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Chapter 16: Problem 18

Identify the Bronsted-Lowry acid and the Bronsted-Lowry base on the left side of each equation, and also identify 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) \(\mathrm{HSO}_{4}^{-}(a q)+\mathrm{HCO}_{3}^{-}(a q) \rightleftharpoons\) \(\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\mathrm{SO}_{4}^{2-}(a q)+\mathrm{H}_{2} \mathrm{CO}_{3}(a q)\) (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 Acid and Base

On the left side, \(\mathrm{HBrO}\) donates \(\mathrm{H}^{+}\), so it is a Bronsted-Lowry acid, and \(\mathrm{H}_{2} \mathrm{O}\) accepts \(\mathrm{H}^{+}\), so it is a Bronsted-Lowry base.
02

Identify Conjugate Acid and Conjugate Base

On the right side, \(\mathrm{H}_{3} \mathrm{O}^{+}\) is the conjugate acid formed by the acceptance of \(\mathrm{H}^{+}\) by \(\mathrm{H}_{2} \mathrm{O}\), and \(\mathrm{BrO}^{-}\) is the conjugate base formed by donating \(\mathrm{H}^{+}\) from \(\mathrm{HBrO}\). (b) \(\mathrm{HSO}_{4}^{-}(a q)+\mathrm{HCO}_{3}^{-}(a q) \rightleftharpoons \mathrm{SO}_{4}^{2-}(a q)+\mathrm{H}_{2} \mathrm{CO}_{3}(a q)\)
03

Identify Acid and Base

On the left side, \(\mathrm{HSO}_{4}^{-}\) donates \(\mathrm{H}^{+}\), so it is a Bronsted-Lowry acid, and \(\mathrm{HCO}_{3}^{-}\) accepts \(\mathrm{H}^{+}\), so it is a Bronsted-Lowry base.
04

Identify Conjugate Acid and Conjugate Base

On the right side, \(\mathrm{H}_{2} \mathrm{CO}_{3}\) is the conjugate acid formed by the acceptance of \(\mathrm{H}^{+}\) by \(\mathrm{HCO}_{3}^{-}\), and \(\mathrm{SO}_{4}^{2-}\) is the conjugate base formed by donating \(\mathrm{H}^{+}\) from \(\mathrm{HSO}_{4}^{-}\). (c) \(\mathrm{HSO}_{3}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{SO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\)
05

Identify Acid and Base

On the left side, \(\mathrm{HSO}_{3}^{-}\) accepts \(\mathrm{H}^{+}\), so it is a Bronsted-Lowry base, and \(\mathrm{H}_{3} \mathrm{O}^{+}\) donates \(\mathrm{H}^{+}\), so it is a Bronsted-Lowry acid.
06

Identify Conjugate Acid and Conjugate Base

On the right side, \(\mathrm{H}_{2} \mathrm{SO}_{3}\) is the conjugate acid formed by the acceptance of \(\mathrm{H}^{+}\) by \(\mathrm{HSO}_{3}^{-}\), and \(\mathrm{H}_{2} \mathrm{O}\) is the conjugate base formed by donating \(\mathrm{H}^{+}\) from \(\mathrm{H}_{3} \mathrm{O}^{+}\).

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Most popular questions from this chapter

Calculate \(\left[\mathrm{OH}^{-}\right]\) for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: \((\mathbf{a})\left[\mathrm{H}^{+}\right]=0.0505 M (\mathbf{b})\left[\mathrm{H}^{+}\right]=2.5 \times 10^{-10} M ;(\mathbf{c})\) a solution in which \(\left[\mathrm{H}^{+}\right]\) is 1000 times greater than \(\left[\mathrm{OH}^{-}\right] .\)

codeine \(\left(\mathrm{C}_{18} \mathrm{H}_{21} \mathrm{NO}_{3}\right)\) is a weak organic base. \(\mathrm{A} 5.0 \times 10^{-3} \mathrm{M}\) solution of codeine has a pH of \(9.95 .\) Calculate the value of \(K_{b}\) for this substance. What is the \(\mathrm{pK}_{b}\) for this base?

Lactic acid \(\left(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{COOH}\right)\) has one acidic hydrogen. A 0.10 \(\mathrm{M}\) solution of lactic acid has a pH of \(2.44 .\) Calculate \(K_{a} .\)

Which of the following statements is false? (a) An Arrhenius base increases the concentration of OH \(^{-}\) in water. (b) A Bronsted-Lowry base is a proton acceptor. (c) Water can act as a Bronsted-Lowry acid. (d) Water can act as a Bronsted-Lowry base. (e) Any compound that contains an \(-\)OH group acts as a Bronsted-Lowry base.

The volume of an adult's stomach ranges from about 50 mL when empty to 1 when full. If the stomach volume is 400 mL and its contents have a pH of \(2,\) how many moles of \(\mathrm{H}^{+}\) does the stomach contain? Assuming that all the \(\mathrm{H}^{+}\) comes from \(\mathrm{HCl}\) , how many grams of sodium hydrogen carbonate will totally neutralize the stomach acid?
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