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Chapter 16: Problem 25

(a) Which of the following is the stronger Br酶nstedLowry acid, \(\mathrm{HBrO}\) or \(\mathrm{HBr}\) ? (b) Which is the stronger Br酶nsted-Lowry base, \(\mathrm{F}^{-}\) or \(\mathrm{Cl}^{-} ?\) Briefly explain your choices.

Short Answer

Expert verified
The stronger Br酶nsted-Lowry acid is \(\mathrm{HBr}\), as its conjugate base, \(\mathrm{Br^-}\), is less stable than the conjugate base of \(\mathrm{HBrO}\), \(\mathrm{BrO^-}\). The stronger Br酶nsted-Lowry base is \(\mathrm{F^-}\), as its conjugate acid, \(\mathrm{HF}\), is less stable than the conjugate acid of \(\mathrm{Cl^-}\), \(\mathrm{HCl}\). This is due to the high electronegativity of fluorine making it less likely to donate a proton.

Step by step solution

01

A Br酶nsted-Lowry acid is a substance that can donate a proton (H+) to another substance. The strength of the acid depends on its ability to donate a proton. #Step 2: Analyze the stability of the conjugate base#

The stronger the acid, the more stable its conjugate base (the species formed after the acid loses a proton) is. We will compare the stability of the conjugate bases of \(\mathrm{HBrO}\) and \(\mathrm{HBr}\) to determine which acid is stronger. #Step 3: Compare conjugate bases of HBrO and HBr#
02

The conjugate base of \(\mathrm{HBrO}\) is \(\mathrm{BrO^-}\) and the conjugate base of \(\mathrm{HBr}\) is \(\mathrm{Br^-}\). The \(\mathrm{BrO^-}\) ion has a stronger electron withdrawing group (oxygen) compared to the \(\mathrm{Br^-}\) ion. This makes \(\mathrm{BrO^-}\) more stable and thus, \(\mathrm{HBrO}\) a weaker acid than \(\mathrm{HBr}\). So, the stronger Br酶nsted-Lowry acid is \(\mathrm{HBr}\). #b) Comparing base strength: F- vs Cl-# #Step 1: Understand Br酶nsted-Lowry base definition#

A Br酶nsted-Lowry base is a substance that can accept a proton (H+) from another substance. The strength of the base depends on its ability to accept a proton. #Step 2: Analyze the stability of the conjugate acids#
03

The stronger the base, the less stable its conjugate acid (the species formed after the base gains a proton) is. We will compare the stability of the conjugate acids of \(\mathrm{F^-}\) and \(\mathrm{Cl^-}\) to determine which base is stronger. #Step 3: Compare conjugate acids of F- and Cl-#

The conjugate acid of \(\mathrm{F^-}\) is \(\mathrm{HF}\) and the conjugate acid of \(\mathrm{Cl^-}\) is \(\mathrm{HCl}\). The \(\mathrm{HF}\) molecule is a weaker acid compared to \(\mathrm{HCl}\) due to the high electronegativity of fluorine, making it less likely to donate a proton. Hence, its conjugate base \(\mathrm{F^-}\) is a stronger base compared to \(\mathrm{Cl^-}\). So, the stronger Br酶nsted-Lowry base is \(\mathrm{F^-}\).

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Most popular questions from this chapter

Calculate \(\left[\mathrm{OH}^{-}\right]\) and \(\mathrm{pH}\) for (a) \(1.5 \times 10^{-3} \mathrm{M} \mathrm{Sr}(\mathrm{OH})_{2}\) (b) \(2.250 \mathrm{~g}\) of \(\mathrm{LiOH}\) in \(250.0 \mathrm{~mL}\) of solution, \((c) 1.00 \mathrm{~mL}\) of \(0.175 \mathrm{M} \mathrm{NaOH}\) diluted to \(2.00 \mathrm{~L}\), (d) a solution formed by adding \(5.00 \mathrm{~mL}\) of \(0.105 \mathrm{M} \mathrm{KOH}\) to \(15.0 \mathrm{~mL}\) of \(9.5 \times 10^{-2} \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}\).

Predict the products of the following acid-base reactions, and predict whether the equilibrium lies to the left or to the right of the equation: (a) \(\mathrm{NH}_{4}{ }^{+}(a q)+\mathrm{OH}^{-}(a q) \rightleftharpoons\) (b) \(\mathrm{CH}_{3} \mathrm{COO}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q) \rightleftharpoons\) (c) \(\mathrm{HCO}_{3}^{-}(a q)+\mathrm{F}^{-}(a q) \rightleftharpoons\)

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Label each of the following as being a strong acid, a weak acid, or a species with negligible acidity. In each case write the formula of its conjugate base, and indicate whether the conjugate base is a strong base, a weak base, or a species with negligible basicity: (a) \(\mathrm{HNO}_{2}\), (b) \(\mathrm{H}_{2} \mathrm{SO}_{4},(\mathrm{c}) \mathrm{HPO}_{4}{ }^{2-}\) (d) \(\mathrm{CH}_{4}\), (e) \(\mathrm{CH}_{3} \mathrm{NH}_{3}{ }^{+}\) (an ion related to \(\mathrm{NH}_{4}{ }^{+}\) ).

Explain the following observations: (a) \(\mathrm{HCl}\) is a stronger acid than \(\mathrm{H}_{2} \mathrm{~S} ;\) (b) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) is a stronger acid than \(\mathrm{H}_{3} \mathrm{AsO}_{4}\); (c) \(\mathrm{HBrO}_{3}\) is a stronger acid than \(\mathrm{HBrO}_{2}\); (d) \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) is a stronger acid than \(\mathrm{HC}_{2} \mathrm{O}_{4}{ }^{-} ;(\mathrm{e})\) benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right)\) is a stronger acid than phenol \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\right)\).
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