(a) Which of the following is the stronger Brønsted-Lowry acid, \(\mathrm{HClO}_{3}\) or \(\mathrm{HClO}_{2} ?\) (b) Which is the stronger Brønsted-

To determine the strength of the given Brønsted-Lowry acids and bases, first, we need to identify their conjugate acids or bases. When an acid donates a proton, it forms its conjugate base, and when a base accepts a proton, it forms its conjugate acid. (a) For the acids \(\mathrm{HClO}_{3}\) and \(\mathrm{HClO}_{2}\): - \(\mathrm{HClO}_{3}\) donates a proton to form its conjugate base: \(\mathrm{ClO}_{3}^-\) - \(\mathrm{HClO}_{2}\) donates a proton to form its conjugate base: \(\mathrm{ClO}_{2}^-\) (b) For the bases \(\mathrm{ClO}^{-}_{3}\) and \(\mathrm{ClO}^{-}_{2}\): - \(\mathrm{ClO}^{-}_{3}\) accepts a proton to form its conjugate acid: \(\mathrm{HClO}_{3}\) - \(\mathrm{ClO}^{-}_{2}\) accepts a proton to form its conjugate acid: \(\mathrm{HClO}_{2}\)

The strength of a Brønsted-Lowry acid depends on the stability of its conjugate base. The more stable the conjugate base, the stronger the acid will be. Comparing the conjugate bases of the given acids in part (a): - \(\mathrm{ClO}_{3}^-\) has three oxygen atoms with -1 formal charge each, whereas \(\mathrm{ClO}_{2}^-\) has two oxygen atoms with -1 formal charge each. - The extra oxygen in \(\mathrm{ClO}_{3}^-\) helps to spread the negative charge over more atoms, which increases the stability by reducing its electron density.

As the conjugate base, \(\mathrm{ClO}_{3}^-\), is more stable than \(\mathrm{ClO}_{2}^-\), the corresponding acid, \(\mathrm{HClO}_{3}\), is the stronger Brønsted-Lowry acid compared to \(\mathrm{HClO}_{2}\). Answer for part (a): \(\mathrm{HClO}_{3}\) is the stronger Brønsted-Lowry acid.

To determine the strength of the given Brønsted-Lowry bases, we should look at the stability of their conjugate acids. The more stable the conjugate acid, the stronger the original base will be. Comparing the conjugate acids of the given bases in part (b): - The conjugate acid of \(\mathrm{ClO}^{-}_{3}\) is \(\mathrm{HClO}_{3}\) - The conjugate acid of \(\mathrm{ClO}^{-}_{2}\) is \(\mathrm{HClO}_{2}\) From part (a), we already know that \(\mathrm{HClO}_{3}\) is stronger than \(\mathrm{HClO}_{2}\).

Since \(\mathrm{HClO}_{3}\) is a stronger acid than \(\mathrm{HClO}_{2}\), its conjugate base, \(\mathrm{ClO}^{-}_{3}\), is weaker than the conjugate base of \(\mathrm{HClO}_{2}\), which is \(\mathrm{ClO}^{-}_{2}\). So, the stronger Brønsted-Lowry base is \(\mathrm{ClO}^{-}_{2}\). Answer for part (b): \(\mathrm{ClO}^{-}_{2}\) is the stronger Brønsted-Lowry base.