pH and pOH are a measure of the concentration of the hydronium ions and hydroxyl ions respectively in the solution.
pH = -log[H+]
pOH = -log[OH-]
and they are related: pH + pOH = 14
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∙ 10y agoIf the pH is 6.00, then the pOH is 8.00 because pH + pOH = 14. pOH = 8.00 = -log[OH-] -8.00 = log[OH-] 10-8.00 = 1 × 10-8 M OH-
The pOH is 6,4.
I will assume you are asking about the pH of pure water if pKw is 14.26. The relationship between pH, pOH, and pKw is as follows: pH + pOH = pKw. If it is pure, neutral water (no acids or bases present), then pH = pOH, so: pH + pOH = 14.26 2(pH) = 14.26 pH = pOH = 7.13
pOH +pH=14 pOH+7.6=14 pOH=(14-7.6)=6.4
A liquid with a pOH of 4 is more acidic. The pOH scale is the inverse of the pH scale, so a lower pOH value corresponds to a higher concentration of hydroxide ions (OH-) and a lower concentration of hydrogen ions (H+). This indicates a higher acidity level.
Yes, if both solutions are at 25oC then in both solutions this is valid: pH + pOH = 14.0
If the pH is 6.00, then the pOH is 8.00 because pH + pOH = 14. pOH = 8.00 = -log[OH-] -8.00 = log[OH-] 10-8.00 = 1 × 10-8 M OH-
pH + pOH =14
The pOH is 6,4.
It will have a pOH of 12. Because pH+pOH=14
pH + pOH =14
pH is -log[H(subscript 3)O+] pOH is the [OH-] pOH = 14 - pH apex
I will assume you are asking about the pH of pure water if pKw is 14.26. The relationship between pH, pOH, and pKw is as follows: pH + pOH = pKw. If it is pure, neutral water (no acids or bases present), then pH = pOH, so: pH + pOH = 14.26 2(pH) = 14.26 pH = pOH = 7.13
pOH +pH=14 pOH+7.6=14 pOH=(14-7.6)=6.4
A liquid with a pOH of 4 is more acidic. The pOH scale is the inverse of the pH scale, so a lower pOH value corresponds to a higher concentration of hydroxide ions (OH-) and a lower concentration of hydrogen ions (H+). This indicates a higher acidity level.
We can subtract pOH from 14, using the formula pH + pOH = 14. This is only true at 14 degrees Celsius.
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