Determine the ph
[OH-] = 2.6×10-7 M
Express your answer using two decimal places.
To find the pH, we can use the formula:
pH = -log[H+]
Since [H+] = [OH-], we can use the concentration of [OH-] to determine the concentration of [H+].
[H+] = 2.6×10^-7 M
Taking the negative logarithm of the concentration:
pH = -log(2.6×10^-7)
≈ 6.59
Therefore, the pH is approximately 6.59.
To determine the pH, we can use the formula:
pOH = -log[OH-]
Given that [OH-] = 2.6×10-7 M, we can substitute this value into the formula:
pOH = -log(2.6×10-7)
Using a calculator, we find:
pOH ≈ 6.59
Since pH + pOH = 14, we can subtract the pOH value from 14 to find the pH:
pH ≈ 14 - 6.59
pH ≈ 7.41
Therefore, the pH is approximately 7.41.
To determine the pH, we need to use the relationship between the concentration of hydroxide ions ([OH-]) and the concentration of hydrogen ions ([H+]) in a solution. This relationship is defined by the equation:
pH = -log [H+]
Given that [OH-] = 2.6×10^-7 M, we can use the concept of Kw (the ionization constant of water) to find [H+]. In water, at 25°C, Kw = [H+][OH-] = 1.0 x 10^-14.
Rearranging the equation, we can solve for [H+]:
[H+] = Kw / [OH-]
[H+] = (1.0 x 10^-14) / (2.6 x 10^-7)
Calculating this expression, we find [H+] = 3.85 x 10^-8 M.
Now, to find the pH, we substitute this value into the equation:
pH = -log [H+]
pH = -log (3.85 x 10^-8)
Using a calculator, we can determine that the pH is approximately 7.41 (rounded to two decimal places).