ka=[H+][NO2_]/[HNO2]
HCN(aq) ==> H^+(aq) + CN^-(aq)Ka = [H+][CN-]/[HCN] and the value can be looked up in a book or on line.
Kb = [CH3NH3 +] [OH-] / [CH3NH2]
The cell notation for the given redox reaction is: Pb₂⁺(aq) | Pb(s) || Cr(s) | Cr³⁺(aq)
A precipitate
ka=[H+][NO2_]/[HNO2]
The Ka for the dissociation of HNO2 is 4.5 x 10^-4. This value represents the equilibrium constant for the reaction of HNO2 dissociating into H+ and NO2-.
Ka= [H+][NO2-] [HNO2]
HCN(aq) ==> H^+(aq) + CN^-(aq)Ka = [H+][CN-]/[HCN] and the value can be looked up in a book or on line.
Nitrous acid in solution can be written as HNO2(aq).
Equilibrium:NO2- (aq) + H2O HNO2 (aq) + OH- (aq)
Hydrogen nitrite acid
3.4 * 10^-8
HNO2 (nitrous acid) in aqueous solution is a weak acid that can dissociate into a hydrogen ion (H+) and nitrite ion (NO2-). The equilibrium between HNO2 and its ions can be represented as: HNO2(aq) ⇌ H+(aq) + NO2-(aq). It is a colorless and unstable compound.
Ka= [H+] [H2BO3-] / [h3BO3] (Apex)
ka=[H+][CN-]/[HCN]
6.6 x 10-9