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.