HBrO2(aq) + BrO3-(aq) ↔ BrO2-(aq) + HBrO3(aq) Would you expect the equilibrium to lie to the right or the left? Why? 2. HSO4-(aq) + H2PO4-(aq) ↔ SO4-2(aq) + H3PO4(aq) a) What is the acid in this reaction (from a Brønsted-Lowry point of view)? b) If the equilibrium lies to the right, what does this mean concerning acid and base strengths?
The Correct Answer and Explanation is:
. HBrO2(aq) + BrO3-(aq) ⇌ BrO2-(aq) + HBrO3(aq)
- Equilibrium Position:
The equilibrium in this reaction is likely to lie to the left, as HBrO2 is a stronger acid compared to HBrO3, and BrO3- is a stronger base compared to BrO2-.- HBrO2 can donate a proton to form BrO2-, while HBrO3 is more likely to accept a proton to form HBrO2.
- Therefore, the system will favor the side with the stronger acid and weaker base. In this case, HBrO2 is the stronger acid, and BrO3- is the stronger base, so the equilibrium tends to shift to the left, favoring the reactants.
2. HSO4-(aq) + H2PO4-(aq) ⇌ SO4²⁻(aq) + H3PO4(aq)
- (a) Acid (from a Brønsted-Lowry Point of View):
- HSO4- is the acid in this reaction.
- According to the Brønsted-Lowry theory, acids are proton donors. In this reaction, HSO4- donates a proton to form SO4²⁻, while H2PO4- (hydrogen phosphate) acts as the base by accepting the proton to form H3PO4 (phosphoric acid).
- (b) Meaning if Equilibrium Lies to the Right:
- If the equilibrium lies to the right, this indicates that SO4²- and H3PO4 are favored products. This means that HSO4- (bisulfate) is a stronger acid than H2PO4- (dihydrogen phosphate), and H3PO4 is a weaker acid than H2PO4-.
- The proton transfer happens in such a way that the stronger acid (HSO4-) donates a proton to the weaker acid (H2PO4-), shifting the equilibrium toward the formation of SO4²- and H3PO4.
In summary, the equilibrium for both reactions is influenced by the relative strengths of the acids and bases involved. Stronger acids favor the dissociation, and weaker bases tend to accept protons, leading to a shift toward the products.
