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Chapter 14: Problem 6

Write formulas for each of the following acids and bases: a. barium hydroxide b. hydroiodic acid c. nitric acid d. strontium hydroxide e. acetic acid if. hypochlorous acid

Short Answer

Expert verified
a. Ba(OH)鈧�, b. HI, c. HNO鈧�, d. Sr(OH)鈧�, e. CH鈧僀OOH, f. HClO

Step by step solution

01

Identify the formula for barium hydroxide

Barium hydroxide consists of barium (Ba) and hydroxide (OH). Barium has a charge of +2 and hydroxide has a charge of -1. Therefore, the formula is Ba(OH)鈧�.
02

Identify the formula for hydroiodic acid

Hydroiodic acid is composed of hydrogen (H) and iodine (I), and contains Iodine as the halogen. The formula is HI.
03

Identify the formula for nitric acid

Nitric acid is a combination of hydrogen (H), nitrogen (N), and oxygen (O). The nitrate ion has the formula NO鈧冣伝. Combining this with a hydrogen ion results in the formula HNO鈧�.
04

Identify the formula for strontium hydroxide

Strontium hydroxide consists of strontium (Sr) and hydroxide (OH). Strontium has a charge of +2 and hydroxide has a charge of -1. Therefore, the formula is Sr(OH)鈧�.
05

Identify the formula for acetic acid

Acetic acid is made up of hydrogen (H), carbon (C), and oxygen (O). The molecular formula for acetic acid is CH鈧僀OOH.
06

Identify the formula for hypochlorous acid

Hypochlorous acid is composed of hydrogen (H), chlorine (Cl), and oxygen (O). The molecular formula for hypochlorous acid is HClO.

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Key Concepts

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

acid-base chemistry
Understanding acid-base chemistry is essential for this exercise. Acids are compounds that release hydrogen ions (H鈦�) when dissolved in water. Bases, on the other hand, release hydroxide ions (OH鈦�). An easy way to remember is:
* Acids have an H at the beginning (e.g., HCl).
* Bases often have OH at the end (e.g., NaOH).
Reactions between acids and bases often result in the formation of water and a salt, a process called neutralization. Keep in mind the strength of acids and bases differs; strong acids/bases dissociate completely in water, while weak ones do not.
nomenclature of compounds
The nomenclature of chemical compounds is a system used to name them. For acids and bases, understanding the naming conventions is crucial.
  • **Binary acids**: Contain hydrogen and one other element. Named by using 'hydro-', the root of the nonmetal name, and '-ic acid' (e.g., HI is hydroiodic acid).
  • **Oxyacids**: Contain hydrogen, oxygen, and another element. Named based on the central atom and its oxidation state (e.g., HNO鈧� is nitric acid).
  • **Bases**: Usually consist of a metal cation and hydroxide. Named like other ionic compounds, with the metal first and 'hydroxide' last (e.g., Ba(OH)鈧� is barium hydroxide).
Get familiar with these rules to make writing chemical formulas easier.
chemical bonding
Chemical bonding teaches us how atoms stick together to form compounds. There are two main types: ionic and covalent bonds.
  • **Ionic bonds**: Formed between metals and nonmetals, where electrons are transferred from one atom to another. For instance, barium hydroxide (Ba(OH)鈧�) involves ionic bonds between Ba虏鈦� and OH鈦� ions.
  • **Covalent bonds**: Formed when atoms share electrons. Acetic acid (CH鈧僀OOH) is an example where C, H, and O atoms are bonded covalently.
Recognizing the type of bond can help predict the behavior and properties of the compound.
molecular structure
The molecular structure of a compound gives insight into its properties and reactivity. This concept involves understanding the 3D arrangement of atoms. For acids and bases we wrote:
  • **Ba(OH)鈧� (Barium hydroxide)**: Two OH groups bonded to a central Ba atom.
  • **HI (Hydroiodic acid)**: Simple diatomic molecule with an H-I bond.
  • **HNO鈧� (Nitric acid)**: Central N atom bonded to three O atoms with one O also bonded to H.
  • **Sr(OH)鈧� (Strontium hydroxide)**: Two OH groups bonded to a central Sr atom.
  • **CH鈧僀OOH (Acetic acid)**: Carboxyl group (COOH) bonded to a methyl group (CH鈧�).
  • **HClO (Hypochlorous acid)**: Central Cl atom bonded to O and H atoms.
Understanding these structures helps in visualizing how compounds interact in chemical reactions.

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Most popular questions from this chapter

Balance each of the following neutralization reactions: a. \(\mathrm{HNO}_{3}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(s) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)\)

Solution \(\mathrm{A}\) has a \(\mathrm{pH}\) of \(4.5\), and solution \(\mathrm{B}\) has a \(\mathrm{pH}\) of \(6.7\). (14.6) a. Which solution is more acidic? b. What is the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in each? c. What is the [OH \(]\) in each?

What is the \(\mathrm{pH}\) and \(\mathrm{pOH}\) of a solution prepared by dissolving \(1.0 \mathrm{~g}\) of \(\mathrm{Ca}(\mathrm{OH})_{2}\) in water to make \(875 \mathrm{~mL}\) of solution? \((14.6)\)

A buffer solution is made by dissolving \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) and \(\mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) in water. (14.9) a. Write an equation that shows how this buffer neutralizes added acid. b. Write an equation that shows how this buffer neutralizes added base. c. Calculate the \(\mathrm{pH}\) of this buffer if it contains \(0.20 \mathrm{M} \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) and \(0.40 \mathrm{M} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\). The \(K_{\mathrm{a}}\) for \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) is \(1.8 \times 10^{-5}\)

Write the formula for the conjugate base for each of the following acids: a. \(\mathrm{HCO}_{3}^{-}\) b. \(\mathrm{CH}_{3}-\mathrm{NH}_{3}^{+}\) c. \(\mathrm{HPO}_{4}^{2-}\) d. \(\mathrm{HNO}_{2}\) e. \(\mathrm{HBrO}\)
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