The [H+] of a 100 mM solution of KOH can be calculated using the equation pH = -log[H+]. Since KOH is a strong base, it will dissociate completely in water to form OH- ions. Therefore, the [H+] will be equal to the concentration of OH- ions, which is 100 mM. This results in a pH of 14, which is highly basic.
The pH of a 100 mM solution of KOH can be calculated using the equation pH = -log[H+]. Since KOH is a strong base, it will dissociate completely in water to form OH- ions. Therefore, the pH will be equal to 14, which is highly basic.
The higher the concentration of KOH, the higher the concentration of OH- ions in the solution. This leads to an increase in the [H+] and pH of the solution. For example, a 200 mM solution of KOH will have a [H+] of 200 mM and a pH of 14.
A 100 mM solution of KOH is considered basic because it has a pH of 14. pH values below 7 are considered acidic, while pH values above 7 are considered basic.
The pH of a 100 mM solution of KOH can be adjusted by adding an acid, such as HCl, to neutralize the excess OH- ions. This will result in a decrease in the [H+] and a decrease in the pH of the solution. Alternatively, the pH can also be adjusted by diluting the solution with water, which will decrease the concentration of KOH and therefore decrease the [H+] and pH.