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Chapter 8: Problem 44

What is the difference between a strong acid and a weak acid?

Short Answer

Expert verified
Answer: The main differences between strong and weak acids are their degree of ionization, ionization constants, pH values, and reactivity. Strong acids ionize completely, have higher ionization constants, lower pH values, and are more reactive, while weak acids ionize partially, have lower ionization constants, higher pH values, and are less reactive.

Step by step solution

01

Define Strong Acids and Weak Acids

Strong acids are acids that ionize completely in water, releasing all of their protons (H+ ions) into the solution. In other words, a strong acid will donate a proton to every water molecule it comes in contact with. Some examples of strong acids include hydrochloric acid (HCl), sulfuric acid (H2SO4), and nitric acid (HNO3). Weak acids, on the other hand, do not ionize completely in water and only release a small percentage of their protons. This means that weak acids only partially donate protons to water molecules. Examples of weak acids include acetic acid (CH3COOH), phosphoric acid (H3PO4), and carbonic acid (H2CO3).
02

Compare the Ionization Constants

The degree of ionization of an acid can be assessed by examining its ionization constant (Ka). Strong acids have a higher Ka value, indicating that they are better proton donors and ionize more completely in water. Weak acids have a lower Ka value, meaning they are less successful at donating protons and have a lower degree of ionization.
03

Compare the pH Values

The pH of a solution is a measure of the concentration of H+ ions in the solution. Since strong acids ionize completely and release all of their protons, the pH value of a solution containing a strong acid will be lower (more acidic) than that of a solution containing a weak acid. A low pH value (< 7) indicates a high concentration of H+ ions, while a higher pH value (> 7) indicates a lower concentration.
04

Reactivity of Acids

Strong acids are more reactive than weak acids due to higher concentrations of H+ ions they release into the solution. They react more vigorously with other substances than weak acids and are more aggressive in their corrosive nature. In summary, the main differences between strong and weak acids lie in their degree of ionization, ionization constants, pH values, and reactivity. While strong acids ionize completely and have low pH values with higher reactivity, weak acids only ionize partially, with higher pH values and lower reactivity.

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Most popular questions from this chapter

According to the label on a bottle of concentrated hydrochloric acid, the contents are \(36.0 \%\) HCl by mass and have a density of \(1.18 \mathrm{g} / \mathrm{mL}\) a. What is the molarity of this concentrated HCl? b. What volume of it would you need to prepare \(0.250 \mathrm{L}\) of \(2.00 \mathrm{MHCl} ?\) c. What mass of sodium hydrogen carbonate would be needed to neutralize the spill if a bottle containing 1.75 L of this concentrated HCl dropped on a lab floor and broke open?

Give the formulas of two strong bases and two weak bases.

Why is the oxidizing agent in a redox reaction reduced and the reducing agent oxidized?

A prototype battery based on iron compounds with large, positive oxidation numbers was developed in \(1999 .\) In the following reactions, assign oxidation numbers to the clements in each compound and balance the redox reactions in basic solution: a. \(\mathrm{FeO}_{4}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{FeOOH}(s)+\mathrm{O}_{2}(g)+\mathrm{OH}^{-}(a q)\) b. \(\mathrm{FeO}_{4}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{O}_{2}(g)+\mathrm{OH}^{-}(a q)\)

Iron is oxidized in a number of chemical weathering processes. How many moles of \(\mathrm{O}_{2}\) are consumed when one mole of magnetite (Fe \(_{3} \mathrm{O}_{4}\) ) is converted into hematite \(\left(\mathrm{Fe}_{2} \mathrm{O}_{3}\right) ?\)
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