Bases feel slippery due to the saponification of skin oils.
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Reference sources confirm that alkaline solutions such as sodium hydroxide and bleach feel slippery upon skin contact due to the saponification of natural skin oils.
defatting and saponification of skin oils and destruction of tissue. The slippery feel of bleach on the skin is due to this process. Contact of sodium hypochlorite
Sodium hypochlorite is an alkaline inorganic chemical compound with the formula NaOCl (also written as NaClO). It is commonly known in a dilute aqueous solution as bleach or chlorine bleach. It is the sodium salt of hypochlorous acid, consisting of sodium cations (Na+) and hypochlorite anions (−OCl, also written as OCl− and ClO−).
The anhydrous compound is unstable and may decompose explosively. I
HOCl(aq) ⇌ H+ + OCl−
HOCl(aq) + Cl− + H+ ⇌ Cl2(aq) + H2O
Cl2(aq) + Cl− ⇌ Cl−3
Cl2(aq) ⇌ Cl2(g)
The second equilibrium equation above will be shifted to the right if the chlorine Cl2 is allowed to escape as gas. The ratios of Cl2, HOCl, and OCl− in solution are also pH dependent. At pH below 2, the majority of the chlorine in the solution is in the form of dissolved elemental Cl2. At pH greater than 7.4, the majority is in the form of hypochlorite ClO−. The equilibrium can be shifted by adding acids (such as hydrochloric acid) or bases (such as sodium hydroxide) to the solution:
solutions, it feels slippery with skin contact due to the process of saponification that occurs between NaOH and natural skin oils. Concentrated (50%)
Sodium hydroxide, also known as caustic soda and, more generically, as lye, is an inorganic compound with the formula NaOH. It is a white solid ionic compound consisting of sodium cations Na+ and hydroxide anions OH−. As a strong nucleophile, it is frequently used in SN2 reactions.
Sodium hydroxide is a highly corrosive base and alkali that decomposes lipids and proteins at ambient temperatures, a
Sodium hydroxide, also known as caustic soda and, more generically, as lye, is an inorganic compound with the formula NaOH. It is a white solid ionic compound consisting of sodium cations Na+ and hydroxide anions OH−. As a strong nucleophile, it is frequently used in SN2 reactions.
Sodium hydroxide is a highly corrosive base and alkali that decomposes lipids and proteins at ambient temperatures, and may cause severe chemical burns at high concentrations. It is highly soluble in water, and readily absorbs moisture and carbon dioxide from the air. It forms a series of hydrates NaOH·nH2O. The monohydrate NaOH·H2O crystallizes from water solutions between 12.3 and 61.8 °C. The commercially available "sodium hydroxide" is often this monohydrate, and published data may refer to it instead of the anhydrous compound.
As one of the simplest hydroxides, sodium hydroxide is frequently used…
OH−(aq) + H+(aq) → H2O(l)
This type of reaction with a strong acid releases heat, and hence is exothermic. Such acid–base reactions can also be used for titrations. However, sodium hydroxide is not used as a primary standard because it is hygroscopic and absorbs carbon dioxide from air.
4 Fe + 6 NaOH → 2 Fe2O3 + 6 Na + 3 H2
A few transition metals, however, may react quite vigorously with sodium hydroxide under milder conditions.
In 1986, an aluminium road tanker in the UK was mistakenly used to transport 25% sodium hydroxide solution, causing pressurization of the contents and damage to tankers. The pressurization is due to the hydrogen gas which is produced in the reaction between sodium hydroxide and aluminium:
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