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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. Hbro2 < hbro4 < hbro < hbro3 o b So i was looking at factors that control the relative strengths of acids and bases
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 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?
Which is the weakest acid 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
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. What is the initial ph of the solution Hbro + h₂o = bro + h30+ acid, hbro is titrated with 0.360…
Solution for the ph of a 0.55 m aqueous solution of hypobromous acid, hbro, at 25oc is 4.48
What is the value of ka for hbro? Solution for place the following in order of increasing acid strength
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