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Chapter 7: Problem 14

Name each of the following acids: a) \({HF}\) d) \({H}_{2} {SO}_{4}\) b) \({HBr}\) e) \({H}_{3} {PO}_{4}\) c) \({HNO}_{3}\)

Short Answer

Expert verified
a) Hydrofluoric acid, b) Hydrobromic acid, c) Nitric acid, d) Sulfuric acid, e) Phosphoric acid

Step by step solution

01

- Identify Binary Acids

Binary acids consist of hydrogen and one other element. For binary acids, the naming convention is 'hydro-' followed by the root name of the element and ending with '-ic acid.'
02

- Name {HF}

Since {HF} is a binary acid, it is named hydrofluoric acid.
03

- Name {HBr}

Similar to {HF}, {HBr} is a binary acid and is named hydrobromic acid.
04

- Identify Oxyacids

Oxyacids contain hydrogen, oxygen, and another element. The naming convention depends on the polyatomic ion it contains. If the polyatomic ion ends in '-ate,' the acid name will end with '-ic acid.' If it ends in '-ite,' the acid name will end with '-ous acid.'
05

- Name {HNO}_{3}

{HNO}_{3} contains the nitrate ion (NO_{3}^{-}), so it is named nitric acid.
06

- Name {H}_{2}SO_{4}

{H}_{2}SO_{4} contains the sulfate ion (SO_{4}^{2-}), so it is named sulfuric acid.
07

- Name {H}_{3}PO_{4}

{H}_{3}PO_{4} contains the phosphate ion (PO_{4}^{3-}), so it is named phosphoric acid.

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Key Concepts

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

Binary Acids
Binary acids are simple compounds consisting of hydrogen and one other nonmetal element. These are easy to identify because they don't contain oxygen. When naming binary acids, the process is straightforward. You'll use the prefix 'hydro-', followed by the root of the nonmetal element's name, and end with '-ic acid.' For example, in the exercise:
  • HF becomes hydrofluoric acid.
  • HBr becomes hydrobromic acid.
Binary acids are typically found in aqueous solutions, and they are known for their ability to donate protons (H+ ions) when dissolved in water.
Oxyacids
Oxyacids are more complex than binary acids as they consist of hydrogen, oxygen, and another nonmetal element. The naming of oxyacids depends on the polyatomic ion present within the compound. Here's how you name them:
  • If the polyatomic ion ends in '-ate,' the acid name changes to end in '-ic acid.'
  • If the polyatomic ion ends in '-ite,' the acid name changes to end in '-ous acid.'
For example, the solution provided includes:
  • HNO3, which contains the nitrate (NO3-) ion, becomes nitric acid.
Similarly,
  • H2SO4 with the sulfate (SO42-) ion becomes sulfuric acid.
  • H3PO4 containing the phosphate (PO43-) ion is named phosphoric acid.
Knowing the rules for these names can greatly simplify your study of chemistry and make it easier to recognize these compounds.
Chemical Nomenclature
Chemical nomenclature is the system used for naming chemical compounds. Its main goal is to provide clear and consistent naming to avoid confusion. There are various types of chemical compounds, and each has its own rules for naming:
  • Binary compounds: Two elements, often a metal and a non-metal.
  • Binary acids: 'Hydro-' prefix, nonmetal root name, and '-ic acid' suffix.
  • Oxyacids: Name based on the polyatomic ions they contain, changing '-ate' to '-ic acid' and '-ite' to '-ous acid.'
Chemical nomenclature extends beyond acids to include ionic compounds, molecular compounds, and coordination complexes. Mastering nomenclature is crucial for understanding and communicating chemical information effectively.
Polyatomic Ions
Polyatomic ions are charged species composed of two or more atoms covalently bonded, that act as a single unit. They play a key role in the formation of oxyacids. Examples include nitrate (NO3-), sulfate (SO42-), and phosphate (PO43-). Naming compounds with polyatomic ions follows specific rules. For oxyacids:
  • If the polyatomic ion ends in '-ate,' the acid name ends in '-ic acid.'
  • If it ends in '-ite,' the acid name ends in '-ous acid.'
More generally, these ions influence the properties and reactivities of the compounds they form. Understanding these ions is crucial for predicting the behavior of acids and other complex compounds in chemical reactions.

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