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If my understanding is correct, bromous acid ($\ce {hbro2}$) is a stronger acid than hypobromous acid ($\ce {hbro}$) because the additional electronegative oxygen atom draws the electron away from the hydrogen atom, making dissociation for $\ce {h+}$ easier. Hbro (aq) + h₂o (1) br (s) +… What is the initial ph of the solution

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Hbro + h₂o = bro + h30+ acid, hbro is titrated with 0.360… Be sure to include the proper phases for all species within the reaction Solution for write the acidic equilibrium equation for hbro

Be sure to include the proper phases for all species within the reaction.

Consider a ph titration curve at 298 k for 50 ml of 0.10 m hypobromous acid, hbro (ka = 2.8 x 10−9), titrated with 0.10 m koh solution  calculate the equivalence point ph. Essential conditions for an oxoacid are Presence of any one element other than oxygen sulphuric acid, nitric acid, perchloric acid, perchlorous acid are examples of oxo acids.

**calculate the ph of a mixture of koh and hbro** **problem statement:** determine the ph when 50.0 ml of 0.150 m koh is mixed with 20.0 ml of 0.300 m hbro The acid dissociation constant (ka) for hbro is 2.5 × 10⁻⁹ Calculate the equilibrium concentrations of all substances if the initial concentration is 0.050 m for hbro. Hbro (aq) + h20 (1) h30* (ag) + bro (aq) a) hypobromous acid dissociates in water according to the above process

In a 0.50 m hbro (aq) solution [bro] was found to be 3.5 x 10³ m at 25°c.

Note that ph is close to pka of both nh4+ and hbro, solution near equivalence is the ph buffer and the titration detection would be very inaccurate.