The hydroiodic acid solution has a molarity of 0.401.
Assume,
Mlb, base = 26.2 ml
Mb, a hydroiodic acid aqueous solution = 0.164
Ma, the hydroiodic acid solution's molarity = Ma
Mla, base required to neutralize = 10.7
Ma x Mla = Mb x Mlb
Ma = (Mb x Mlb) / ml
Ma = (0.164M) × (26.2ml) / 10.7ml
Ma = 0.401
When an aqueous solution of hydroiodic acid is standardized by titration with a 0.164 m sodium hydroxide solution, the molarity of the solution is 0.401.
Normalization is the process of finding the precise concentration (molarity) of a solution. Titration is a typical standardized analytical procedure. Titration is the process of interacting a known amount of one chemical with a known amount of another molecule.
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