If a solution had a pOH equals 10.7 what would be the H plus?

Answer 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.

Answer 2

The pH and pOH of a solution always add up to 14. Therefore, if the pOH is 10.7, the pH would be 3.3. To find the concentration of H+ ions, you would take the antilog of the negative pH value, which is 10^-3.3 or approximately 5 x 10^-4 M.