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Chapter 16: Problem 14

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

Short Answer

Expert verified
The false statement is (e) - Any compound that contains an \(-\)OH group acts as a Bronsted-Lowry base. Not all compounds with an \(-\)OH group act as Bronsted-Lowry bases, such as alcohols.

Step by step solution

01

Identify Arrhenius base properties

According to the Arrhenius theory, a base is a substance that increases the concentration of hydroxide ions (OH\(^⁻\)) in water when dissolved. That means an Arrhenius base makes the solution more alkaline.
02

Identify Bronsted-Lowry base and acid properties

The Bronsted-Lowry theory defines a base as a proton (H\(^+\)) acceptor and an acid as a proton donor. In this theory, bases and acids can only react with each other in a process called proton transfer.
03

Recognize the role of water in the Bronsted-Lowry theory

According to the Bronsted-Lowry theory, water can indeed act as both an acid and a base. For example, when an acid dissolves in water, water will act as a base by accepting a proton. Conversely, when a base dissolves in water, water will act as an acid by donating a proton.
04

Considering compounds with an \(-\)OH group

Compounds with an \(-\)OH group can sometimes act as Bronsted-Lowry bases by accepting a proton. However, not all compounds with an \(-\)OH group will necessarily act as a Bronsted-Lowry base. For example, alcohols such as ethanol (C\(_2\)H\(_5\)OH) have an \(-\)OH group but do not behave as Bronsted-Lowry bases in reactions.
05

Verify each statement from the exercise

(a) An Arrhenius base increases the concentration of OH\(^⁻\) in water - This statement is true. (b) A Bronsted-Lowry base is a proton acceptor - This statement is also true. (c) Water can act as a Bronsted-Lowry acid - This statement is true. (d) Water can act as a Bronsted-Lowry base - This statement is true. (e) Any compound that contains an \(-\)OH group acts as a Bronsted-Lowry base - This statement is false, as not all compounds with an \(-\)OH group act as Bronsted-Lowry bases, such as alcohols. The false statement is (e).

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Most popular questions from this chapter

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) \(\left[\mathrm{H}^{+}\right]=\left[\mathrm{OH}^{-}\right],\) or (iii) \(\left[\mathrm{H}^{+}\right]<\left[\mathrm{OH}^{-}\right] ?\)

(a) Give the conjugate base of the following Bronsted-Lowry acids: (i) HCOOH, (ii) \(\mathrm{HPO}_{4}^{2-} .\) (b) Give the conjugate acid of the following Bronsted-Lowry bases: (i) SO \(_{4}^{2-}\) (ii) \(\mathrm{CH}_{3} \mathrm{NH}_{2} .\)

The active ingredient in aspirin is acetylsalicylic acid \(\left(\mathrm{HC}_{9} \mathrm{H}_{7} \mathrm{O}_{4}\right),\) a monoprotic acid with \(K_{a}=3.3 \times 10^{-4}\) at \(25^{\circ} \mathrm{C} .\) What is the pH of a solution obtained by dissolving two extra-strength aspirin tablets, containing 500 \(\mathrm{mg}\) of acetylsalicylic acid each, in 250 \(\mathrm{mL}\) of water?

Identify the Lewis acid and Lewis base in each of the following reactions: (a) \(\mathrm{HNO}_{2}(a q)+\mathrm{OH}^{-}(a q) \rightleftharpoons \mathrm{NO}_{2}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) (b) \(\mathrm{FeBr}_{3}(s)+\mathrm{Br}^{-}(a q) \rightleftharpoons \mathrm{FeBr}_{4}^{-}(a q)\) (c) \(\mathrm{Zn}^{2+}(a q)+4 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}^{2+}(a q)\) (d) \(\mathrm{SO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}_{3}(a q)\)

Benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right)\) and aniline \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\right)\) are both derivatives of benzene. Benzoic acid is an acid with \(K_{a}=6.3 \times 10^{-5}\) and aniline is a base with \(K_{a}=4.3 \times 10^{-10} .\) (a) What are the conjugate base of benzoic acid and the conjugate acid of aniline? (b) Anilinium chloride \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3} \mathrm{Cl}\right)\) is a strong electrolyte that dissociates into anilinium ions \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}\right)\) and chloride ions. Which will be more acidic, a 0.10\(M\) solution of benzoic acid or a 0.10 M solution of anilinium chloride? (c) What is the value of the equilibrium constant for the following equilibrium? $$\begin{array}{c}{\mathrm{C}_{6} \mathrm{H}_{5} \operatorname{COOH}(a q)+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}(a q) \rightleftharpoons} \\\ \quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad\quad {\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COO}^{-}(a q)+\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}(a q)}\end{array}$$
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