Multiple Choice
What is the pH of a solution made by mixing 0.30 mol of NaOH, 0.25 mol of Na2HPO4, and 0.20 mol of H3PO4 with water and diluting to 1.00 L?
17. Acid and Base Equilibrium
pH of Strong Acids and Bases
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What is the pH of a 0.040 M Ba(OH)_2 solution?
A
12.60
B
1.40
C
2.70
D
13.30
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⁻ ions will be twice the concentration of Ba(OH)_2. Use the formula: [OH⁻] = 2 × [Ba(OH)_2].
Use the concentration of OH⁻ ions to find the pOH of the solution. The pOH is calculated using the formula: pOH = -log[OH⁻].
Convert the pOH to pH. Remember that pH and pOH are related by the equation: pH + pOH = 14. Use this relationship to find the pH: pH = 14 - pOH.
Review the calculated pH value and compare it to the given options to ensure it matches one of the provided answers.
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