What is the [OH⁻] (hydroxide concentration) of that same solution? (pH = 4.00)

Answer: 1 x 10^-10M

Explanation:

Given that,

pOH of solution = ?

pH of solution = 4.00

Recall that pH is the negative logarithm of hydrogen ion concentration in the solution while pOH is the negative logarithm of hydroxide ion concentration in the solution.

Hence, pH + pOH = 14

4.00 + pOH = 14

pOH = 14 - 4.00

pOH = 10

Apply the formula pOH = - log (OH-) to get [OH⁻]

10 = - log (OH-)

(OH-) = Antilog (-10)

(OH-) = 1 x 10^-10M

Thus, 1 x 10^-10M is the [OH⁻] (hydroxide concentration) of that same solution with pH value of 4.00