Read the Assertion and Reason below and choose the correct option. — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

$10^{-4}\text{ M HCl}$ has $[\text{H}^+] = 10^{-4}\text{ M}$. $1\text{ M HCOOH}$ has $[\text{H}^+] \approx \sqrt{K_a C} = \sqrt{10^{-3} \times 1} \approx 3.16 \times 10^{-2}\text{ M}$. Since $3.16 \times 10^{-2}\text{ M} > 10^{-4}\text{ M}$, the HCOOH solution has a higher $\text{H}^+$ concentration and is more acidic, making Statement I false. Statement II is true as HCl is indeed a strong acid while HCOOH is weak.