Question

acid strength is compared for each set of compounds. given the main reason that would explain the trend:

NH₃<H_​2O<HF    why?

HF<HCl<HBr<HI why?

H₃PO₄​<H₂SO₄<HClO₄   why?

HClO<HClO₂<HClO₃​<HClO₄    why?

CH₃CO₂H<CH₂ClCO₂H<CHCl₂CO₂H<CCl₃CO₂H    why?

Answer 1

1) NH₃<H_​2O<HF    why?

reason :

F is the most electronegative atom than O and N so H-F bond is very weak and readily loose H+ ion from HF so HF is strong acid

2) HF<HCl<HBr<HI why?

reason :

the bond length between H and I is very high so the bond disscoation enrgy for H-I bond is very low compared reamining so HI is strong acid

3) H₃PO₄​<H₂SO₄<HClO₄   why?

reason :

central atom electronegativity increases acidity also increases in case of oxoacids.

electronegativity order P < S < Cl

4) HClO<HClO₂<HClO₃​<HClO₄    why?

reason :

oxidation state of central atom increases acidity also increases

oxidation state of central atoms in the compounds in HClO4 , Cl oxidation state is + 7 so highest acidic nature

5) CH₃CO₂H<CH₂ClCO₂H<CHCl₂CO₂H<CCl₃CO₂H    why?

reason :

number -I groups increases at alpha position of carboxylic acids the acidity also increases