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Chapter 2: Problem 3

A solution of sulfurous acid, \(\mathrm{H}_{2} \mathrm{SO}_{3}\) , is present in an aqueous solution. Which of the following represents the concentrations of three different ions in solution? (A) \(\left[\mathrm{SO}_{3}^{2-}\right]>\left[\mathrm{HSO}_{3}^{-}\right]>\left[\mathrm{H}_{2} \mathrm{SO}_{3}\right]\) (B) \(\left[\mathrm{H}_{2} \mathrm{SO}_{3}\right]>\left[\mathrm{HSO}_{3}^{-}\right]>\left[\mathrm{SO}_{3}^{2-}\right]\) (C) \(\left[\mathrm{H}_{2} \mathrm{SO}_{3}\right]>\left[\mathrm{HSO}_{3}^{-}\right]=\left[\mathrm{SO}_{3}^{2-}\right]\) (D) \(\left[\mathrm{SO}_{3}^{2-}\right]=\left[\mathrm{HSO}_{3}^{-}\right]>\left[\mathrm{H}_{2} \mathrm{SO}_{3}\right]\)

Short Answer

Expert verified
The correct representation of the ion concentration in a solution of sulfurous acid is (B) \( [\mathrm{H}_{2}\mathrm{SO}_{3}] > [\mathrm{HSO}_{3}^{-}] > [\mathrm{SO}_{3}^{2-}] \).

Step by step solution

01

Understand the Ionization of Sulfurous Acid

Sulfurous acid is a weak acid and it ionizes in water in a step-by-step manner. It is important to remember that weak acids do not ionize completely. The first step of ionization of sulfurous acid produces bisulfite ion and a proton, i.e., \( \mathrm{H}_{2} \mathrm{SO}_{3} \) \( \leftrightarrow \mathrm{HSO}_{3}^{-} + \mathrm{H}^{+} \). The bisulfite ion can then further ionize to sulfate ion and another proton, \( \mathrm{HSO}_{3}^{-} \leftrightarrow \mathrm{SO}_{3}^{2-} + \mathrm{H}^{+} \).
02

Analyze the Equilibrium State of the Acid Ionization

In the equilibrium state of a weak acid solution, the major species present are the weak acid itself and the first ionized species. The second ionization produces ions in much lesser quantities. Thus, in sulfurous acid solution, the concentration of \( \mathrm{H}_{2}\mathrm{SO}_{3} \) is more than \( \mathrm{HSO}_{3}^{-} \), and \( \mathrm{HSO}_{3}^{-} \) is more than \( \mathrm{SO}_{3}^{2-} \).
03

Choose the Correct Option

Given the result of the previous step, the correct option can be chosen. In this case, \( [\mathrm{H}_{2} \mathrm{SO}_{3}] > [\mathrm{HSO}_{3}^{-}] > [\mathrm{SO}_{3}^{2-}] \) best represents the state of the sulfurous acid solution, so the correct option is (B).

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Most popular questions from this chapter

Most transition metals share a common oxidation state of \(+2 .\) Which of the following best explains why? (A) Transition metals all have a minimum of two unpaired electrons. (B) Transition metals have unstable configurations and are very reactive. (C) Transition metals tend to gain electrons when reacting with other elements. (D) Transition metals will lose their outermost s-block electrons when forming bonds.

\(\mathrm{SF}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{SO}_{2}(g)+4 \mathrm{HF}(g) \Delta H=-828 \mathrm{kJ} / \mathrm{mol}\) Which of the following statements accurately describes the above reaction? (A) The entropy of the reactants exceeds that of the products. (B) \(\mathrm{H}_{2} \mathrm{O}(l)\) will always be the limiting reagent. (C) This reaction is never thermodynamically favored. (D) The temperature of the surroundings will increase as this reaction Progresses.

A sample of \(\mathrm{H}_{2} \mathrm{S}\) gas is placed in an evacuated, sealed container and heated until the following decomposition reaction occurs at \(1000 \mathrm{K} :\) $$2 \mathrm{H}_{2} \mathrm{S}(g) \rightarrow 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) \qquad K_{\mathrm{c}}=1.0 \times 10^{-6}$$ As the reaction progresses at a constant temperature of 1000 K, how does the value for the Gibbs free energy constant for the reaction change? (A) It stays constant. (B) It increases exponentially. (C) It increases linearly. (D) It decreases exponentially.

A compound is made up of entirely silicon and oxygen atoms. If there are 14.0 g of silicon and 32.0 g of oxygen present, what is the empirical formula of the compound? (A) \(\mathrm{SiO}_{2}\) (B) \(\mathrm{SiO}_{4}\) (C) \(\mathrm{Si}_{2} \mathrm{O}\) (D) \(\mathrm{Si}_{2} \mathrm{O}_{3}\)

An unknown substance is found to have a high melting point. In addition, it is a poor conductor of electricity and does not dissolve in water. The substance most likely contains (A) ionic bonding (B) nonpolar covalent bonding (C) covalent network bonding (D) metallic bonding
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