Determine the pH of a 2.8 ×10−4 M solution of Ca(OH)2. September 2, 2021 by Tài Đức Determine the pH of a 2.8 ×10−4 M solution of Ca(OH)2.
Answer: pH = 10.75 Explanation: To solve this problem, we must find the molarity of [OH⁻]. With the molarity we can find the pOH = -log[OH⁻] Using the equation: pH = 14 – pOH We can find the pH of the solution. The molarity of Ca(OH)₂ is 2.8×10⁻⁴M, as there are 2 moles of OH⁻ in 1 mole of Ca(OH)₂, the molarity of [OH⁻] is 2*2.8×10⁻⁴M = 5.6×10⁻⁴M pOH is pOH = -log 5.6×10⁻⁴M pOH = 3.25 pH = 14-pOH pH = 10.75 Reply
Answer:
pH = 10.75
Explanation:
To solve this problem, we must find the molarity of [OH⁻]. With the molarity we can find the pOH = -log[OH⁻]
Using the equation:
pH = 14 – pOH
We can find the pH of the solution.
The molarity of Ca(OH)₂ is 2.8×10⁻⁴M, as there are 2 moles of OH⁻ in 1 mole of Ca(OH)₂, the molarity of [OH⁻] is 2*2.8×10⁻⁴M = 5.6×10⁻⁴M
pOH is
pOH = -log 5.6×10⁻⁴M
pOH = 3.25
pH = 14-pOH
pH = 10.75