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Chapter 16: Problem 41

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 \(\mathrm{pH}=1.0\)

Short Answer

Expert verified
(a) True: Strong acids must contain one or more H atoms to donate as protons (H+) in a solution. (b) True: Strong acids are strong electrolytes, as they fully ionize in a solution, releasing all of their protons as H3O+ ions. (c) False: A 1.0-M solution of a strong acid will have a pH of 0, not 1.0, as \(\mathrm{pH} = -\log_{10}(1) = 0\).

Step by step solution

01

Statement (a): All strong acids contain one or more H atoms.

For an acid to behave as an acid, it has to donate a proton (H+) in a solution. Therefore, a strong acid must contain one or more H atoms to be able to donate them. Hence, statement (a) is true.
02

Statement (b): A strong acid is a strong electrolyte.

When an acid dissolves in water, it donates protons (H+) to the solution, creating hydronium ions (H3O+). A strong acid completely ionizes in water, releasing all of its protons as H3O+ ions. This would increase the conductivity of the solution, as more ions would be available to carry electrical charge. A strong electrolyte is a substance that completely dissociates into ions when dissolved in water. Since strong acids fully ionize in a solution, they are strong electrolytes. Therefore, statement (b) is true.
03

Statement (c): A 1.0-M solution of a strong acid will have \(\mathrm{pH}=1.0\).

The pH of a solution is calculated using the equation \(\mathrm{pH} = -\log_{10}[\mathrm{H^{+}}]\), where \([\mathrm{H^{+}}]\) represents the concentration of H+ ions in the solution. In a 1.0-M solution of a strong acid, the concentration of H+ ions will be 1.0 M, since the strong acid completely ionizes in water. Plugging the value into the pH equation, we get:\[\mathrm{pH} = -\log_{10}(1) = 0\] Therefore, a 1.0-M solution of a strong acid will have a pH of 0, not 1.0. So, statement (c) is false.

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Most popular questions from this chapter

(a) Given that \(K_{a}\) for cyanic acid is \(3.5 \times 10^{-4}\) and that for hydrofluoric acid is \(6.8 \times 10^{-4},\) which is the stronger acid? (b) Which is the stronger base, the cyanate ion or the fluoride ion? (c) Calculate \(K_{b}\) values for \(\mathrm{NCO}^{-}\) and \(\mathrm{F}^{-}\).

If a neutral solution of water, with \(\mathrm{pH}=7.00,\) is cooled to \(10^{\circ} \mathrm{C},\) the pH rises to \(7.27 .\) Which of the following three statements is correct for the cooled water: (i) \(\left[\mathrm{H}^{+}\right]>\left[\mathrm{OH}^{-}\right]\) (ii) \(\left[\mathrm{H}^{+}\right]=\left[\mathrm{OH}^{-}\right], \mathrm{or}\) (iii) \(\left[\mathrm{H}^{+}\right]<\left[\mathrm{OH}^{-}\right] ?\)

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

(a) Using dissociation constants from Appendix D, determine the value for the equilibrium constant for each of the following reactions. (i) $\mathrm{HCO}_{3}^{-}(a q)+\mathrm{OH}^{-}(a q) \rightleftharpoons \mathrm{CO}_{3}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$ (ii) $\mathrm{NH}_{4}^{+}(a q)+\mathrm{CO}_{3}^{2-}(a q) \rightleftharpoons \mathrm{NH}_{3}(a q)+\mathrm{HCO}_{3}^{-}(a q)$ (b) We usually use single arrows for reactions when the forward reaction is appreciable ( \(K\) much greater than 1) or when products escape from the system, so that equilibrium is never established. If we follow this convention, which of these equilibria might be written with a single arrow?

Based on their compositions and structures and on conjugate acid-base relationships, select the stronger base in each of the following pairs: (a) \(\mathrm{NO}_{3}^{-}\) or \(\mathrm{NO}_{2}^{-},\) (b) \(\mathrm{PO}_{4}^{3-}\) or \(\mathrm{AsO}_{4}^{3-}\), (c) \(\mathrm{HCO}_{3}^{-}\) or \(\mathrm{CO}_{3}^{2-}\).
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