Respuesta :
Answer:
The concentration of the pyridinium cation at equilibrium is 1.00×10⁻³ M
Explanation:
In water we have
C₅H₅NHBr + H₂O ⇒ C₅H₅NH+ + Br−
Pyridinium Bromide (C₅H₅NHBr) Dissociates Completely Into C₅H₅NH+ And Br− as such it is a strong Electrolyte.
Therefore the number of moles of positive ion produced per mole of C₅H₅NHBr is one
pH = - log [H₃O⁺] Therefore 10^-pH = [H₃O⁺] = concentration of C₅H₅NHBr
= 10⁻³ = 0.001M = concentration of C₅H₅NHBr
The concentration of C₅H₅NHBr is = 1.00×10⁻³ M to two places of decimal
1.00×10⁻³ M is the concentration of the pyridinium cation at equilibrium, in units of molarity to two decimal places.
What is pH?
pH defines the acidity and basicity of any solution and it is calculated as:
pH = -log[H⁺], where
[H⁺] = concentration of H⁺ ions.
pH of pyridinium bromide solution = 3 (given)
At equilibrium chemical reaction in water is shown as:
C₅H₅NHBr + H₂O → C₅H₅NH⁺ + Br⁻
Pyridinium bromide is a strong electrolyte that's why it shows complete dissociation in water and produces equal no. of cations and anions. So, 1 mole of pyridinium bromide produces 1 mole of C₅H₅NH⁺ cation and its concentration is calculated as:
pH = -log[C₅H₅NH⁺]
or [tex]${\rm{1}}{{\rm{0}}^{{\rm{ - pH}}}}$[/tex] = [C₅H₅NH⁺]
On putting values in this equation, we get
[C₅H₅NH⁺] = 10⁻³ = 0.001 M = concentration of C₅H₅NHBr
Hence, the concentration of pyridinium cation is 1.00×10⁻³ M.
To learn more about pH, visit below link:
https://brainly.com/question/172153
