Question

PH = 10.88
what is the OH-

Answer 1

The pH of a solution is defined as the negative logarithm (base 10) of the concentration of hydrogen ions [H+]. The concentration of hydroxide ions [OH-] can be calculated using the equation Kw = [H+][OH-], where Kw is the ion product constant for water, which is equal to 1.0 × 10^-14 at 25°C.

To find the [OH-] of a solution with pH 10.88, we first find the [H+]:

pH = -log[H+]

10.88 = -log[H+]

[H+] = 10^(-10.88) = 1.4 × 10^(-11) M

Now we can calculate the [OH-]:

Kw = [H+][OH-]

1.0 × 10^-14 = (1.4 × 10^-11)[OH-]

[OH-] = (1.0 × 10^-14) / (1.4 × 10^-11) = 7.1 × 10^-4 M

Therefore, the [OH-] of the solution is 7.1 × 10^-4 M.

Step-by-step explanation:

Answer 2

The concentration of hydroxide ions (OH-) in a solution with a given pH can be calculated using the formula [OH-] = 10^-pOH. In this case, the pH is 10.88, so the concentration of OH- is 7.74 x 10^-4 M.

Step-by-step explanation:

pH is a measure of the acidity or basicity of a solution. In this case, the given pH is 10.88. To find the concentration of hydroxide ions (OH-), we can use the formula:

[H3O+] = 10^-pH

Therefore, [H3O+] = 10^-10.88 = 1.5 x 10^-11 M. Since pH + pOH = 14, we can calculate the pOH as:

pOH = 14 - pH = 14 - 10.88 = 3.12

Finally, we can find the concentration of OH- using the formula:

[OH-] = 10^-pOH = 10^-3.12 = 7.74 x 10^-4 M