객관식
Calculate the pH of 50.00 mL of 4.3 x 10-7 M H2SO4.
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17. Acid and Base Equilibrium
The pH Scale
객관식
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
검증된 단계별 안내1
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.
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