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Chapter 4: Problem 60

(a) Name three common weak acids. (b) Name one common weak base. (c) What is the major difference between a weak acid and a strong acid or between a weak base and a strong base, and what experiment would you perform to observe it?

Short Answer

Expert verified
Common weak acids: acetic acid, citric acid, carbonic acid. Common weak base: ammonia. Difference: extent of dissociation. Experiment: conduct a conductivity test.

Step by step solution

01

Identify Common Weak Acids

Weak acids only partially dissociate in water. Three common weak acids are acetic acid (CH鈧僀OOH), citric acid (C鈧咹鈧圤鈧�), and carbonic acid (H鈧侰O鈧�).
02

Identify a Common Weak Base

Weak bases only partially dissociate in water. One common weak base is ammonia (NH鈧�).
03

Major Difference Between Weak vs. Strong Acids/Bases

The major difference is the extent of dissociation in water. Strong acids/bases completely dissociate, while weak acids/bases partially dissociate. For example, hydrochloric acid (HCl) is a strong acid, and sodium hydroxide (NaOH) is a strong base.
04

Experiment to Observe the Difference

Perform a conductivity test. Measure the electrical conductivity of solutions prepared with equal molar concentrations of a strong acid/base and a weak acid/base. Strong acids/bases will show higher conductivity due to complete dissociation, whereas weak acids/bases will show lower conductivity due to partial dissociation.

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Key Concepts

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

weak acid examples
Weak acids are acids that do not dissociate completely in water. Instead, only a small portion of the acid molecules ionize.
This partial dissociation means they release fewer hydrogen ions (H鈦�) compared to strong acids.
Here are three common examples of weak acids that you might see:

  • **Acetic acid (CH鈧僀OOH)**: Commonly found in vinegar. It gives vinegar its characteristic sour taste.
  • **Citric acid (C鈧咹鈧圤鈧�)**: Present in citrus fruits like lemons and oranges. Often used as a natural preservative and to add a sour flavor in foods and drinks.
  • **Carbonic acid (H鈧侰O鈧�)**: Formed when carbon dioxide (CO鈧�) is dissolved in water. It is present in carbonated beverages like soda.
Understanding weak acids helps in recognizing everyday substances we encounter.
weak base examples
Just like weak acids, weak bases do not fully dissociate in water. This results in a lower concentration of hydroxide ions (OH鈦�).
Instead, only a small number of base molecules ionize or react with water.
A common weak base example is:

  • **Ammonia (NH鈧�)**: Often used as a household cleaner. It has a distinctive pungent smell and is less corrosive than strong bases.
Understanding weak bases can help you grasp why some basic solutions are safer and less reactive than others.
dissociation in water
Dissociation in water is the process where acids and bases separate into ions when dissolved.
This process defines the strength of the acid or base.

  • **Strong acids/bases**: Completely dissociate in water, meaning they break apart fully into ions. For example, hydrochloric acid (HCl) dissociates into H鈦� and Cl鈦�, and sodium hydroxide (NaOH) dissociates into Na鈦� and OH鈦�.
  • **Weak acids/bases**: Only partially dissociate in water, meaning only some of the molecules break into ions while the rest stay intact. For instance, acetic acid (CH鈧僀OOH) dissociates slightly to form H鈦� and CH鈧僀OO鈦� ions.
The extent of dissociation affects many properties of the solution, such as pH and conductivity.
strong vs. weak acids and bases
The major difference between strong and weak acids and bases lies in their dissociation in water:

  • **Strong acids/bases:** These substances fully dissociate yielding a high concentration of ions. This complete dissociation makes them more reactive and more capable of conducting electricity.
  • **Weak acids/bases:** These only partially dissociate, resulting in fewer ions in solution. This partial dissociation means they are less reactive and less conductive compared to strong acids/bases.
The reactivity and conductivity of these acids and bases can be experimentally measured and observed.
conductivity test
Conductivity is a measure of a solution's ability to conduct electricity, which depends on the concentration of ions present.
It can be used to distinguish between strong and weak acids/bases:

  • **Experimental setup**: Prepare solutions of equal molar concentration for both a strong acid/base and a weak acid/base. Then, measure their electrical conductivity using a conductivity meter.
  • **Observations**: The strong acid/base solution will have higher conductivity due to a higher concentration of dissociated ions. Conversely, the weak acid/base solution will display lower conductivity because of fewer dissociated ions.
This experiment helps in understanding the practical implications of dissociation in different acidic and basic solutions.

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Most popular questions from this chapter

Water "softeners" remove metal ions such as \(\mathrm{Ca}^{2+}\) and \(\mathrm{Fe}^{3+}\) by replacing them with enough \(\mathrm{Na}^{+}\) ions to maintain the same number of positive charges in the solution. If \(1.0 \times 10^{3} \mathrm{~L}\) of "hard" water is \(0.015 \mathrm{M} \mathrm{Ca}^{2+}\) and \(0.0010 \mathrm{M} \mathrm{Fe}^{3+},\) how many moles of \(\mathrm{Na}^{+}\) are needed to replace these ions?

Describe how to determine the oxidation number of sulfur in (a) \(\mathrm{H}_{2} \mathrm{~S}\) and \((\mathrm{b}) \mathrm{SO}_{3}^{2-}\)

When each of the following pairs of aqueous solutions is mixed, does a precipitation reaction occur? If so, write balanced molecular, total ionic, and net ionic equations: (a) Sodium sulfide + nickel(II) sulfate (b) Lead(II) nitrate + potassium bromide

A sample of concentrated nitric acid has a density of \(1.41 \mathrm{~g} / \mathrm{mL}\) and contains \(70.0 \%\) HNO \(_{3}\) by mass. (a) What mass \((\mathrm{g})\) of \(\mathrm{HNO}_{3}\) is present per liter of solution? (b) What is the molarity of the solution?

Ammonia is produced by the millions of tons annually for use as a fertilizer. It is commonly made from \(\mathrm{N}_{2}\) and \(\mathrm{H}_{2}\) by the Haber process. Because the reaction reaches equilibrium before going completely to product, the stoichiometric amount of ammonia is not obtained. At a particular temperature and pressure, \(10.0 \mathrm{~g}\) of \(\mathrm{H}_{2}\) reacts with \(20.0 \mathrm{~g}\) of \(\mathrm{N}_{2}\) to form ammonia. When equilibrium is reached, \(15.0 \mathrm{~g}\) of \(\mathrm{NH}_{3}\) has formed. (a) Calculate the percent yield. (b) How many moles of \(\mathrm{N}_{2}\) and \(\mathrm{H}_{2}\) are present at equilibrium?
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