[H+] = Kw / [OH-] = 1.0*10-14 / 2.5*10-4 = 4.0*10-11 mol/L
solution with [OH-] = 2.5 x 10-9 , A solution with [H+] = 1.2 x 10-4, A solution with pH = 4.5
Na+ plus OH- plus H+ equals H2O plus Na+ plus Cl-
If -h = 14, then ... h = -14
(OH- is a base) (H+ is an acid) Therefore by adding water to HSO3, the OH- ion is produced therefore it is an Arrhenius base.
[H+] = Kw / [OH-] = 1.0*10-14 / 2.5*10-4 = 4.0*10-11 mol/L
solution with [OH-] = 2.5 x 10-9 , A solution with [H+] = 1.2 x 10-4, A solution with pH = 4.5
Na+ plus OH- plus H+ equals H2O plus Na+ plus Cl-
h = 0.538462 14 + 5h + 2h = 5h + 28h 14 + 7h = 33h 14 + 7h - 7h = 33h - 7h 14 = 26h 14/26 = 26/26h 0..538462 = h
The sum of pH and pOH is always equal to 14 in a neutral solution at 25°C. This is because pH is a measure of the concentration of H+ ions in a solution while pOH is a measure of the concentration of OH- ions. In a neutral solution, the concentration of H+ ions is equal to the concentration of OH- ions, resulting in a sum of 14.
If -h = 14, then ... h = -14
(OH- is a base) (H+ is an acid) Therefore by adding water to HSO3, the OH- ion is produced therefore it is an Arrhenius base.
H+ or a proton.
The pH of a neutral solution with equal concentrations of H+ and OH- ions is 7. This is because the concentration of H+ ions equals the concentration of OH- ions in a neutral solution, resulting in a pH of 7.
If the concentration of H+ is 0.0020 M, the concentration of OH- can be calculated using the equation Kw = [H+][OH-]. Since Kw is a constant (1.0 x 10^-14 at 25°C), you can rearrange the equation to find the concentration of OH-. In this case, [OH-] = Kw / [H+] = 1.0 x 10^-14 / 0.0020 = 5.0 x 10^-12 M.
The concentration of OH- decreases as the concentration of H+ increases. This is beacause there is an equilibrium H2O <-> H+ + OH- and therefore the [H+][OH-] is a constant
To find the [H+] concentration in a solution with a pOH of 0.253, you first need to find the pOH of the solution which is 14 - pOH = 14 - 0.253 = 13.747. Then, you can use the relation [H+][OH-] = 1.0 x 10^-14 to calculate the [H+] concentration. [H+] = 10^-13.747 = 1.93 x 10^-14 M.