pOH is the negative log of the OH- concentration. It is also related to pH by pH + pOH = 14.
pH + pOH = 14. So pOH = 14 - 1.12 = 12.88 pOH = -log[OH-] [OH-] = 1.31 x 10-13 M
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
An acidic solution will have a pOH ranging from 7 to 14
The pOH is 6,4.
pH + pOH = 14. So pOH = 14 - 6 = 8 pOH = -log[OH-] [OH-] = 10-8 M
pH= -log[H+] pH + pOH = 14 pOH = 14 - pH pOH= -log[OH], so the antilog of -pOH will give you the OH concentration.
If your given pH or pOH, you can also find [H+] or [OH-] use antilog
12.85 is the pOH.
[OH-] = 3.31 log[OH-] = pOH = .51982 14-pOH = pH = 13.48
The pOH is the negative log of the OH- concentration. Thus, pOH = -log 2.0x10^-2pOH = 1.699 = 1.7
The pOH is the negative log of the OH- concentration. Thus, pOH = -log 2.0x10^-2pOH = 1.699 = 1.7