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3 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. Hbro2 < hbro4 < hbro < hbro3 o b So i was looking at factors that control the relative strengths of acids and bases

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We know that $\\ce{hi}$ is a stronger acid that $\\ce{hbr}$ because $\\ce{i}$ is a much larger atom Hbro2 hbro3 hbro hb:o4 select one 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.

What is the initial ph of the solution Hbro + h₂o = bro + h30+ acid, hbro is titrated with 0.360… Calculate the ph of a 0.200 kbro solution Solution for the ph of a 0.55 m aqueous solution of hypobromous acid, hbro, at 25.0 °c is 4.48

What is the value of ka for hbro The ph of a 0.55 m aqueous solution of hypobromous acid, h b r o, at 25 ∘ c is 4.48 What is the value of k a for h b r o? Solution for write the acidic equilibrium equation for hbro

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

Solution for place the following in order of increasing acid strength