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1.79x10^-14 M
If an aqueous solution has a pOH value of 10.7 and is at standard temperature and pressure, the pH value is 14 - 10.7 = 3.3. From the definition of pH, this means that the logarithm (to base 10) of the molar concentration of H+, [H+] is -3.3. This can be written as +0.7 - 4. The antilog of 0.7 is 5, to the justified number of significant digits. Therefore, [H+] = 5 X 10-4.
ONLY in pure water at 25 0C :pH + pOH = 14.00
pH is defined as -log[H+]. This means that if one knows the concentration of hydrogen ion in solution, the pH is simply the negative logarithm (base 10) of that. Similarly, one can find the pOH simply by substituting the concentration of OH- for the concentration of H+ in the aforementioned formula.
We can subtract pOH from 14, using the formula pH + pOH = 14. This is only true at 14 degrees Celsius.
7.5
5.6
pH + pOH = 14 If the pH is 3.4, the pOH is 10.6
The pOH is 5,23.
7.8
pOH = -log(10)[OH^-] pOH = -log(10) [ 48. x 10^-2] pOH = - (-1.31875...) pOH = 1.31875... pH = 14 - pOH pH = 14 - 1.31875... pH = 12.68124... pH = 12.68
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
The pOH is the negative log of the OH- concentration. Thus, pOH = -log 2.0x10^-2pOH = 1.699 = 1.7
1.79x10^-14 M
By definition pH = -log[H+], so pH = -log(4.9*10-4) = 3.31Only at 25oC: pOH = 14.00 - pH, so 14.00 - 3.31 = 10.69 = pOH
A solution with [H+] = 1.1 x 10-7 A solution with pOH = 10.1
If an aqueous solution has a pOH value of 10.7 and is at standard temperature and pressure, the pH value is 14 - 10.7 = 3.3. From the definition of pH, this means that the logarithm (to base 10) of the molar concentration of H+, [H+] is -3.3. This can be written as +0.7 - 4. The antilog of 0.7 is 5, to the justified number of significant digits. Therefore, [H+] = 5 X 10-4.