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Chapter 16: Problem 14

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.

Short Answer

Expert verified
The false statement is (e): Any compound that contains an -OH group acts as a Brønsted-Lowry base.

Step by step solution

01

Statement (a)

An Arrhenius base is a substance that produces hydroxide ions (\(\mathrm{OH}^{-}\)) when dissolved in water. Therefore, according to Arrhenius definition, this statement is true.
02

Statement (b)

A Brønsted-Lowry base is defined as a proton acceptor, meaning that it can accept a hydrogen ion (\(\mathrm{H}^{+}\)) from another substance. This is the main concept of the Brønsted-Lowry definition, making this statement also true.
03

Statement (c)

Water (\(\mathrm{H}_{2}\mathrm{O}\)) can indeed act as a Brønsted-Lowry acid, as it can donate a hydrogen ion (\(\mathrm{H}^{+}\)) to another substance. For example, when water reacts with ammonia, it donates a hydrogen ion to form the ammonium ion and hydroxide ion. Thus, this statement is true.
04

Statement (d)

Water can also act as a Brønsted-Lowry base because it can accept a hydrogen ion from another substance. When water reacts with an acid, it accepts a hydrogen ion to form the hydronium ion (\(\mathrm{H}_{3}\mathrm{O}^{+}\)). This behavior confirms that this statement is true.
05

Statement (e)

While many compounds containing an -OH group (hydroxyl group) can act as Brønsted-Lowry bases, it is not universally true for all compounds. Some compounds, like alcohols, do not readily donate or accept protons in water, and thus do not behave as bases. Therefore, this statement is false. The result is, the false statement is (e): Any compound that contains an -OH group acts as a Brønsted-Lowry base.

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Most popular questions from this chapter

A \(0.100 \mathrm{M}\) solution of bromoacetic acid $\left(\mathrm{BrCH}_{2} \mathrm{COOH}\right)$ is 13.2\% ionized. Calculate $\left[\mathrm{H}^{+}\right],\left[\mathrm{BrCH}_{2} \mathrm{COO}^{-}\right],\left[\mathrm{BrCH}_{2} \mathrm{COOH}\right]$ and \(K_{a}\) for bromoacetic acid.

Indicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true. (a) Acid strength in a series of \(\mathrm{H}-\mathrm{A}\) molecules increases with increasing size of A. (b) For acids of the same general structure but differing electronegativities of the central atoms, acid strength decreases with increasing electronegativity of the central atom. (c) The strongest acid known is HF because fluorine is the most electronegative element.

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Based on their compositions and structures and on conjugate acid-base relationships, select the stronger base in each of the following pairs: (a) \(\mathrm{BrO}^{-}\) or \(\mathrm{ClO}^{-},(\mathbf{b}) \mathrm{BrO}^{-}\) or \(\mathrm{BrO}_{2}^{-}\), (c) \(\mathrm{HPO}_{4}^{2-}\) or $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$.

Codeine \(\left(\mathrm{C}_{18} \mathrm{H}_{21} \mathrm{NO}_{3}\right)\) is a weak organic base. A \(5.0 \times 10^{-3} \mathrm{M}\) solution of codeine has a pH of 9.95. Calculate the value of \(K_{b}\) for this substance. What is the \(\mathrm{p} K_{b}\) for this base?
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