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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 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. Solution for the ph of a 0.55 m aqueous solution of hypobromous acid, hbro, at 25.0 °c is 4.48 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
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? Calculate the ph of a 0.200 kbro solution You should not use the quadratic formula for this problem.
Calculate the ph of a 1.60 m kbro solution By signing up, you'll get thousands of. 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
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.
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