This worksheet will guide you through the process of naming acids and bases, a fundamental skill in chemistry. Understanding the nomenclature of these essential compounds is crucial for effective communication and comprehension in the field. We'll cover both common and systematic naming conventions, providing examples and practice problems to solidify your understanding.
Understanding Acids and Bases
Before diving into naming, let's briefly review the definitions of acids and bases. While several definitions exist (Arrhenius, Brønsted-Lowry, Lewis), we'll focus on the common characteristics relevant to naming:
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Acids: Acids typically donate a proton (H⁺) to a base in a chemical reaction. They often taste sour (though never taste chemicals!), react with metals to produce hydrogen gas, and turn blue litmus paper red. Many acids contain hydrogen (H) at the beginning of their chemical formula.
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Bases: Bases often accept a proton (H⁺) from an acid. They typically taste bitter and feel slippery. They turn red litmus paper blue. Many bases contain hydroxide ions (OH⁻).
Naming Acids
Acid nomenclature is largely dependent on the anion (negatively charged ion) present. Here's a breakdown:
Binary Acids (containing only hydrogen and one other nonmetal):
These acids are named using the prefix hydro- and the suffix -ic acid.
- Example: HCl (hydrochloric acid), HBr (hydrobromic acid), HI (hydroiodic acid)
Oxyacids (containing hydrogen, oxygen, and another nonmetal):
Oxyacids are named based on the oxyanion (anion containing oxygen). The rules are as follows:
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If the oxyanion ends in -ate, the acid name ends in -ic acid.
- Example: HNO₃ (nitric acid) from nitrate (NO₃⁻), H₂SO₄ (sulfuric acid) from sulfate (SO₄²⁻)
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If the oxyanion ends in -ite, the acid name ends in -ous acid.
- Example: HNO₂ (nitrous acid) from nitrite (NO₂⁻), H₂SO₃ (sulfurous acid) from sulfite (SO₃²⁻)
Naming Bases
Naming bases is generally simpler than naming acids. Many common bases are metal hydroxides. Their names consist of the name of the cation (positively charged ion) followed by "hydroxide."
- Examples: NaOH (sodium hydroxide), KOH (potassium hydroxide), Ca(OH)₂ (calcium hydroxide)
Worksheet: Naming Acids and Bases
Part 1: Name the following acids:
- HCl
- H₂SO₄
- HNO₃
- HBr
- H₂CO₃
- H₃PO₄
- HF
- HNO₂
- H₂SO₃
- HI
Part 2: Write the chemical formulas for the following acids:
- Hydrofluoric acid
- Nitric acid
- Sulfurous acid
- Hydrochloric acid
- Phosphoric acid
- Carbonic acid
- Hydrobromic acid
- Hypochlorous acid (Hint: Consider the hypochlorite ion)
- Perchloric acid (Hint: Consider the perchlorate ion)
- Acetic acid (Hint: This is an organic acid; its anion is acetate, CH₃COO⁻)
Part 3: Name the following bases:
- NaOH
- KOH
- Mg(OH)₂
- Ca(OH)₂
- LiOH
- Al(OH)₃
- Fe(OH)₂
- Fe(OH)₃
Part 4: Write the chemical formulas for the following bases:
- Barium hydroxide
- Strontium hydroxide
- Ammonium hydroxide (Hint: Ammonium is NH₄⁺)
- Potassium hydroxide
- Sodium hydroxide
- Calcium hydroxide
- Lithium hydroxide
Answer Key (provided separately upon request; encourage self-checking first!)
This worksheet provides a solid foundation for understanding acid and base nomenclature. Remember to practice regularly to master these naming conventions. Further exploration into polyprotic acids (acids that can donate more than one proton) and more complex oxyanions can enhance your chemical knowledge.
