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Chapter 1: Problem 201

Find the number of compounds which are more acidic than \(\mathrm{H}_{2} \mathrm{O}\).

Short Answer

Expert verified
In conclusion, there are a vast number of compounds more acidic than H鈧侽, including various types of acids like organic acids, inorganic acids, and binary acids. It's impossible to provide an exact number, but understanding the characteristics and examples of more acidic compounds, such as hydrochloric acid, sulfuric acid, and citric acid, is more practical and useful.

Step by step solution

01

1. Acids

First, consider various types of acids. Acids are compounds that donate hydrogen ions (H鈦�) when dissolved in water. Their pH typically ranges from 0 to 6.99. Some common examples include hydrochloric acid (HCl), sulfuric acid (H鈧係O鈧�), nitric acid (HNO鈧�), and acetic acid (CH鈧僀OOH).
02

2. Organic Acids

Organic acids are a subset of acids that contain carbon and are found in living organisms. These can include carboxylic acids, such as formic acid (HCOOH) and citric acid (C鈧咹鈧圤鈧�), as well as some amino acids, like aspartic acid and glutamic acid.
03

3. Inorganic Acids

Inorganic acids are another subset of acids that do not contain carbon and are often derived from mineral sources. Some examples include hydrofluoric acid (HF), phosphoric acid (H鈧働O鈧�), and hydrosulfuric acid (H鈧係).
04

4. Binary Acids

Binary acids are another type of weak acid that has one acidic proton and only one other non-metal element, typically hydrogen combined with another element in the periodic table. Examples include hydrogen bromide (HBr) and hydrogen iodide (HI). In conclusion, there is a vast number of compounds more acidic than H鈧侽, including a variety of organic and inorganic acids. As an exact number is impossible to obtain, it is more practical to understand the characteristics of compounds that make them more acidic than water and be able to recognize examples within each category.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Organic Acids
Organic acids are acidic compounds that are found primarily within living organisms. They are characterized by the presence of carbon and often contain the carboxyl group (-COOH). This group is key to their acidic properties, as it can release a hydrogen ion (\(H^+\)), making the compound acidic.
Carboxylic acids, such as formic acid (HCOOH) and citric acid (C鈧咹鈧圤鈧�), are familiar examples. Formic acid is found in ant venom, while citric acid is common in citrus fruits.
  • Carboxylic acids: Feature the carboxyl group and are typically weak acids.
  • Amino acids: Have both acidic and basic properties; examples include aspartic acid and glutamic acid.
  • Lactic acid: Found in sour milk and muscle cells during exercise.
Organic acids generally tend to have mild acidic strength but are significant in biological processes and food industries.
Inorganic Acids
Inorganic acids, also called mineral acids, do not contain carbon as part of their chemical structure. They are derived from minerals, and their acidic strength can range from weak to very strong. These acids often play crucial roles in industrial applications and laboratory settings.
Some well-known inorganic acids include:
  • Hydrochloric acid (HCl): A strong acid used in various industries, including steel manufacturing.
  • Sulfuric acid (H鈧係O鈧�): An essential acid in the production of fertilizers and batteries.
  • Phosphoric acid (H鈧働O鈧�): Commonly used in food and beverages as an acidulating agent.
Inorganic acids are typically stronger than organic acids and are known for their capability to fully dissociate in water, thereby increasing their acidic strength.
pH Scale
The pH scale is a measurement system used to indicate the acidity or basicity of an aqueous solution. It ranges from 0 to 14, with 7 being neutral. Solutions with a pH less than 7 are considered acidic, while those with a pH greater than 7 are basic. The lower the pH value, the more acidic the solution.
Here's how it works:
  • Acidic solutions: Have a pH range of 0 to 6.99. These solutions have a higher concentration of hydrogen ions (\(H^+\)).
  • Neutral solution: Pure water is at pH 7, meaning the concentration of hydrogen ions equals the concentration of hydroxide ions (\(OH^-\)).
  • Basic solutions: Have a pH range from 7.01 to 14. They have more \(OH^-\) ions than \(H^+\) ions.
The pH scale helps in determining the acidity level of compounds, like those more acidic than water, which has a neutral pH of 7.
Binary Acids
Binary acids belong to a unique category of acids consisting of hydrogen and one other non-metal element. They are typically weaker acids compared to polyatomic acids but are essential in chemistry due to their simple composition.
Examples of binary acids include:
  • Hydrogen chloride (HCl): Often known in its aqueous form as hydrochloric acid, which is a strong binary acid.
  • Hydrogen bromide (HBr) and hydrogen iodide (HI): Both are strong acids used in refining and synthesis.
  • Hydrofluoric acid (HF): Although a binary acid, it is unique in its ability to etch glass despite being weaker than HCl.
Binary acids are named based on their component elements and provide significant insight into acidic behavior, particularly when dealing with elemental chemistry and reactions.

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Most popular questions from this chapter

Ambident nucleophile is/are (A) \(\stackrel{\ominus}{\mathrm{CN}}\) (B) \(\stackrel{\ominus}{\mathrm{NO}}_{2}\) (C) (D) \(\stackrel{\ominus}{\mathrm{NO}}_{3}\)

Both compounds are arranged in order of their: (A) Acidic strength (B) Boiling point (C) Dipole moment (D) Solubility in \(\mathrm{H}_{2} \mathrm{O}\)

The compound that does not liberate \(\mathrm{CO}_{2}\) on treatment with aqueous sodium bicarbonate solution is (A) Benzoic acid (B) Benzenesulphonic acid (C) Salicylic acid (D) Carbolic acid (phenol)

The dominating factor for stability of \(t\)-Butyl carbocation is (A) Resonance effect of \(\mathrm{CH}_{3}\) (B) Inductive effect of \(\mathrm{CH}_{3}\) (C) Hyperconjugation of \(\mathrm{CH}_{3}\) (D) Electromeric effect of \(\mathrm{CH}_{3}\)

Which of the following cannot behave like both bronsted acid as well as bronsted base? (A) \(\mathrm{H}_{3} \mathrm{O}^{\oplus}\) (B) \(\mathrm{H}_{2} \mathrm{O}\) (C) \(\mathrm{NH}_{3}\) (D) \(\mathrm{HSO}_{4}^{-}\)
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