Question

Write the formula of the conjugate base of each acid: HBr, HCO3−, and CH3CH2CH2OH. Be sure to answer all parts. (Note: If a number has been placed as a subscript, the cursor needs to be returned to the main writing line before selecting the superscript.)

Answer 1

Explanation:

According to the Bronsted-Lowry conjugate acid-base theory:

• An acid is defined as a substance which looses donates protons and thus forming conjugate base.
• A base is defined as a substance which accepts protons and thus forming conjugate acid.

1) The conjugate base of acid : HBr

$HBr\rightarrow H^++Br^-$

$Br^-$ is the conjugate base of HBr.

2) The conjugate base of acid : $HCO_3^{-}$

$HCO_3^{-}\rightarrow H^++CO_3^{2-}$

$CO_3^{2-}$ is the conjugate base of $HCO_3^{-}$

3) The conjugate base of acid : $CH_3CH_2CH_2OH$

$CH_3CH_2CH_2OH\rightarrow H^++CH_3CH_2CH_2O^-$

$CH_3CH_2CH_2O^-$ is the conjugate base of $CH_3CH_2CH_2OH$