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Chapter 14: Problem 37

Of the hydrogen halides, only \(\mathrm{HF}\) is a weak acid. Give a possible explanation.

Short Answer

Expert verified
HF is a weak acid among the hydrogen halides because of its high bond strength and the high electronegativity of fluorine. The strong H-F bond and fluorine's strong pull on bonding electrons make HF less likely to donate a proton in solution, resulting in its weak acidity. On the other hand, HCl, HBr, and HI have weaker bonds and are more likely to donate protons, classifying them as strong acids.

Step by step solution

01

Understanding the properties of hydrogen halides

Hydrogen halides are binary compounds formed from hydrogen and a halogen (Group 17 element). They include HF, HCl, HBr, and HI. Generally, these compounds are acidic in nature when dissolved in water.
02

Understanding strong and weak acids

Acids can be classified as strong or weak based on their ability to dissociate into their constituent ions in water. A strong acid completely dissociates into its constituent ions, while a weak acid only partially dissociates. In other words, a strong acid has a stronger tendency to donate a proton (H+), whereas a weak acid has a lesser tendency to donate a proton.
03

Comparing the bond strength of hydrogen halides

The strength of an acid is mainly determined by the bond strength between hydrogen and the halogen. The bond strength decreases as we go down the periodic table because the size of the halogen atom increases, making it easier to break the bond. In the case of hydrogen halides, the bond strength decreases in the order HF > HCl > HBr > HI.
04

Explaining the weaker acidity of HF

Although HF has the highest bond strength among the hydrogen halides, it is a weak acid. The reason lies in the fact that the fluorine atom has a very high electronegativity, which means it strongly attracts the bonding electrons, making the H-F bond more polar. As a result, HF is more reluctant to lose a proton (H+) due to the strong pull from the electronegative fluorine atom. Therefore, HF only partially donates a proton (H+) in the solution, making it a weak acid.
05

Comparing the acidity of other hydrogen halides

Now let's consider the other hydrogen halides. The bond strength decreases as we go down the group, so HCl, HBr, and HI have weaker bonds than HF. This means they can more easily lose a proton (H+) in solution, making them strong acids. Since their bond strengths are weaker relative to HF, the electron pull from the halogen atom does not prevent their proton donation as much as it does in HF. Therefore, HCl, HBr, and HI are strong acids. In conclusion, HF is a weak acid among the hydrogen halides because its bond strength is higher than the other hydrogen halides, and the high electronegativity of fluorine makes it less likely to donate a proton in solution.

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