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Chapter 6: Problem 41

Make a list of the common strong acids and strong bases. Memorize this list.

Short Answer

Expert verified
Memorize common strong acids: HCl, HBr, HI, HNO3, H2SO4, HClO4 and strong bases: NaOH, KOH, LiOH, Ca(OH)2, Ba(OH)2, Sr(OH)2.

Step by step solution

01

Understanding Strong Acids

Strong acids are those that completely dissociate in water, meaning they release all their hydrogen ions into the solution. You should familiarize yourself with the common strong acids and their chemical formulas, so you can easily recognize them.
02

List of Strong Acids

The common strong acids to remember are:1. Hydrochloric acid (\( ext{HCl} \))2. Hydrobromic acid (\( ext{HBr} \))3. Hydroiodic acid (\( ext{HI} \))4. Nitric acid (\( ext{HNO}_3 \))5. Sulfuric acid (\( ext{H}_2 ext{SO}_4 \))6. Perchloric acid (\( ext{HClO}_4 \))
03

Understanding Strong Bases

Strong bases are substances that completely dissociate in water to release hydroxide ions (\( ext{OH}^- \)). Like strong acids, strong bases are fully ionized in solution.
04

List of Strong Bases

The common strong bases to memorize are:1. Sodium hydroxide (\( ext{NaOH} \))2. Potassium hydroxide (\( ext{KOH} \))3. Lithium hydroxide (\( ext{LiOH} \))4. Calcium hydroxide (\( ext{Ca(OH)}_2 \))5. Barium hydroxide (\( ext{Ba(OH)}_2 \))6. Strontium hydroxide (\( ext{Sr(OH)}_2 \))

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Key Concepts

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

Chemical Dissociation
Chemical dissociation is a process by which a compound breaks down into its component ions when dissolved in water. Understanding this is key when learning about strong acids and bases.

In the case of strong acids and bases, this dissociation is complete, meaning all molecules of the compound release their ions into the solution.

For instance,
  • Strong acids release hydrogen ions ( H^+) in water.
  • Strong bases release hydroxide ions ( OH^- ) in water.
This complete ionization results in a highly conductive solution due to the abundance of charged particles.

The degree of dissociation is a significant distinction between strong and weak acids or bases. Strong ones dissociate fully, while weak ones only partially dissociate in solution.
Hydrochloric Acid
Hydrochloric acid, also known by its chemical formula HCl , is one of the most commonly encountered strong acids.

It fully dissociates in water to release hydrogen ions ( H^+ ) and chloride ions ( Cl^- ), making it a potent acid.

  • It is widely used in industrial applications, such as refining metals and making organic compounds.
  • In laboratories, it is used to adjust pH and prepare chloride salts.

Due to its high reactivity, special caution is needed when handling hydrochloric acid. Protective gear is generally recommended to prevent skin contact or inhalation, as it can be quite corrosive.
Sodium Hydroxide
Sodium hydroxide, symbolized as NaOH , is a well-known strong base. When NaOH is dissolved in water, it completely dissociates into sodium ions ( Na^+ ) and hydroxide ions ( OH^- ).

This makes it extremely effective at increasing the pH of a solution, making it highly alkaline.
  • Sodium hydroxide is used in various manufacturing processes, such as paper production and soap making.
  • It is also used in cleaning agents due to its ability to dissolve grease and oils.
It's important to note that sodium hydroxide is caustic, so handling it with care and using protective equipment is essential to avoid burns.

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Most popular questions from this chapter

If a solution containing \(0.10 \mathrm{M} \mathrm{Cl}^{-}, \mathrm{Br}^{-}, \mathrm{I}^{-}\), and \(\mathrm{CrO}_{4}^{2-}\) is treated with \(\mathrm{Ag}^{+}\), in what order will the anions precipitate?

Write the \(K_{\mathrm{a}}\) reaction for trichloroacetic acid, \(\mathrm{Cl}_{3} \mathrm{CCO}_{2} \mathrm{H}\), for \(\left\langle\bigcirc-\mathrm{NH}_{3}\right.\), and for lanthanum ion, \(\mathrm{La}^{3+} .\)

Identify the Br酶nsted-Lowry acids among the reactants in the following reactions: (a) \(\mathrm{KCN}+\mathrm{HI} \rightleftharpoons \mathrm{HCN}+\mathrm{KI}\) (b) \(\mathrm{PO}_{4}^{3-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{HPO}_{4}^{2-}+\mathrm{OH}^{-}\)

Calculate \(\left[\mathrm{H}^{+}\right]\)and \(\mathrm{pH}\) for the following solutions: (a) \(0.010 \mathrm{M} \mathrm{HNO}_{3}\) (d) \(3.0 \mathrm{MHCl}\) (b) \(0.035 \mathrm{M} \mathrm{KOH}\) (e) \(0.010 \mathrm{M}\left[\left(\mathrm{CH}_{3}\right)_{4} \mathrm{~N}^{+}\right] \mathrm{OH}^{-}\) (c) \(0.030 \mathrm{M} \mathrm{HCl}\) Tetramethylammonium hydroxide

Find \(\left[\mathrm{Cu}^{2+}\right]\) in a solution saturated with \(\mathrm{Cu}_{4}(\mathrm{OH})_{6}\left(\mathrm{SO}_{4}\right)\) if \(\left[\mathrm{OH}^{-}\right]\)is fuxed at \(1.0 \times 10^{-6} \mathrm{M}\). Note that \(\mathrm{Cu}_{4}(\mathrm{OH})_{6}\left(\mathrm{SO}_{4}\right)\) gives \(1 \mathrm{~mol}\) of \(\mathrm{SO}_{4}^{2-}\) for \(4 \mathrm{~mol}\) of \(\mathrm{Cu}^{2+}\). $$ \begin{aligned} \mathrm{Cu}_{4}(\mathrm{OH})_{6}\left(\mathrm{SO}_{4}\right)(s) \rightleftharpoons 4 \mathrm{Cu}^{2+}+6 \mathrm{OH}^{-}+\mathrm{SO}_{4}^{2-} \\\ K_{\mathrm{sp}}=2.3 \times 10^{-69} \end{aligned} $$
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