In dilute aqueous solution HF is a weaker acid than HI because

Question

In dilute aqueous solution HF is a weaker acid than HI because (A) H-F bond energy is greater than HI bond energy (B) The hydration energy of F is higher than that of I- (C) Of the presence of hydrogen bonds in HF (D) Fluorine is a stronger base as compared to iodine

Tardigrade Admin · Accepted Answer

HI is strongest acid because due to largest size of I, the H-I bond is weakest and its bond dissociation energy is least so it breaks most readily and hence HI is the strongest acid. The order of acidic strength is
HI > HBr > HCl > HF

Q. In dilute aqueous solution HF is a weaker acid than HI because

H-F bond energy is greater than HI bond energy

The hydration energy of F is higher than that of $I^{-}$

Of the presence of hydrogen bonds in HF

Fluorine is a stronger base as compared to iodine

HI is strongest acid because due to largest size of I, the H-I bond is weakest and its bond dissociation energy is least so it breaks most readily and hence HI is the strongest acid. The order of acidic strength is
HI > HBr > HCl > HF

Q. In dilute aqueous solution HF is a weaker acid than HI because

H-F bond energy is greater than HI bond energy

The hydration energy of F is higher than that of I−

Of the presence of hydrogen bonds in HF

Fluorine is a stronger base as compared to iodine

HI is strongest acid because due to largest size of I, the H-I bond is weakest and its bond dissociation energy is least so it breaks most readily and hence HI is the strongest acid. The order of acidic strength is HI > HBr > HCl > HF

The hydration energy of F is higher than that of $I^{-}$

HI is strongest acid because due to largest size of I, the H-I bond is weakest and its bond dissociation energy is least so it breaks most readily and hence HI is the strongest acid. The order of acidic strength is
HI > HBr > HCl > HF