Why is it unsafe to acid to bleach?

Question

If you don't know the answer to this question then you better google it fast. When acid is added to bleach it breaks down and one of the products of it is chlorine gas, which is extremely dangerous and deadly.

2HOCl + 2HAc ↔ Cl2↑ + 2H2O + 2Ac

this inst really a question. i made for informational purposes.

Answer 1

You equation is not correct. Household bleach contains Sodium hypochlorite, which will react with acids (like the acetic acid in vinegar) to give Chlorine gas:

NaOCl + NaCl + 2 HAc --> Cl2↑ + H2O + 2 NaAc

Answer 2

Lancenigo di Villorba (TV), Italy

I AM SORRY, YOU WROTE SOME MISTAKES.
In the past times, I executed several experiments on this reaction and its possible variances.

WHAT IS BLEACH
Bleach is a very common house-hold chemical stuff. Its chemical action interests the "Wear's decoloration", more precisely it acts on common "Cloth's dyes" converting them in its uncoloured forms. On the other hand, it is well-known that it destroy many and many types of micro-organisms, e.g. bacteria and fungi on the others.
Bleach is made starting from an aqueous solutions of sodium hydroxide where it is dissolved sodium chloride and sodium hypochlorite( e.g. respectively NaCl and NaClO). The latter is a very reactive compound, so it exists not in nature.

ABOUT HYPOCHLORITES
Some industrial plants produce hypochlorite salts, so it is employed in "Bleach's making". An electrochemical application is the following :

2 Na+Cl-(aq) + 2 H2O(aq) <---> Cl2(g) + H2(g) + 2 Na+OH-(aq)

where one starts from brine's solutions, so obtaining chlorine and hydrogen gas. The liquid product is sodium hydroxide increasing concentrated by reaction's running.
Instead hypochlorite salts do, chloride salts are the "unactive moieties". In effects, chloride take part to a very smaller reaction's number respect to hypochlorite salts do. The term "active chlorine" interest the analogous role played by hypochlorite salts as chlorine gas do.
Chlorine may react with alkaline solutions, so the alkaline product containts also hypochlorite salts :

Cl2(g) + 2 Na+OH-(aq) <--->
<---> Na+Cl-(aq) + Na+ClO-(aq) + H2O(aq)

CHLORINE's RESCUE
Nonetheless it is prepared in stuffs containing parfum and other essences, you may highlight its "Chlorine's containt".
Hypochlorite salts are related to hypochlorous acid. Since the latter is a very weak acid, you note acidic surrounding leads to "Chlorine bubble" 's evolvement :

Cl-(aq) + ClO-(aq) + 2 H+(aq) <---> Cl2(aq) + 2 H2O(aq)

VINEGAR's ROLE
Vinegar is an aqueous mixture of several organic chemicals. Since it is an acidic stuff, it favours the "Chlorine gas's evolvement". Moreover, among its organic constitutings there are someones reacting with hypochlorite salts. The vinegar you shopped at markets is prepared in industrial plants. The productors put some additives, e.g. sodium hydrogenosulphite NaHSO3, a common reducing agent. The latter belongs to reaction's actors versus hypochlorite ones.
The redox reactions occuring, so chloride ions are formed while hydrogenosulphite ions become sulphate ones ; similarly, chloride ions are formed while organic compounds undergo chemical oxidation.

Finally, acidic surrounding permit the "Chlorine bubble" 's evolvement by chloride/hypochlorite interaction.

I hope this helps you.