Multiple Choice
Calculate the pH of 50.00 mL of 4.3 x 10-7 M H2SO4.
17. Acid and Base Equilibrium
The pH Scale
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 a solution of 0.0350 M Ba(OH)2?
A
1.15
B
1.46
C
12.24
D
12.54
E
12.85
Verified step by step guidance1
Understand that Ba(OH)₂ is a strong base and dissociates completely in water. Each formula unit of Ba(OH)₂ produces two hydroxide ions (OH⁻).
Calculate the concentration of hydroxide ions (OH⁻) in the solution. Since Ba(OH)₂ dissociates into two OH⁻ ions, the concentration of OH⁻ is twice the concentration of Ba(OH)₂. Use the formula: [OH⁻] = 2 × [Ba(OH)₂].
Use the concentration of OH⁻ to find the pOH of the solution. The formula to calculate pOH is: pOH = -log₁₀([OH⁻]).
Convert the pOH to pH using the relationship between pH and pOH: pH + pOH = 14. Rearrange this equation to solve for pH: pH = 14 - pOH.
Verify the calculated pH value against the provided options to ensure it matches the correct answer.
Related Videos
Related Practice
