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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. calculate the equivalence point ph. 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 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 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 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 place the following in order of increasing acid strength Hbro2 hbro3 hbro hb:o4 select one
Hbro2 < hbro4 < hbro < hbro3 o b Calculate the ph of a 0.200 kbro solution 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.
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? What is the initial ph of the solution Hbro + h₂o = bro + h30+ acid, hbro is titrated with 0.360…
