The behaviour of HC1O4 in H2SO4 and SbF5 inHF are respectively.a)Strong acid and weak acidb)Weak acid and strong acidc)Strong base and strong acidd)Weak base and weak acidCorrect answer is option 'B'. Can you explain this answer?

Question

Answer

The behavior of HClO4 in H2SO4 and SbF5 in HF can be explained as follows:

1. HClO4 in H2SO4:
- HClO4 is a strong acid, meaning it ionizes completely in water to produce H+ ions.
- When HClO4 is dissolved in H2SO4, the H2SO4 acts as a solvent and does not affect the behavior of HClO4.
- Therefore, HClO4 still behaves as a strong acid in H2SO4, producing H+ ions.

2. SbF5 in HF:
- SbF5 is a weak acid, meaning it ionizes only partially in water to produce H+ ions.
- When SbF5 is dissolved in HF, the HF acts as a solvent and affects the behavior of SbF5.
- HF is a strong acid and readily donates H+ ions to the solution.
- In the presence of excess HF, SbF5 reacts with HF to form SbF6- ions, which are stable.
- This reaction consumes the H+ ions produced by SbF5, resulting in a decrease in the concentration of H+ ions in the solution.
- Therefore, SbF5 behaves as a weak acid in HF, producing fewer H+ ions compared to its behavior in water.

Summary:
- HClO4 behaves as a strong acid in H2SO4 because H2SO4 does not affect its behavior.
- SbF5 behaves as a weak acid in HF because HF reacts with SbF5 to form stable SbF6- ions, leading to a decrease in H+ ion concentration in the solution.

Answer

HClO4 dissociate as H+ and ClO4-. H2SO4 dissociate as 2H+ and SO42-. As Sulfuric acid can give more hydrogen ion so, HClO4 acts as a weaker acid in comparison to sulfuric acid.

HF can be dissociate as H+ and F-. SbF5 can accept F- and form stable SbF6-. As it accepts anion so, acts as a strong acid.

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