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Chapter 2: Problem 75

Give the name or chemical formula, as appropriate, for each of the following acids: (a) \(\mathrm{HBrO}_{3}\), (b) \(\mathrm{HBr}\), (c) \(\mathrm{H}_{3} \mathrm{PO}_{4}\), (d) hypochlorous acid, (e) iodic acid, (f) sulfurous acid.

Short Answer

Expert verified
(a) Bromic acid, (b) Hydrobromic acid, (c) Phosphoric acid, (d) \(HClO\), (e) \(HIO_3\), (f) \(H_2SO_3\).

Step by step solution

01

Identify and name HBrO3

The given chemical formula is HBrO3. We can tell it's an acid because the hydrogen (H) is in front. Since it has bromine (Br) and oxygen (O), it鈥檚 a type of oxyacid. The general rule for naming oxyacids is this: 1. If the anion has one more oxygen than the "-ate" ion, then the acid will have the prefix "per-" and the suffix "-ic." 2. If the anion has the same number of oxygens as the "-ate" ion, the acid name will have the suffix "-ic." 3. If the anion has one less oxygen than the "-ite" ion, the acid name will have the suffix "-ous." 4. If the anion has the same number of oxygens as the "-ite" ion, then the acid name will have the prefix "hypo-" and the suffix "-ous." In this case, we have the bromate ion (from BrO3) and 1 hydrogen atom. The name for this acid is bromic acid.
02

Identify and name HBr

The given chemical formula is HBr. We have a hydrogen atom and a bromine atom here, and they form a binary acid. Binary acids are named based on the halogen they contain, followed by the suffix "-ic." In this case, we have hydrogen bromide, which is referred to as hydrobromic acid.
03

Identify and name H3PO4

The given chemical formula is H3PO4. We have a phosphate ion (from PO4) and 3 hydrogen atoms. Since this is an oxyacid, we will follow the naming rules for oxyacids mentioned in step 1. The name for this acid is phosphoric acid.
04

Identify the chemical formula for hypochlorous acid

We are given the name "hypochlorous acid." Based on our naming rules for oxyacids, we know hypochlorous acid has the prefix "hypo-" and the suffix "-ous," which means it contains the same number of oxygens as the "-ite" ion. In this case, the "-ite" ion of chlorine is chlorite (ClO2). Since hypochlorous acid has the same number of oxygens as the chlorite ion, its chemical formula is HClO.
05

Identify the chemical formula for iodic acid

We are given the name "iodic acid." Since it's an oxyacid, we will follow the naming rules for oxyacids mentioned in step 1. Iodic acid has the suffix "-ic," which means it has the same number of oxygens as the "-ate" ion. In this case, the "-ate" ion of iodine is iodate (IO3). So, the chemical formula for iodic acid is HIO3.
06

Identify the chemical formula for sulfurous acid

We are given the name "sulfurous acid." Since it's an oxyacid, we will follow the naming rules for oxyacids mentioned in step 1. Sulfurous acid has the suffix "-ous," which means it has one less oxygen than the "-ite" ion. In this case, the "-ite" ion of sulfur is sulfite (SO3). So, the chemical formula for sulfurous acid is H2SO3. To summarize, here are the names or chemical formulas for each acid: a) HBrO3 - Bromic acid b) HBr - Hydrobromic acid c) H3PO4 - Phosphoric acid d) Hypochlorous acid - HClO e) Iodic acid - HIO3 f) Sulfurous acid - H2SO3

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Key Concepts

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

Oxyacids
Oxyacids are a type of acid that contains hydrogen, oxygen, and another element, which is often a non-metal. What distinguishes oxyacids from other acids is the presence of oxygen in their chemical composition. Understanding oxyacids is key to naming or writing their formulas correctly.
The typical method of naming oxyacids revolves around the associated polyatomic ion. For example, in the case of phosphoric acid, the relevant ion is phosphate. There are a few key rules to help remember:
  • When the polyatomic ion ends in "-ate," the corresponding acid name ends in "-ic." Thus, phosphate (PO鈧勨伝鲁) becomes phosphoric acid (H鈧働O鈧�).
  • If the ion ends in "-ite," the acid name becomes "-ous." The sulfite ion (SO鈧冣伝虏) becomes sulfurous acid (H鈧係O鈧�).
  • The prefixes "per-" and "hypo-" may also be used if the polyatomic ion has variations with more or fewer oxygen atoms.
Memorizing the names of common ions and understanding these rules will help in swiftly identifying and naming oxyacids.
Binary Acids
Binary acids consist of only two elements. In the chemical formula of a binary acid, hydrogen is always the first element, followed by a non-metal.
A few key features of binary acids include:
  • They are typically gases and only exhibit acidic properties when dissolved in water.
  • Common examples include hydrochloric acid (HCl) and hydrobromic acid (HBr).
The naming involves the following steps:
  • Add the prefix "hydro-" to the root name of the non-metal element.
  • Subtract the suffix "-ide" from the non-metal and replace it with "-ic."
  • Finish by adding the word "acid."
For instance, HBr becomes hydrobromic acid, as it consists of hydrogen and bromine. This method ensures consistency in naming across various binary acids.
Chemical Formulas
Chemical formulas act as a shorthand to represent molecules and compounds using element symbols and numerical subscripts to show the number of each atom present. Understanding how to write and interpret these formulas is crucial for chemistry students.
Key aspects of chemical formulas include:
  • For acids like HClO, the formula represents one atom of hydrogen, one atom of chlorine, and one atom of oxygen.
  • Polyatomic ions such as sulfate (SO鈧�) or nitrate (NO鈧�) require knowledge of their composition to correctly write the formulas of their acids, like sulfuric acid (H鈧係O鈧�).
  • Binary acids use the formula H + base element, like hydrogen chloride (HCl).
Seeing these formulas repeatedly and practicing writing them can help students associate chemical names with their correct formulas, thereby easing their work with acids.
Naming Rules for Acids
Naming acids can be tricky, but by learning specific rules, the process becomes more manageable. There are multiple naming rules depending on the type of acid you're dealing with.
For oxyacids:
  • If the acid is derived from an "-ate" anion, the acid name ends in "-ic" (e.g., nitrate to nitric acid).
  • If derived from an "-ite" anion, the name ends with "-ous" (e.g., sulfite to sulfurous acid).
  • Prefixes like "per-" or "hypo-" indicate the number of oxygen atoms relative to the standard "-ate" ion.
For binary acids:
  • The name starts with "hydro-" and ends with "-ic."
  • Only the non-metal element changes from "-ide" to "-ic."
By consistently applying these naming conventions, students can confidently name acids in various chemical contexts, ensuring clear communication of chemical information.

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Most popular questions from this chapter

Name each of the following oxides. Assuming that the compounds are ionic, what charge is associated with the metallic element in each case? (a) \(\mathrm{NiO}\), (b) \(\mathrm{MnO}_{2}\), (c) \(\mathrm{Cr}_{2} \mathrm{O}_{3}\), (d) \(\mathrm{MoO}_{3}\).

The first atoms of seaborgium (Sg) were identified in 1974 . The longest-lived isotope of Sg has a mass number of 266 . (a) How many protons, electrons, and neutrons are in an \({ }^{266} \mathrm{Sg}\) atom? (b) Atoms of \(\mathrm{Sg}\) are very unstable, and it is therefore difficult to study this element's properties. Based on the position of \(\mathrm{Sg}\) in the periodic table, what element should it most closely resemble in its chemical properties?

Mass spectrometry is more often applied to molecules than to atoms. We will see in Chapter 3 that the molecular weight of a molecule is the sum of the atomic weights of the atoms in the molecule. The mass spectrum of \(\mathrm{H}_{2}\) is taken under conditions that prevent decomposition into \(\mathrm{H}\) atoms. The two naturally occurring isotopes of hydrogen are \({ }^{1} \mathrm{H}\) (atomic mass \(=1.00783 \mathrm{amu}\) abundance \(99.9885 \%\) ) and \({ }^{2} \mathrm{H}\) (atomic mass \(=2.01410 \mathrm{amu}\) abundance \(0.0115 \%\) ). (a) How many peaks will the mass spectrum have? (b) Give the relative atomic masses of each of these peaks. (c) Which peak will be the largest, and which the smallest?

The explosion of an atomic bomb releases many radioactive isotopes, including strontium- 90 . Considering the location of strontium in the periodic table, suggest a reason for the fact that this isotope is particularly dangerous for human health.

(a) Assuming the dimensions of the nucleus and atom shown in Figure 2.11, what fraction of the volume of the atom is taken up by the nucleus? (b) Using the mass of the proton from Table \(2.1\) and assuming its diameter is \(1.0 \times 10^{-15} \mathrm{~m}\), calculate the density of a proton in \(\mathrm{g} / \mathrm{cm}^{3}\).
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