What is (a)PH(b) POH of a solution wholes hydrogen ion consentration is 5.00x10-4?
pH = -log(H^+) and pOH from
pH + pOH = pKw = 14.
Pls help me answer this question
Calculated the pH and POH of 5.00×10^-4 hydrogen of the concentration solution
To find the pH and pOH of a solution with a given hydrogen ion concentration, you can use the formulas:
pH = -log[H+]
pOH = -log[OH-]
We are given the hydrogen ion concentration as 5.00x10-4.
Step 1: Calculate pH
pH = -log(5.00x10-4)
= -log(5.00) - log(10-4)
≈ -log(5.00) - (-4) (since log(10) = 1 and log(10x) = x for any positive x)
≈ -0.6990 - (-4)
≈ 4 - 0.6990
≈ 3.3010
So the pH of the given solution is approximately 3.3010.
Step 2: Calculate pOH
Since water is neutral, the OH- concentration is equal to the H+ concentration in pure water. This means that the pOH of a solution can be calculated using the following equation:
pOH = 14 - pH
pOH = 14 - 3.3010
≈ 10.6990
So the pOH of the given solution is approximately 10.6990.