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?
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17. Acid and Base Equilibrium
pH of Strong Acids and Bases
Multiple Choice
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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