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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.

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? You should not use the quadratic formula for this problem. 25.0 ml of 0.600 m hypobromous acid, hbro, is titrated with 0.400 m sodium hydroxide, naoh Calculate the ph of the solution after the addition of 20.0 ml of naoh solution. Calculate the ph of a 0.200 kbro solution

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 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 which one of the following correctly shows the weak acid equilibrium for hypobromous acid, hbro A) hbro (aq) + h₂o (1) bro (aq) + h³o+ (aq) b)…

What is the initial ph of the solution

Hbro + h₂o = bro + h30+ acid, hbro is titrated with 0.360… Solution for choose the strongest acid from each group (a) hclo, hbro, hio (b) hio, hio3, hio4 (c) hio, hbro2, hbro4