Given the molar concentration of hydrogen ion, calculate the concentration of hydroxide ion [H+]=7.9*10-7
[OH][H] = 10^-14
[OH] = (1/7.9)(10^-14/10^-7)
= .127 * 10^-7
= 1.27 * 10^-8
a bit acidic
To calculate the concentration of hydroxide ion (OH-) from the given molar concentration of hydrogen ion (H+), we can make use of the relationship involving the equilibrium constant for the autoionization of water:
Kw = [H+][OH-]
At 25°C, the value of Kw is constant and equal to 1.0 x 10^-14.
Given [H+] = 7.9 x 10^-7, we can substitute these values into the equation:
1.0 x 10^-14 = (7.9 x 10^-7)[OH-]
Now we can solve for [OH-]:
[OH-] = (1.0 x 10^-14) / (7.9 x 10^-7)
Simplifying the expression:
[OH-] = 1.27 x 10^-8
Therefore, the concentration of hydroxide ion is 1.27 x 10^-8 M.
To calculate the concentration of hydroxide ion (OH-), we can use the relationship between hydrogen ion concentration (H+) and hydroxide ion concentration (OH-) in water. According to the concept of acidity and basicity, in a neutral solution at 25°C, the concentration of hydrogen ions is equal to the concentration of hydroxide ions.
So, if [H+] = 7.9 x 10^-7 mol/L, the concentration of hydroxide ions (OH-) will also be 7.9 x 10^-7 mol/L.
Therefore, the concentration of hydroxide ion [OH-] is 7.9 x 10^-7 mol/L.