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Chapter 16: Problem 18

Identify the Brønsted-Lowry acid and the BrønstedLowry base on the left side of each equation, and also identify the conjugate acid and conjugate base of each on the right side. $$ \begin{array}{l} \text { (a) } \mathrm{HBrO}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{BrO}^{-}(a q) \\\ \text { (b) } \mathrm{HSO}_{4}^{-}(a q)+\mathrm{HCO}_{3}^{-}(a q) \rightleftharpoons \mathrm{SO}_{4}^{2-}(a q)+\mathrm{H}_{2} \mathrm{CO}_{3}(a q) \\ \text { (c) } \mathrm{HSO}_{3}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{SO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \end{array} $$

Short Answer

Expert verified
(a) Brønsted-Lowry acid: \(HBrO\), base: \(H_2O\), conjugate acid: \(H_3O^{+}\), conjugate base: \(BrO^{-}\) (b) Brønsted-Lowry acid: \(HSO_{4}^{-}\), base: \(HCO_{3}^{-}\), conjugate acid: \(H_2CO_3\), conjugate base: \(SO_{4}^{2-}\) (c) Brønsted-Lowry acid: \(H_{3}O^{+}\), base: \(HSO_{3}^{-}\), conjugate acid: \(H_2SO_3\), conjugate base: \(H_2O\)

Step by step solution

01

Identify the Brønsted-Lowry acid and base

Compare the species on the left side. Look for species that are donating or accepting a proton. Here, \(HBrO\) donates a proton to \(H_2O\). So, \(HBrO\) is the acid and \(H_2O\) is the base.
02

Identify the conjugate acid and base

On the right side, after the reaction has taken place, the species formed after accepting the proton is the conjugate acid and the species formed after donating the proton is the conjugate base. In this case, \(H_3O^{+}\) is the conjugate acid and \(BrO^-\) is the conjugate base. (b) \(HSO_{4}^{-}(aq) + HCO_{3}^{-}(aq) \rightleftharpoons SO_{4}^{2-}(aq) + H_{2}CO_{3}(aq) \)
03

Identify the Brønsted-Lowry acid and base

Let's compare the species on the left side. Here, \(HSO_{4}^-\) donates a proton to \(HCO_3^-\). So, \(HSO_{4}^-\) is the acid and \(HCO_3^-\) is the base.
04

Identify the conjugate acid and base

On the right side, after the reaction, the species formed after accepting the proton is the conjugate acid and the species formed after donating the proton is the conjugate base. In this case, \(H_2CO_{3}\) is the conjugate acid and \(SO_{4}^{2-}\) is the conjugate base. (c) \(HSO_{3}^{-}(aq) + H_{3}O^{+}(aq) \rightleftharpoons H_{2}SO_{3}(aq) + H_{2}O(l) \)
05

Identify the Brønsted-Lowry acid and base

Lets compare the species on the left side. In this reaction, \(H_{3}O^{+}\) donates a proton to \(HSO_3^{-}\). So, \(H_{3}O^{+}\) is the acid and \(HSO_3^{-}\) is the base.
06

Identify the conjugate acid and base

On the right side, after the reaction, the species formed after accepting the proton is the conjugate acid and the species formed after donating the proton is the conjugate base. In this case, \(H_2SO_3\) is the conjugate acid and \(H_2O\) is the conjugate base.

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Most popular questions from this chapter

Predict the stronger acid in each pair: (a) \(\mathrm{HNO}_{3}\) or HNO \(_{2}\) (b) \(\mathrm{H}_{2} \mathrm{~S}\) or \(\mathrm{H}_{2} \mathrm{O} ;\) ; (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) or \(\mathrm{H}_{2} \mathrm{SeO}_{4}\) (d) \(\mathrm{CH}_{3} \mathrm{COOH}\) or \(\mathrm{CCl}_{3}\) ?OOH.

Is each of the following statements true or false? (a) All strong acids contain one or more H atoms. (b) A strong acid is a strong electrolyte. (c) A 1.0-M solution of a strong acid will have \(\mathrm{pH}=1.0\)

Which, if any, of the following statements are true? (a) The stronger the base, the smaller the \(\mathrm{p} K_{b}\). (b) The stronger the base, the larger the \(\mathrm{p} K_{b}\). (c) The stronger the base, the smaller the \(K_{b}\). (d) The stronger the base, the larger the \(K_{b}\). (e) The stronger the base, the smaller the \(\mathrm{p} K_{a}\) of its conjugate acid. (f) The stronger the base, the larger the \(\mathrm{p} K_{a}\) of its conjugate acid.

Benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right)\) and aniline \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\right)\) are both derivatives of benzene. Benzoic acid is an acid with $K_{a}=6.3 \times 10^{-5}\( and aniline is a base with \)K_{a}=4.3 \times 10^{-10}$ (a) What are the conjugate base of benzoic acid and the conjugate acid of aniline? (b) Anilinium chloride $\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3} \mathrm{Cl}\right)$ is a strong electrolyte that dissociates into anilinium ions \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}\right)\) and chloride ions. Which will be more acidic, a \(0.10 \mathrm{M}\) solution of benzoic acid or a 0.10 \(M\) solution of anilinium chloride? (c) What is the value of the equilibrium constant for the following equilibrium?

The active ingredient in aspirin is acetylsalicylic acid \(\left(\mathrm{HC}_{9} \mathrm{H}_{7} \mathrm{O}_{4}\right),\) a monoprotic acid with \(K_{a}=3.3 \times 10^{-4}\) at \(25^{\circ} \mathrm{C}\) What is the \(\mathrm{pH}\) of a solution obtained by dissolving one regular aspirin tablet, containing \(100 \mathrm{mg}\) of acetylsalicylic acid, in $200 \mathrm{~mL}$ of water?
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