Bronsted-Lowry Theory and Reactions

The video tutorial explains how to find the conjugate acid of the bisulfate ion (HS-) using the Bronsted-Lowry theory. It describes how bases accept hydrogen ions (H+), and demonstrates the process of adding an H+ to the bisulfate ion, resulting in a neutral compound, H2S. The video concludes with the identification of H2S as the conjugate acid of HS-.

What is the role of a base according to the Bronsted-Lowry theory?

• To donate an electron

• To donate a proton

• To accept a proton

• To accept an electron

What happens when a hydrogen ion (H+) is added to the bisulfate ion (HS-)?

• It forms a neutral compound

• It forms a negatively charged ion

• It forms a compound with a net positive charge

• It forms a positively charged ion

What is the net charge of the compound formed after adding H+ to HS-?

• Positive

• Undefined

• Negative

• Zero

What is the conjugate acid of the bisulfate ion (HS-)?

• HSO4

• SO4

• H2S

• H2O

Why is the compound no longer considered a base after adding H+?

• Because it loses a proton

• Because it gains an electron

• Because it becomes a neutral compound

• Because it becomes positively charged