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3 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. What is the value of ka for hbro? 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 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 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 place the following in order of increasing acid strength
Hbro2 hbro3 hbro hb:o4 select one Hbro2 < hbro4 < hbro < hbro3 o b 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.
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. Express the ph numerically using one decimal place Calculate the ph of a 4.0 m solution of hypobromous acid Round your answer to 1 decimal place
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