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Nitrous acid (molecular formula H N O 2) is a weak and monoprotic acid known only in solution, in the gas phase, and in the form of nitrite (NO − 2) salts. [3] It was discovered by Carl Wilhelm Scheele, who called it "phlogisticated acid of niter". Nitrous acid is used to make diazonium salts from amines.
For example, acetic acid is a weak acid which has a = 1.75 x 10 −5. Its conjugate base is the acetate ion with K b = 10 −14 /K a = 5.7 x 10 −10 (from the relationship K a × K b = 10 −14), which certainly does not correspond to a strong base. The conjugate of a weak acid is often a weak base and vice versa.
There are two possible structures of hyponitrous acid, trans and cis.trans-Hyponitrous acid forms white crystals that are explosive when dry.In aqueous solution, it is a weak acid (pK a1 = 7.21, pK a2 = 11.54), [2] and decomposes to nitrous oxide and water with a half life of 16 days at 25 °C at pH 1–3:
Nitrite is the conjugate base of the weak acid nitrous acid: HNO 2 ⇌ H + + NO − 2; pK a ≈ 3.3 at 18 °C [3] Nitrous acid is also highly unstable, tending to disproportionate: 3 HNO 2 (aq) ⇌ H 3 O + + NO − 3 + 2 NO. This reaction is slow at 0 °C. [2]
On the other hand, if a chemical is a weak acid its conjugate base will not necessarily be strong. Consider that ethanoate, the conjugate base of ethanoic acid, has a base splitting constant (Kb) of about 5.6 × 10 −10, making it a weak base. In order for a species to have a strong conjugate base it has to be a very weak acid, like water.
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