2006-06-20 22:27:49 · 3 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
Sodium Hypochlorite can exist at any pH that is on the "basic" side of neutral. Having said that, most commercial sodium hypochlorite solution (read "Liquid Pool Chlorine") is stabilised by the addition of sodium hydroxide and so has a pH between 11 and 12.
2006-06-20 23:45:13 · answer #1 · answered by Bruce H 3 · 0⤊ 0⤋
Sodium hypochlorite, commonly known as the household "beach" is a weak base and will have a pH of greater than 7, however the exact pH varies, depending on the concentration of the NaClO.
Sodium hypochlorite acts as a base because once it is in water, its anion (ClO-) will accept a H+ from the water to from OH- in the solution, as shown in equation below.
ClO- + H2O --> HClO + OH-
Then, use:
Kb = [HClO][OH-]/[ClO-]
To figure out the [OH-]
Then you can use [H+] = (1 x 10^-14)/[OH-] to figure out concentration of proton (or Hydronium).
Then use pH = -log[H+] to figure out the exact pH for the given concentration of sodium hypochlorite.
2006-06-20 22:29:26 · answer #2 · answered by †ђ!ηK †αηK² 6 · 0⤊ 0⤋
Sodium Hypochlorite is an IONIC COMPOUND.
2006-06-20 22:29:55 · answer #3 · answered by Anonymous · 0⤊ 1⤋