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Chapter 4: Problem 36

Classify each of the following as a strong or weak acid or base. a. \(\mathrm{NH}_{3}\) b. HCNO c. \(\mathrm{Sr}(\mathrm{OH})_{2}\) d. HI

Short Answer

Expert verified
a. Weak base; b. Weak acid; c. Strong base; d. Strong acid.

Step by step solution

01

Understanding Acid and Base Classification

Acids and bases can be classified as strong or weak based on their ability to dissociate completely in water. Strong acids and bases dissociate completely, whereas weak acids and bases do not. Understanding these dissociation properties is key to classification.
02

Classifying Ammonia (NH3)

Ammonia, \( ext{NH}_3\), is a base. It is known for its incomplete dissociation in aqueous solutions, meaning it does not ionize completely to form \( ext{NH}_4^+ \) and \( ext{OH}^- \). Therefore, it is classified as a weak base.
03

Classifying Isocyanic Acid (HCNO)

HCNO, or isocyanic acid, is a lesser-known acid that partially dissociates in solution. Its incomplete dissociation mechanism makes it a weak acid.
04

Classifying Strontium Hydroxide (Sr(OH)2)

Strontium hydroxide, \( ext{Sr(OH)}_2 \), dissociates completely in water to produce \( ext{Sr}^{2+} \) and \( 2 ext{OH}^- \). It is a strong base, similar to other soluble hydroxides of Group 2 elements.
05

Classifying Hydroiodic Acid (HI)

Hydroiodic acid, \( ext{HI} \), is known to dissociate completely in water to form hydrogen ions and iodide ions. Its full dissociation characterizes it as a strong acid.

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Key Concepts

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

Strong Acid
A strong acid is one that dissociates completely in water, releasing all of its hydrogen ions into the solution. This complete dissociation results in a high concentration of hydrogen ions, making the solution highly acidic.
One key example of a strong acid is hydroiodic acid (HI). In water, HI separates entirely into hydrogen ions (H\(^+\)) and iodide ions (I\(^-\)). This complete ionization is why HI is considered a strong acid.
  • Strong acids have low pH values, typically less than 3.
  • They are strong electrolytes, meaning they conduct electricity well in solution.
  • Common strong acids include hydrochloric acid (HCl), sulfuric acid (H\(_2\)SO\(_4\)), and nitric acid (HNO\(_3\)).
Understanding the behavior of strong acids is essential for various applications, from chemistry labs to industrial processes.
Weak Acid
Unlike strong acids, weak acids do not completely dissociate in water. This means they release fewer hydrogen ions into the solution.
Isocyanic acid (HCNO) is an example of a weak acid. In solution, it only partially dissociates into hydrogen ions and cyanate ions (CNO\(^-\)), meaning not all its molecules ionize.
  • Weak acids have higher pH values compared to strong acids, usually ranging between 3 and 7.
  • They are weak electrolytes, indicating that they do not conduct electricity as well.
  • Examples of weak acids include acetic acid (CH\(_3\)COOH) and formic acid (HCOOH).
Understanding weak acids is important in buffering solutions and biochemical processes.
Strong Base
Strong bases, like strong acids, dissociate completely in water, releasing all available hydroxide ions (OH\(^-\)).
Strontium hydroxide (Sr(OH)\(_2\)) is a good example of a strong base. It fully separates into strontium ions (Sr\(^{2+}\)) and hydroxide ions in aqueous solutions.
  • Strong bases have high pH values, generally greater than 10.
  • They are strong electrolytes, making them excellent conductors of electricity.
  • Other examples of strong bases include sodium hydroxide (NaOH) and potassium hydroxide (KOH).
Strong bases are crucial in neutralizing acids and in various industrial applications.
Weak Base
Weak bases only partially ionize in solution, meaning they do not produce many hydroxide ions.
Ammonia (NH\(_3\)) is a classic example. While it can accept a hydrogen ion from water, forming ammonium (NH\(_4^+\)) and hydroxide ions, it does so only to a small extent.
  • Weak bases typically have pH values between 7 and 10.
  • They are weak electrolytes, with lower conductivity than strong bases.
  • Other examples include methylamine (CH\(_3\)NH\(_2\)) and pyridine (C\(_5\)H\(_5\)N).
Weak bases are vital in biological systems and various chemical reactions.

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Most popular questions from this chapter

An aqueous solution contains \(4.00 \% \mathrm{NH}_{3}\) (ammonia) by mass. The density of the aqueous ammonia is \(0.979 \mathrm{~g} / \mathrm{mL}\). What is the molarity of \(\mathrm{NH}_{3}\) in the solution?

Barium carbonate is the source of barium compounds. It is produced in an aqueous precipitation reaction from barium sulfide and sodium carbonate. (Barium sulfide is a soluble compound obtained by heating the mineral barite, which is barium sulfate, with carbon.) What are the molecular equation and net ionic equation for the precipitation reaction? A solution containing \(33.9 \mathrm{~g}\) of barium sulfide requires \(21.2 \mathrm{~g}\) of sodium carbonate to react completely with it, and \(15.6 \mathrm{~g}\) of sodium sulfide is produced in addition to whatever barium carbonate is obtained. How many grams of barium sulfide are required to produce \(10.0\) tons of barium carbonate? (One ton equals 2000 pounds.)

The active ingredients of an antacid tablet contained only magnesium hydroxide and aluminum hydroxide. Complete neutralization of a sample of the active ingredients required \(48.5 \mathrm{~mL}\) of \(0.187 \mathrm{M}\) hydrochloric acid. The chloride salts from this neutralization were obtained by evaporation of the filtrate from the titration; they weighed \(0.4200 \mathrm{~g}\). What was the percentage by mass of magnesium hydroxide in the active ingredients of the antacid tablet?

A \(0.608-\mathrm{g}\) sample of fertilizer contained nitrogen as \end{tabular} ammonium sulfate, \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\). It was analyzed for nitrogen by heating with sodium hydroxide. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(s)+2 \mathrm{NaOH}(a q) \longrightarrow\) $$ \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{NH}_{3}(g) $$ The ammonia was collected in \(46.3 \mathrm{~mL}\) of \(0.213 \mathrm{M} \mathrm{HCl}\) (hydrochloric acid), with which it reacted. $$ \mathrm{NH}_{3}(g)+\mathrm{HCl}(a q) \longrightarrow \mathrm{NH}_{4} \mathrm{Cl}(a q) $$ This solution was titrated for excess hydrochloric acid with \(44.3 \mathrm{~mL}\) of \(0.128 \mathrm{M} \mathrm{NaOH}\). $$ \mathrm{NaOH}(a q)+\mathrm{HCl}(a q) \longrightarrow \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l) $$ What is the percentage of nitrogen in the fertilizer?

A solution of scandium chloride was treated with silver nitrate. The chlorine in the scandium compound was converted to silver chloride, AgCl. A \(58.9\) -mg sample of scandium chloride gave \(167.4 \mathrm{mg}\) of silver chloride. What are the mass percentages of \(\mathrm{Sc}\) and \(\mathrm{Cl}\) in scandium chloride? What is its empirical formula?
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