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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
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?
What is the initial ph of the solution Hbro + h₂o = bro + h30+ acid, hbro is titrated with 0.360… Calculate the ph of a 0.200 kbro solution Which is the weakest acid
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 The acid dissociation constant ka of hypobromous acid (hbro) is 2.3*10 9 calculate the ph of a 4.0 m solution of hypobromous acid Round your answer to 1 decimal place.
Solution for place the following in order of increasing acid strength
Hbro2 hbro3 hbro hb:o4 select one Hbro2 < hbro4 < hbro < hbro3 o b
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