pH = 13.30
D
pH = 1.00
Verified step by step guidance1
Identify that barium hydroxide, Ba(OH)₂, is a strong base that dissociates completely in water to produce barium ions, Ba²⁺, and hydroxide ions, OH⁻.
Write the balanced dissociation equation for barium hydroxide: Ba(OH)₂ → Ba²⁺ + 2OH⁻.
Determine the concentration of hydroxide ions, OH⁻, produced. Since each formula unit of Ba(OH)₂ produces two OH⁻ ions, the concentration of OH⁻ is twice the concentration of Ba(OH)₂. Therefore, [OH⁻] = 2 × 0.10 M = 0.20 M.
Calculate the pOH of the solution using the formula: pOH = -log[OH⁻]. Substitute the concentration of OH⁻ into the formula to find the pOH.
Convert the pOH to pH using the relationship: pH + pOH = 14. Solve for pH by subtracting the calculated pOH from 14.
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