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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 Calculate the ph of a 0.200 kbro solution

What is the initial ph of the solution

Hbro + h₂o = bro + h30+ acid, hbro is titrated with 0.360… 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. 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 Solution for write the acidic equilibrium equation for hbro Be sure to include the proper phases for all species within the reaction. 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 place the following in order of increasing acid strength