Determine the ph
[OH-] = 2.6×10^-7 M
Express your answer using two decimal places
To determine the pH, we can use the relationship between [OH-] and [H+]:
[H+] = Kw / [OH-]
Where Kw is the ion product of water, which is equal to 1.0 x 10^-14 at 25°C.
[H+] = (1.0 x 10^-14) / (2.6 x 10^-7)
= 3.846 x 10^-8
Then, we can calculate the pH using the formula:
pH = -log10[H+]
pH = -log10(3.846 x 10^-8)
= 7.41
Therefore, the pH is 7.41.
To determine the pH given the hydroxide ion concentration [OH-], we can use the formula:
pOH = -log[OH-]
First, calculate the pOH using the given [OH-]:
pOH = -log(2.6×10^-7) ≈ 6.59
Next, we can use the relation between pH and pOH:
pH + pOH = 14
Substitute the calculated pOH into the equation:
pH + 6.59 = 14
Solve for pH:
pH = 14 - 6.59 ≈ 7.41
Therefore, the pH is approximately 7.41.
To determine the pH given the hydroxide ion concentration [OH-], you can use the equation:
pOH = -log[OH-]
First, let's calculate the pOH using the given hydroxide ion concentration:
pOH = -log(2.6×10^-7) ≈ 6.59
Since pH + pOH = 14 (at 25 °C), we can find the pH by subtracting the pOH value from 14:
pH = 14 - 6.59 ≈ 7.41
So, the pH is approximately 7.41.