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Chapter 16: Problem 20

(a) Write an equation for the react ion in which \(\mathrm{HSO}_{4}^{-}(a q)\) acts as a base in \(\mathrm{H}_{2} \mathrm{O}(l) .(\mathbf{b})\) Write an equation for the reaction in which \(\mathrm{HSO}_{4}^{-}(a q)\) acts as an acid in \(\mathrm{H}_{2} \mathrm{O}(I) \cdot(\mathbf{c})\) What is the conjugate acid of \(\mathrm{HSO}_{4}^{-}(a q) ?\) What is its conjugate base?

Short Answer

Expert verified
When HSO4- acts as a base in H2O, the following reaction occurs: \( \mathrm{HSO}_{4}^{-}(a q) + \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{SO}_{4}^{2-}(a q) + \mathrm{H}_{3} \mathrm{O}^{+}(a q) \). When HSO4- acts as an acid in H2O, the reaction is: \( \mathrm{HSO}_{4}^{-}(a q) + \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2}\mathrm{SO}_{4}(a q) + \mathrm{OH}^{-}(a q) \). The conjugate acid of HSO4- is H2SO4, and its conjugate base is SO4 2-.

Step by step solution

01

Part A: HSO4- as a base in H2O

When HSO4- acts as a base in H2O, it means the ion is accepting a proton (H+) from water (H2O). The following reaction takes place: \[ \mathrm{HSO}_{4}^{-}(a q) + \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{SO}_{4}^{2-}(a q) + \mathrm{H}_{3} \mathrm{O}^{+}(a q) \]
02

Part B: HSO4- as an acid in H2O

When HSO4- acts as an acid in H2O, the ion is donating a proton to water (H2O). This reaction can be represented as follows: \[ \mathrm{HSO}_{4}^{-}(a q) + \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2}\mathrm{SO}_{4}(a q) + \mathrm{OH}^{-}(a q) \]
03

Part C: Conjugate Acid and Conjugate Base

In the first reaction (Part A), HSO4- is acting as a base, meaning it accepts a proton. When HSO4- accepts a proton, it becomes H2SO4. So, the conjugate acid of HSO4- is H2SO4. In the second reaction (Part B), HSO4- is acting as an acid, meaning it donates a proton. When HSO4- donates a proton, it becomes SO4 2-. Therefore, the conjugate base of HSO4- is SO4 2-.

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Most popular questions from this chapter

In many reactions, the addition of \(\mathrm{AlCl}_{3}\) produces the same effect as the addition of \(\mathrm{H}^{+}\). (a) Draw a Lewis structure for \(\mathrm{AlCl}_{3}\) in which no atoms carry formal charges, and determine its structure using the VSEPR method. (b) What characteristic is notable about the structure in part (a) that helps us understand the acidic character of \(\mathrm{AlCl}_{3}\) ? (c) Predict the result of the reaction between \(\mathrm{AlCl}_{3}\) and \(\mathrm{NH}_{3}\) in a solvent that does not participate as a reactant. (d) Which acid-base theory is most suitable for discussing the similarities between \(\mathrm{AlCl}_{3}\) and \(\mathrm{H}^{+}\) ?

Oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) is a diprotic acid. By using data in Appendix \(\mathrm{D}\) as needed, determine whether each of the following statements is true: (a) \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) can serve as both a Bronsted-Lowry acid and a Brønsted-Lowry base. (b) $\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\( is the conjugate base of \)\mathrm{HC}_{2} \mathrm{O}_{4}^{-}$. (c) An aqueous solution of the strong electrolyte \(\mathrm{KHC}_{2} \mathrm{O}_{4}\) will have \(\mathrm{pH}<7\).

Ephedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic base: $$ \mathrm{C}_{10} \mathrm{H}_{15} \mathrm{ON}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{C}_{10} \mathrm{H}_{15} \mathrm{ONH}^{+}(a q)+\mathrm{OH}^{-}(a q) $$ A \(0.035 \mathrm{M}\) solution of ephedrine has a \(\mathrm{pH}\) of 11.33 . (a) What are the equilibrium concentrations of $\mathrm{C}_{10} \mathrm{H}_{15} \mathrm{ON}, \mathrm{C}_{10} \mathrm{H}_{15} \mathrm{ONH}^{+},\( and \)\mathrm{OH}^{-} ?$ (b) Calculate \(K_{b}\) for ephedrine.

Which member of each pair produces the more acidic aqueous solution: \((\mathbf{a}) \mathrm{Zn} \mathrm{Br}_{2}\) or \(\mathrm{CdCl}_{2},\) (b) \(\mathrm{CuCl}\) or \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\), (c) \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) or \(\mathrm{NiBr}_{2} ?\)

Calculate \(\left[\mathrm{H}^{+}\right]\) for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) $\left[\mathrm{OH}^{-}\right]=7.3 \times 10^{-10} \mathrm{M}(\mathbf{b})\left[\mathrm{OH}^{-}\right]=0.015 \mathrm{M} ;$ (c) a solution in which \(\left[\mathrm{H}^{+}\right]\) is 10 times greater than \(\left[\mathrm{OH}^{-}\right]\).
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