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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. Hbro + h₂o = bro + h30+ acid, hbro is titrated with 0.360… 25.0 ml of 0.600 m hypobromous acid, hbro, is titrated with 0.400 m sodium hydroxide, naoh
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Calculate the ph of the solution after the addition of 20.0 ml of naoh solution. What is the initial ph of the 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?
Transcribed image text: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. 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.
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 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
 what volume of koh is needed to.
