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Chapter 16: Problem 18

Designate the Bronsted-Lowry acid and the Bronsted-Lowry base on the left side of each equation, and also designate the conjugate acid and conjugate base of each on the right side. (a) \(\mathrm{HBrO}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{BrO}^{-}(a q)\) (b) \(\mathrm{HSO}_{4}^{-}(a q)+\mathrm{HCO}_{3}^{-}(a q) \rightleftharpoons \mathrm{SO}_{4}^{2-}(a q)+\mathrm{H}_{2} \mathrm{CO}_{3}(a q)\) (c) \(\mathrm{HSO}_{3}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{SO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\)

Short Answer

Expert verified
(a) Acid: \(\mathrm{HBrO}\), Base: \(\mathrm{H}_{2}\mathrm{O}\), Conjugate acid: \(\mathrm{H}_{3}\mathrm{O}^{+}\), Conjugate base: \(\mathrm{BrO}^{-}\) (b) Acid: \(\mathrm{HSO}_{4}^{-}\), Base: \(\mathrm{HCO}_{3}^{-}\), Conjugate acid: \(\mathrm{H}_{2}\mathrm{CO}_{3}\), Conjugate base: \(\mathrm{SO}_{4}^{2-}\) (c) Acid: \(\mathrm{H}_{3}\mathrm{O}^{+}\), Base: \(\mathrm{HSO}_{3}^{-}\), Conjugate acid: \(\mathrm{H}_{2}\mathrm{SO}_{3}\), Conjugate base: \(\mathrm{H}_{2}\mathrm{O}\)

Step by step solution

01

Identify the acid and base in the reactants

First, we're looking for the species that donates a proton and the species that accepts a proton. In this case, \(\mathrm{HBrO}\) will donate a proton to \(\mathrm{H}_{2}\mathrm{O}\), which will accept it.
02

Identify the conjugate acid and conjugate base in the products

After donating a proton, \(\mathrm{HBrO}\) will become \(\mathrm{BrO}^{-}\), which is the conjugate base. On the other hand, after accepting a proton, \(\mathrm{H}_{2}\mathrm{O}\) will become \(\mathrm{H}_{3}\mathrm{O}^{+}\), which is the conjugate acid. (b) \(\mathrm{HSO}_{4}^{-}(aq) + \mathrm{HCO}_{3}^{-}(aq) \rightleftharpoons \mathrm{SO}_{4}^{2-}(aq) + \mathrm{H}_{2}\mathrm{CO}_{3}(aq)\)
03

Identify the acid and base in the reactants

In this reaction, we can see that \(\mathrm{HSO}_{4}^{-}\) will donate a proton to \(\mathrm{HCO}_{3}^{-}\), which will accept it.
04

Identify the conjugate acid and conjugate base in the products

After donating a proton, \(\mathrm{HSO}_{4}^{-}\) will become \(\mathrm{SO}_{4}^{2-}\), which is the conjugate base. After accepting a proton, \(\mathrm{HCO}_{3}^{-}\) will become \(\mathrm{H}_{2}\mathrm{CO}_{3}\), which is the conjugate acid. (c) \(\mathrm{HSO}_{3}^{-}(aq) + \mathrm{H}_{3}\mathrm{O}^{+}(aq) \rightleftharpoons \mathrm{H}_{2}\mathrm{SO}_{3}(aq) + \mathrm{H}_{2}\mathrm{O}(l)\)
05

Identify the acid and base in the reactants

Here, we can readily see that \(\mathrm{HSO}_{3}^{-}\) will accept a proton from \(\mathrm{H}_{3}\mathrm{O}^{+}\), which will donate it.
06

Identify the conjugate acid and conjugate base in the products

After accepting a proton, \(\mathrm{HSO}_{3}^{-}\) will become \(\mathrm{H}_{2}\mathrm{SO}_{3}\), which is the conjugate acid. Conversely, after donating a proton, \(\mathrm{H}_{3}\mathrm{O}^{+}\) will become \(\mathrm{H}_{2}\mathrm{O}\), which is the conjugate base.

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Most popular questions from this chapter

Calculate \(\left[\mathrm{OH}^{-}\right]\) and \(\mathrm{pH}\) for (a) \(1.5 \times 10^{-3} \mathrm{M} \mathrm{Sr}\left(\mathrm{OH}_{2}\right),\) (b) \(2.250 \mathrm{~g}\) of \(\mathrm{LiOH}\) in \(250.0 \mathrm{~mL}\) of solution, (c) \(1.00 \mathrm{~mL}\) of \(0.175 \mathrm{M} \mathrm{NaOH}\) diluted to \(2.00 \mathrm{~L},\) (d) a solution formed by adding \(5.00 \mathrm{~mL}\) of \(0.105 \quad M \mathrm{KOH}\) to \(15.0 \mathrm{~mL}\) of \(9.5 \times 10^{-2} \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}\)

Although pure \(\mathrm{NaOH}\) and \(\mathrm{NH}_{3}\) have very different properties, their aqueous solutions possess many common properties. List some general properties of these solutions, and explain their common behavior in terms of the species present.

Calculate the molar concentration of \(\mathrm{OH}^{-}\) ions in a \(0.724 \mathrm{M}\) solution of hypobromite ion \(\left(\mathrm{BrO}^{-} ; K_{b}=4.0 \times 10^{-6}\right) .\) What is the \(\mathrm{pH}\) of this solution?

The hypochlorite ion, \(\mathrm{ClO}^{-},\) acts as a weak base. (a) Is \(\mathrm{ClO}^{-}\) a stronger or weaker base than hydroxylamine? (b) When ClO \(^{-}\) acts as a base, which atom, Cl or \(\mathrm{O}\), acts as the proton acceptor? (c) Can you use formal charges to rationalize your answer to part (b)?

Calculate the concentration of an aqueous solution of \(\mathrm{Ca}(\mathrm{OH})_{2}\) that has a \(\mathrm{pH}\) of \(10.05 .\)
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