Question

Consider the following reaction: HNO2 (aq) + HPO42-(aq) ⇌ NO2-(aq) + H2PO4-(aq)

a.)Identify the Brønsted-Lowry acids and bases in the forward reaction

b.)State the conjugate pairs for the above reaction. Be specific.

Identify the acids and bases in the following reactions and identify the conjugate pairs.

HF(aq) + H2O(l) ⇌ H3O+(aq) + F-(aq)

CH3NH2(aq) + H2O(l) ⇌ OH-(aq) + CH3NH3+(aq)

HCO3-(aq) + HSO4-(aq) ⇌ H2CO3(aq) + SO42-(aq)

Complete the following reactions:

____________(aq) + Br-(aq) ⇌ NH3(aq) + HBr(aq)

CH3COOH(aq) + CN-(aq) ⇌ __________(aq) + HCN(aq)

Of the following species, one is acidic, one is basic, and one is amphiprotic in their reactions with water: HCO3−, PO43−, and HNO2. Write the four equations needed to represent these facts.

Answer 1

a) Bronsted Lowry considers acid as any substance capable of releasing H⁺ and the acid is termed as Bronsted Lowry acid whereas the substance which accepts H⁺ are termed as Bronsted Lowry base.

Thus, in this reaction HNO_{​​​​2} gets converted to NO_{​​​​​2}^{​​​​-} thereby losing proton and hence Bronsted Lowry acid.

Also HPO_{​​​​4}^​​​2- gets converted into H_{​​​​​​​​​​​​2}​​​​​PO₄^- thus accepting proton and hence it's a Bronsted Lowry Base.

b) for HF + H_{​​​​​​2}O   H_{​​​​​​3}​​​​​O⁺ + F^{​​​​​​-}

Bronsted acid is HF as it donates H⁺

Bronsted base is H_{^{​​​​​​}​​​​​​2}​​​​O as it accepts proton

Conjugate acid is H_{​​​​​​3}​​​​​O⁺ and conjugate base is F^{​​​​​​-}.

Hope this helps you.