Answer:
6.5
Explanation:
Since pure water is neutral, the hydrogen ion concentration equals the hydroxide ion concentration.
[H⁺] = [OH⁻] and pK = pH + pOH. Since [H⁺] = [OH⁻], pH = -log[H⁺] = pOH = -log[OH⁻].
So, pK = 2pH and K = ionisation constant for water at 60 °C = 9.6 × 10⁻¹⁴
pH = pK/2 = -logK/2 = - log(9.6 × 10⁻¹⁴)/2 = (14 - log9.6)/2 = 6.5
So, pH of water at 60 °C is 6.5
Answer:
Explanation:
H2O --> H+ + OH-
Ka = [H+][OH-]/[H2O]
Ka × [H2O] = Kw
Kw = [H+] × [OH-]
[H+] = [OH-] = x
Therefore,
9.6 x 10^-14 = x^2
x = 3.098 × 10^-7
[H+] = 3.098 × 10^-7 M
pH = -log[H+]
= -log [3.098 × 10^-7]
= 6.51
