MHTCET 14 May 2023 Shift 2 Solved Paper

The Bronsted-Lowry theory defines an acid as a substance that can donate a proton ( $\mathrm{H}^{+}$ion), and a base as a substance that can accept a proton. For the given chemical reaction:$\mathrm{HCl}_{\mathrm{(aq)}} + \mathrm{H}_2\mathrm{O}_{\mathrm{(l)}} \rightleftharpoons \mathrm{H}_3\mathrm{O}_{\mathrm{(aq)}}^{+} + \mathrm{Cl}_{\mathrm{(aq)}}^{-}$In this reaction, hydrochloric acid $(\mathrm{HCl})$ donates a proton to water $(\mathrm{H}_2\mathrm{O})$, which acts as a base and accepts the proton, forming hydronium ion $(\mathrm{H}_3\mathrm{O}^{+})$and chloride ion $(\mathrm{Cl}^{-})$. Here is the role of each species according to the Bronsted-Lowry theory:$\mathrm{HCl}$ is a Bronsted-Lowry acid because it donates a proton to water. $\mathrm{H}_2\mathrm{O}$ is a Bronsted-Lowry base because it accepts a proton from $\mathrm{HCl}$. $\mathrm{H}_3\mathrm{O}^{+}$is the conjugate acid formed after $\mathrm{H}_2\mathrm{O}$ accepts the proton. $\mathrm{Cl}^{-}$is the conjugate base formed after $\mathrm{HCl}$ donates the proton.According to these roles, the correct option identifying the base that accepts a proton in this reaction is: Option B: $\mathrm{H}_2\mathrm{O}_{\mathrm{(l)}}$