Question

A. Which of the following can behave as Bronsted-Lowry bases in aqueous solution?

NO₃^-

H₃PO₄

NH₄⁺

HClO

None of the Above

B. Which of the following can behave as Bronsted-Lowry bases in aqueous solution?

NH₄⁺

NH₃

Ca(OH)₂

Br^-

None of the Above

C. Which of the following can behave as Bronsted-Lowry bases in aqueous solution?

HCO₃^-

NaOH

KOH

HF

None of the Above

* please help me I am really struggling with this concept. I fully cannot seem to grasp it and really need to understand it*

Answer 1

A Bronsted-Lowry base is the one which can accept a proton(H+)

A. When NO3- accept a proton forms HNO3 so it acts a Bronsted-Lowry base

H3PO4 cannot accept a proton so it cannot acts as Bronsted-Lowry base.

NH4+ cannot accept a proton so it cannot acts as Bronsted-Lowry base.

HClO cannot accept a proton so it cannot acts as Bronsted-Lowry base.

B. NH4+ cannot accept a proton so it cannot acts as Bronsted-Lowry base.

When NH3 accept a proton forms NH4+ so it acts a Bronsted-Lowry base

Ca(OH)2 cannot accept a proton so it cannot acts as Bronsted-Lowry base.

When Br- accept a proton forms HBr so it acts a Bronsted-Lowry base

C. When HCO3- accept a proton forms H2CO3 so it acts a Bronsted-Lowry base

NaOH cannot accept a proton so it cannot acts as Bronsted-Lowry base.

KOH cannot accept a proton so it cannot acts as Bronsted-Lowry base.

HF cannot accept a proton so it cannot acts as Bronsted-Lowry base.