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Chapter 2: Problem 23

$$\begin{array}{|c|c|c|}\hline & {\text { Initial pH }} & {\text { PH after NaOH }} \\ \hline \text { Acid 1 } & {3.0} & {3.5} \\ \hline \text { Acid 2 } & {3.0} & {5.0} \\ \hline\end{array}$$ Two different acids with identical pH are placed in separate beakers. Identical portions of NaOH are added to each beaker, and the resulting pH is indicated in the table above. What can be determined about the strength of each acid? (A) Acid 1 is a strong acid and acid 2 is a weak acid because acid 1 resists change in pH more effectively. (B) Acid 1 is a strong acid and acid 2 is a weak acid because the NaOH is more effective at neutralizing acid 2. (C) Acid 1 is a weak acid and acid 2 is a strong acid because the concentration of the weak acid must be significantly greater to have the same pH as the strong acid. (D) Acid 1 is a weak acid and acid 2 is a strong acid because the concentration of the hydrogen ions will be greater in acid 2 after the NaOH addition.

Short Answer

Expert verified
Therefore, option (D) is correct. Acid 1 is a weak acid and Acid 2 is a strong acid because the concentration of the hydrogen ions will be greater in Acid 2 after the NaOH addition.

Step by step solution

01

Understand pH scale

The pH scale provides a measure of the acidity or basicity of a solution. A lower pH indicates a higher concentration of hydrogen ions and therefore a more acidic solution, whereas a higher pH indicates a lower concentration of hydrogen ions and therefore a more basic or alkaline solution.
02

Analyze the given pH changes

Acid 1 starts with a pH of 3.0, and after the addition of NaOH, its pH rises to 3.5. This is a small change in pH, indicating a strong resistance to change, i.e., a high buffering capacity. On the other hand, Acid 2 starts with the same pH of 3.0, but after the addition of NaOH, its pH rises significantly to 5.0, indicating a weak resistance to changing pH, i.e., a low buffering capacity.
03

Determine the strength of the acids

Acids with a high buffering capacity are weak acids because they can resist change in their pH. Conversely, acids with low buffering capacity are strong acids as they do not resist pH change well. Therefore, based on the given data, Acid 1 which showed a minor change in pH is a weak acid while Acid 2, which showed a major change in pH, is a strong acid.

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Most popular questions from this chapter

20.0 \(\mathrm{mL}\) of 1.0 \(\mathrm{M} \mathrm{Na}_{2} \mathrm{CO}_{3}\) is placed in a beaker and titrated with a solution of \(1.0 \mathrm{M} \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2},\) resulting in the creation of a precipitate. If the experiment were repeated and the \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) was diluted to 40.0 \(\mathrm{mL}\) with distilled water prior to the titration, how would that affect the volume of \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) needed to reach the equivalence point? (A) It would be cut in half. (B) It would decrease by a factor of 1.5. (C) It would double. (D) It would not change.

Consider the Lewis structures for the following molecules: $$\begin{equation} \mathrm{CO}_{2}, \mathrm{CO}_{3}^{2-}, \mathrm{NO}_{2}^{-}, \text {and } \mathrm{NO}_{3}^{-} \end{equation}$$ Which molecule or molecules exhibit \(s p^{2}\) hybridization around the central atom? (A) \(\mathrm{CO}_{2}\) and \(\mathrm{CO}_{3}^{2-}\) (B) \(\mathrm{NO}_{2}^{-}\) and \(\mathrm{NO}_{3^{-}}\) (C) \(\mathrm{CO}_{3}^{2-}\) and \(\mathrm{NO}_{3}^{-}\) (D) \(\mathrm{CO}_{3}^{2-}, \mathrm{NO}_{2}^{-},\) and \(\mathrm{NO}_{3}^{-}\)

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) \(\left[\mathrm{SO}_{3}^{2-}\right]=\left[\mathrm{HSO}_{3}^{-}\right]>\left[\mathrm{H}_{2} \mathrm{SO}_{3}\right]\)

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) \(\mathrm{Si}_{2} \mathrm{O}_{3}\)

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.
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