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.
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 HNO2 gets converted to NO2- thereby losing proton and hence Bronsted Lowry acid.
Also HPO42- gets converted into H2PO4- thus accepting proton and hence it's a Bronsted Lowry Base.
b) for HF + H2O H3O+ + F-
Bronsted acid is HF as it donates H+
Bronsted base is H2O as it accepts proton
Conjugate acid is H3O+ and conjugate base is F-.
Hope this helps you.
Consider the following reaction: HNO2 (aq) + HPO42-(aq) ⇌ NO2-(aq) + H2PO4-(aq) a.)Identify the Brønsted-Lowry acids...
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In the following equation, label the Bronsted-Lowry acid, base and conjugate pairs. CH3NH2 (aq) + H2PO4- (aq) ↔ CH3NH3+ (aq) + HPO42- (aq)
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