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Chapter 13: Problem 33

Of the hydrogen halides, only HF is a weak acid. Give a possible explanation.

Short Answer

Expert verified
HF is a weak acid among hydrogen halides due to the stronger bond between hydrogen and fluorine and the higher electronegativity of fluorine. These factors make it more difficult for HF to dissociate and release H+ ions in a solution, compared to other hydrogen halides.

Step by step solution

01

Identify the hydrogen halides

Hydrogen halides are binary compounds of hydrogen with halogen elements, and they include the following: hydrogen fluoride (HF), hydrogen chloride (HCl), hydrogen bromide (HBr), and hydrogen iodide (HI).
02

Understand acidity strength

The strength of an acid is determined by its ability to donate a proton (H+) to a solution. A strong acid will dissociate completely, releasing more H+ ions, while a weak acid will only partially dissociate, releasing fewer H+ ions.
03

Analyze bond strength

One of the factors affecting the acidity of a compound is the strength of the bond between hydrogen and the halogen atom. The weaker the bond, the easier it is for the compound to dissociate and release H+ ions. The bond strength decreases as the size of the halogen atoms increases, meaning that the bond between hydrogen and fluorine (in HF) is stronger compared to that with other halogens, making it more difficult to dissociate and release H+ ions.
04

Consider electronegativity

Another essential factor in determining acidity is the electronegativity of the halogen atoms. A higher electronegativity implies that the atom has a greater ability to attract the shared electron pair in the molecule. Fluorine is the most electronegative element, meaning it holds the electrons more tightly compared to the other halogen atoms. This strong attraction further results in the HF bond being difficult to dissociate, thus making HF a weak acid.
05

Conclusion

The reason why HF is a weak acid among hydrogen halides is due to its stronger bond between hydrogen and fluorine, and the higher electronegativity of fluorine. These factors make it more difficult for HF to dissociate and release H+ ions in a solution, making it a weak acid compared to the other hydrogen halides.

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Most popular questions from this chapter

Consider a \(0.60-M\) solution of \(\mathrm{HC}_{3} \mathrm{H}_{5} \mathrm{O}_{3},\) lactic acid \(\left(K_{\mathrm{a}}=\right.\) \(\left.1.4 \times 10^{-4}\right)\) a. Which of the following are major species in the solution? i. \(\mathrm{HC}_{3} \mathrm{H}_{5} \mathrm{O}_{3}\) ii. \(\mathrm{C}_{3} \mathrm{H}_{5} \mathrm{O}_{3}^{-}\) iii. \(\mathrm{H}^{+}\) iv. \(\mathrm{H}_{2} \mathrm{O}\) \(\mathbf{v} . \mathrm{OH}^{-}\) b. Complete the following ICE table in terms of \(x,\) the amount (mol/L) of lactic acid that dissociates to reach equilibrium. c. What is the equilibrium concentration for \(\mathrm{C}_{3} \mathrm{H}_{5} \mathrm{O}_{3}^{-} ?\) d. Calculate the \(p H\) of the solution.

A certain acid, HA, has a vapor density of \(5.11 \mathrm{g} / \mathrm{L}\) when in the gas phase at a temperature of \(25^{\circ} \mathrm{C}\) and a pressure of 1.00 atm. When 1.50 g of this acid is dissolved in enough water to make 100.0 mL of solution, the \(p\) H is found to be \(1.80 .\) Calculate \(K_{\mathrm{a}}\) for the acid.

Monochloroacetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{2} \mathrm{ClO}_{2}\), is a skin irritant that is used in "chemical peels" intended to remove the top layer of dead skin from the face and ultimately improve the complexion. The value of \(K_{\mathrm{a}}\) for monochloroacetic acid is \(1.35 \times 10^{-3}\) Calculate the \(\mathrm{pH}\) of a \(0.10-M\) solution of monochloroacetic acid.

A typical sample of vinegar has a pH of \(3.0 .\) Assuming that vinegar is only an aqueous solution of acetic acid \(\left(K_{a}=1.8 \times\right.\) \(10^{-5}\) ), calculate the concentration of acetic acid in vinegar.

A solution is prepared by adding \(50.0 \mathrm{mL}\) of \(0.050 \mathrm{M}\) HBr to 150.0 mL of 0.10 \(M\) HI. Calculate \(\left[\mathrm{H}^{+}\right]\) and the pH of this solution. HBr and HI are both considered strong acids.
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