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Chapter 15: Problem 69

Predict the acid strengths of the following compounds: \(\mathrm{H}_{2} \mathrm{O}, \mathrm{H}_{2} \mathrm{~S},\) and \(\mathrm{H}_{2} \mathrm{Se}\).

Short Answer

Expert verified
H2Se > H2S > H2O, indicating that H2Se is the strongest acid followed by H2S and H2O.

Step by step solution

01

Analyzing the Acids

Let's start by working with the concept that these compounds are all binary hydrides of the Oxygen family (Group 16 elements). As we move from top to bottom in this group, the size of the atom increases, thus the bond strength decreases. This will hint us towards the conclusion about acid strength among these compounds.
02

Comparing the Acid Strength

The acid strength of these compounds can be compared based on the strength of the H−X bond and the stability of the X− ion in solution. When we go down the group, the bond strength decreases because the size of the atom increases. Thus, the bond length increases and it becomes easier to remove a proton (H⁺). Additionally, the larger anions are more polarizable, meaning they can spread out their negative charge over a larger volume, making the anions more stable. Therefore, we can say the acidity increases as we move down this group from oxygen to selenium.
03

Concluding the Acid Strength

Based on the previous steps, we can say that H2Se is the strongest acid followed by H2S and then followed by H2O. This is because Selenium is larger than sulfur and oxygen, and thus has weaker H-Se bonds, making H2Se more likely to donate a proton.

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Most popular questions from this chapter

Classify the following oxides as acidic, basic, amphoteric, or neutral: (a) \(\mathrm{CO}_{2},\) (b) \(\mathrm{K}_{2} \mathrm{O},\) (c) \(\mathrm{CaO}\), (d) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (e) CO, (f) \(\mathrm{NO}\) (g) \(\mathrm{SnO}_{2}\), (h) \(\mathrm{SO}_{3}\), (i) \(\mathrm{Al}_{2} \mathrm{O}_{3},(\mathrm{j}) \mathrm{BaO}\)

Compare the strengths of the following pairs of acids: (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(\mathrm{H}_{2} \mathrm{SeO}_{4}\), (b) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) and \(\mathrm{H}_{3} \mathrm{AsO}_{4}\).

Which of the following has a higher pH: (a) \(0.20 \mathrm{M}\) \(\mathrm{NH}_{3},\) (b) \(0.20 \mathrm{M} \mathrm{NaOH} ?\)

The \(K_{\mathrm{a}}\) for benzoic acid is \(6.5 \times 10^{-5} .\) Calculate the \(\mathrm{pH}\) of a \(0.10 \mathrm{M}\) benzoic acid solution.

The three common chromium oxides are \(\mathrm{CrO}\), \(\mathrm{Cr}_{2} \mathrm{O}_{3},\) and \(\mathrm{CrO}_{3} .\) If \(\mathrm{Cr}_{2} \mathrm{O}_{3}\) is amphoteric, what can you say about the acid-base properties of \(\mathrm{CrO}\) and \(\mathrm{CrO}_{3} ?\)
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