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Magazine Chapter 14: Problem 92
Classify each of these as a strong acid, weak acid, strong base, weak base, amphiprotic substance, or neither acid nor base. (a) \(\mathrm{CH}_{3} \mathrm{COOH}\) (b) \(\mathrm{Na}_{2} \mathrm{O}\) (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (d) \(\mathrm{NH}_{3}\) (e) \(\mathrm{Ba}(\mathrm{OH})_{2}\) (f) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)
Short Answer
Expert verified
(a) Weak acid, (b) Neither, (c) Strong acid, (d) Weak base, (e) Strong base, (f) Amphiprotic.
Step by step solution
01
Identify Acetic Acid
(a) \( \mathrm{CH}_{3}\mathrm{COOH} \) is acetic acid, which is a weak acid. Although it can donate a proton, it doesn't completely ionize in water.
02
Identify Sodium Oxide
(b) \( \mathrm{Na}_{2}\mathrm{O} \) is a basic anhydride and reacts with water to form \( \mathrm{NaOH} \), a strong base. Therefore, sodium oxide is neither an acid nor a base, in its solid form, but it forms a strong base when dissolved in water.
03
Identify Sulfuric Acid
(c) \( \mathrm{H}_{2}\mathrm{SO}_{4} \) is sulfuric acid, which is classified as a strong acid because it completely dissociates in water to release protons.
04
Identify Ammonia
(d) \( \mathrm{NH}_{3} \) is ammonia, considered a weak base because it partially accepts protons in water to form \( \mathrm{NH}_{4}^{+} \).
05
Identify Barium Hydroxide
(e) \( \mathrm{Ba(OH)}_{2} \) is barium hydroxide, known as a strong base because it dissociates completely in water to provide hydroxide ions.
06
Identify Dihydrogen Phosphate Ion
(f) \( \mathrm{H}_{2}\mathrm{PO}_{4}^{-} \) is dihydrogen phosphate, which is amphiprotic. It can act as an acid by donating a proton to become \( \mathrm{HPO}_{4}^{2-} \) or as a base by accepting a proton to become \( \mathrm{H}_{3}\mathrm{PO}_{4} \).
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
strong acids
Strong acids are substances that completely dissociate in water, donating their protons fully to create a solution of ions. A notable example is sulfuric acid \( \mathrm{H}_{2}\mathrm{SO}_{4} \). When sulfuric acid is added to water, it breaks apart almost entirely into hydrogen ions \( \mathrm{H}^{+} \) and sulfate ions \( \mathrm{SO}_{4}^{2-} \). This characteristic of complete dissociation is what makes sulfuric acid and similar substances strong acids.
- Properties: Strong acids have high conductivity due to free ions in solution.
- Applications: They're often used in laboratories and industries for reactions requiring a strong acidic environment.
- Examples Include: Hydrochloric acid \( \mathrm{HCl} \), nitric acid \( \mathrm{HNO}_{3} \), and perchloric acid \( \mathrm{HClO}_{4} \).
weak acids
Weak acids, unlike strong acids, do not completely dissociate in solution. A perfect illustration is acetic acid \( \mathrm{CH}_{3}\mathrm{COOH} \), which only partially ionizes when dissolved in water.
- As a result, weak acids have a higher concentration of nondissociated molecules and fewer free hydrogen ions.
- This leads to weaker acidic solutions compared to strong acids.
- Characteristics: They have lower electrical conductivity and react more slowly.
- Examples Include: Formic acid \( \mathrm{HCOOH} \), citric acid, and phosphoric acid \( \mathrm{H}_3\mathrm{PO}_4 \).
strong bases
Strong bases are characterized by their ability to fully dissociate in water to produce hydroxide ions \( \mathrm{OH}^{-} \). An example is barium hydroxide \( \mathrm{Ba(OH)}_{2} \), commonly known for releasing two moles of hydroxide ions per mole of base.
- This complete dissociation leads to highly conductive solutions, making strong bases efficient agents for neutralizing acids.
- Common Examples: Sodium hydroxide \( \mathrm{NaOH} \) and potassium hydroxide \( \mathrm{KOH} \) are frequently used in cleaning agents and chemical manufacturing.
- Care Required: Just like strong acids, strong bases must be handled with caution due to their corrosive properties and potential to cause burns.
weak bases
Weak bases are substances that do not completely accept protons in solution, resulting in only partial ionization. A common example is ammonia \( \mathrm{NH}_{3} \), which forms ammonium ions \( \mathrm{NH}_{4}^{+} \) when in water.
- Weak bases are characterized by their equilibrium between ionized and non-ionized molecules.
- This results in a less concentrated solution of hydroxide ions \( \mathrm{OH}^{-} \), thus they are less effective compared to strong bases.
- Examples: Ammonia is frequently used in household cleaning products for its mild basic properties.
- Applications: Agriculture benefits from weak bases in soil treatment to manage pH levels.
amphiprotic substances
Amphiprotic substances are unique in that they can either donate or accept a proton depending on the environment. A good example is the dihydrogen phosphate ion \( \mathrm{H}_{2}\mathrm{PO}_{4}^{-} \), which can act as an acid by donating a proton to form \( \mathrm{HPO}_{4}^{2-} \), or as a base by accepting a proton to become \( \mathrm{H}_{3}\mathrm{PO}_{4} \).
- Versatility: This dual ability makes amphiprotic substances flexible and essential in various natural processes, including buffer systems that maintain pH balance in blood and other fluids.
- Examples: Water is another classic amphiprotic substance, acting as either an acid or a base depending on the substances it interacts with.
- Relevance: Understanding amphiprotic substances helps in fields like biochemistry and environmental science, where controlling pH is crucial.
