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Chapter 13: Problem 40

Rank the following solutions in order of increasing \(\left[\mathrm{H}^{+}\right]\). \(\begin{array}{llll}0.1 & M \mathrm{HBr}, & 0.1 \mathrm{M} \mathrm{HF}, & 0.1 \mathrm{MHCHO}_{2} & 0.1 \mathrm{MHCN}\end{array}\)

Short Answer

Expert verified
Question: Arrange the following solutions in order of increasing proton concentration: 0.1 M HBr, 0.1 M HF, 0.1 M HCHO2, and 0.1 M HCN. Answer: HCN, HCHO2, HF, HBr

Step by step solution

01

Identify the Acids and their Dissociation Constants

The given solutions contain the following acids: 1. Hydrobromic Acid (HBr) 2. Hydrofluoric Acid (HF) 3. Formic Acid (HCHO2) 4. Hydrocyanic Acid (HCN) The acids dissociation constants ( \(K_a\) ) are: 1. HBr: \(K_a = 10^{9}\) 2. HF: \(K_a = 6.76 × 10^{-4}\) 3. HCHO2: \(K_a = 1.8 × 10^{-4}\) 4. HCN: \(K_a = 6.2 × 10^{-10}\)
02

Determine the Concentration of protons (\(\left[\mathrm{H}^{+}\right]\)) for each acid

The concentration of protons for a given acid can be approximated using the following formula: \(\left[\mathrm{H}^{+}\right] \approx \sqrt{K_a × M}\) For the given acids: 1. HBr: \(\left[\mathrm{H}^{+}\right] \approx \sqrt{10^{9} × 0.1} = 10^{4}\) 2. HF: \(\left[\mathrm{H}^{+}\right] \approx \sqrt{6.76 × 10^{-4} × 0.1} = 8.21× 10^{-3}\) 3. HCHO2: \(\left[\mathrm{H}^{+}\right] \approx \sqrt{1.8 × 10^{-4} × 0.1} = 4.24× 10^{-3}\) 4. HCN: \(\left[\mathrm{H}^{+}\right] \approx \sqrt{6.2 × 10^{-10} × 0.1} = 7.87 × 10^{-6}\)
03

Rank the Acids in Order of Increasing Proton Concentration

Now, arrange the acids based on increasing \(\left[\mathrm{H}^{+}\right]\): 1. Hydrocyanic Acid (HCN): \(\left[\mathrm{H}^{+}\right] = 7.87 × 10^{-6}\) 2. Formic Acid (HCHO2): \(\left[\mathrm{H}^{+}\right] = 4.24 × 10^{-3}\) 3. Hydrofluoric Acid (HF): \(\left[\mathrm{H}^{+}\right] = 8.21 × 10^{-3}\) 4. Hydrobromic Acid (HBr): \(\left[\mathrm{H}^{+}\right] = 10^{4}\) The correct order in terms of increasing proton concentration is HCN, HCHO2, HF, and HBr.

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Most popular questions from this chapter

According to the Brønsted-Lowry theory, which of the following would you expect to act as an acid? Which as a base? (a) \(\mathrm{CHO}_{2}^{-}\) (b) \(\mathrm{NH}_{4}^{+}\) (c) \(\mathrm{HSO}_{3}^{-}\)

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