Chemistry MCQs for NEET — Practice Questions with Answers

According to the Lowry-Bronsted concept, an acid is a substance that can donate a proton (H⁺ ion). The $H_3O^+$ ion, also known as the hydronium ion, can donate a proton, hence it is considered an acid.

The conjugate acid of a base is formed when the base accepts a proton (H⁺ ion). For the base $NH_2^-$ (amide ion), accepting a proton forms $NH_3$ (ammonia), which is the conjugate acid of $NH_2^-$. Therefore, the conjugate acid of $NH_2^-$ is $NH_3$.

$ N_3 H \rightleftharpoons N_3 ^ - + H^ + Hydrazoic acid N_3 H $

In the reaction $NH_3 + Na ightarrow NaNH_2 + rac{1}{2} H_2$, ammonia ($NH_3$) donates a proton (H⁺) to form sodium amide ($NaNH_2$), acting as an acid according to the Lowry-Bronsted definition.

$ H_2S $ can donate proton but can't accept proton.

In the given reaction, $H_2SO_4$ donates a proton to $H_2O$, forming $HSO_4^-$ and $H_3O^+$. Therefore, $HSO_4^-$ is the conjugate base of $H_2SO_4$ and $H_2O$ is the conjugate base of $H_3O^+$.

With increase in temperature, ionic product increases. because self ionisation of is endothermic process

EDTA is Arrhenius acid as it can give $ H ^ + $ ions in aqueous solution, bronsted base. as it can accept protons and lewis base because N and O in it can donate lone paris of electrons.

$ K_w = [ H^+ ] [ OH^ - ] $ $ = mol L ^ {-1} \times mol L ^ {-1} = mol ^ 2 L ^ { -2 } $