Chemistry Chapter 13: Acids and Bases
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Questions and Answers

What characterizes a strong acid?

  • Partially dissociates in solution
  • Increases the pH of the solution
  • Releases fewer hydrogen ions than weak acids
  • Completely dissociates in solution (correct)

    • Which of the following correctly describes a base?

  • Accepts protons from acids (correct)
  • Releases hydroxide ions in solution (correct)
  • Donates electrons to acids
  • Increases the concentration of hydronium ions

    • What is the primary role of sodium bicarbonate (NaHCO₃) in antacid action?

  • It neutralizes excess stomach acid (correct)
  • It acts as a catalyst for acid reactions
  • It lowers the pH of the stomach contents
  • It increases acidity in the digestive tract

    • Which statement about acid-base reactions is true?

    <p>They always produce water and salts</p> Signup and view all the answers

    What impact does acid rain have on the environment?

    <p>It can damage aquatic ecosystems</p> Signup and view all the answers

    Which of these statements about pH and acidity is correct?

    <p>A solution with pH = 2 has a higher concentration of H3O+ than one with pH = 3.</p> Signup and view all the answers

    Which acid is primarily responsible for the sour taste in vinegar?

    <p>Acetic acid</p> Signup and view all the answers

    Which of these acids is commonly not found in wines?

    <p>Salicylic acid</p> Signup and view all the answers

    Which property is characteristic of acids?

    <p>They taste sour.</p> Signup and view all the answers

    Which of the following substances would exhibit the highest acidity?

    <p>1.0 M HNO3</p> Signup and view all the answers

    Which substance is classified as a base?

    <p>NaOH</p> Signup and view all the answers

    Which equation best describes the dissociation of magnesium hydroxide in water?

    <p>Mg(OH)2 = Mg2+ + 2OH−</p> Signup and view all the answers

    In the chemical reaction HSO4− + OH− → SO42− + H2O, which species acts as a Bronsted-Lowry base?

    <p>OH−</p> Signup and view all the answers

    Which of the following statements about stomach acid is accurate?

    <p>Stomach acid helps in the digestion of food.</p> Signup and view all the answers

    What is the best definition of an Arrhenius base?

    <p>Any substance that produces OH− ions in solution.</p> Signup and view all the answers

    What is the role of calcium carbonate when consumed as an antacid?

    <p>It produces water and carbon dioxide through a neutralization reaction.</p> Signup and view all the answers

    Which of the following statements about water is true?

    <p>Water can act as either a proton donor or acceptor.</p> Signup and view all the answers

    Which of the following substances is considered the most basic?

    <p>Milk of magnesia</p> Signup and view all the answers

    Which substance functions as a weak acid?

    <p>HCN</p> Signup and view all the answers

    What is the hydroxide ion formula?

    <p>OH–</p> Signup and view all the answers

    Which statement regarding pH and strong bases is accurate?

    <p>The pH of a 1.0 M strong base is 14.</p> Signup and view all the answers

    What is the value of the ion product of water ($K_w$)?

    <p>$1.0 imes 10^{-14}$</p> Signup and view all the answers

    In an acidic solution, which relationship holds true regarding the concentrations of hydronium and hydroxide ions?

    <p>$[H_3O^+] &gt; [OH^-]$</p> Signup and view all the answers

    What is the pH of a neutral solution at 25 degrees Celsius?

    <p>7</p> Signup and view all the answers

    What is the relationship between pH and pOH in any aqueous solution?

    <p>pH + pOH = 14</p> Signup and view all the answers

    Which equation can be used to calculate the hydronium ion concentration from the hydroxide ion concentration?

    <p>$[H^+] = rac{1.0 imes 10^{-14}}{[OH^-]}$</p> Signup and view all the answers

    Which definition best describes an acid in the Brønsted-Lowry theory?

    <p>A substance that donates protons.</p> Signup and view all the answers

    Which of the following pairs constitutes a conjugate acid-base pair?

    <p>$NH_4^+$ and $NH_3$</p> Signup and view all the answers

    What characterizes strong acids compared to weak acids?

    <p>Strong acids completely ionize in solution.</p> Signup and view all the answers

    In the reaction $NH_3(g) + H_2O(l) \longrightarrow NH_4^+(aq) + OH^-(aq)$, what role does $H_2O$ play?

    <p>It is the acid.</p> Signup and view all the answers

    Which of the following is true about the ion product of water at 25 °C?

    <p>$[H_3O^+]$ equals $[OH^-]$.</p> Signup and view all the answers

    Which substance is classified as a strong base?

    <p>Potassium hydroxide ($KOH$)</p> Signup and view all the answers

    How does the concentration of $H_3O^+$ ions relate to the acidity of a solution?

    <p>Higher $H_3O^+$ concentration indicates a more acidic solution.</p> Signup and view all the answers

    What describes the role of hydroxide ions ($OH^-$) in acid-base reactions?

    <p>They can accept protons.</p> Signup and view all the answers

    In the Brønsted-Lowry definition, what function does water serve in the reaction $NH_3(g) + H_2O(l) \longrightarrow NH_4^+(aq) + OH^-(aq)$?

    <p>Proton donor</p> Signup and view all the answers

    Which substances can be classified as a conjugate acid-base pair in the reaction $H_2O + NH_3 \longrightarrow OH^- + NH_4^+$?

    <p>$NH_3$ and $NH_4^+$</p> Signup and view all the answers

    What is the significance of the ion product of water ($K_w$) at 25 °C?

    <p>It equals $1.0 \times 10^{-14}$</p> Signup and view all the answers

    Which of the following statements regarding strong acids is accurate?

    <p>They completely ionize in solution.</p> Signup and view all the answers

    What is the role of $H_3O^+$ in determining the acidity of a solution?

    <p>It determines the $pH$ value of the solution.</p> Signup and view all the answers

    In terms of acid strength, how do the listed strong acids compare?

    <p>They are all strong electrolytes.</p> Signup and view all the answers

    How does the concentration of $OH^-$ change in a basic solution compared to a neutral one?

    <p>It increases above $1 \times 10^{-7} M$.</p> Signup and view all the answers

    What describes the condition of pure water at 25 °C in terms of $H_3O^+$ and $OH^-$ concentrations?

    <p>They are both equal to $1 \times 10^{-7} M$.</p> Signup and view all the answers

    Which of the following best defines a strong base?

    <p>It completely dissociates in water to produce $OH^-$.</p> Signup and view all the answers

    In the context of acid-base reactions, what occurs between acids and bases?

    <p>They exchange protons to form conjugate pairs.</p> Signup and view all the answers

    What is the value of the ion product of water ($K_w$) at 25 degrees Celsius?

    <p>$1.0 imes 10^{-14}$</p> Signup and view all the answers

    How does the concentration of hydronium ions $[H_3O^+]$ change in an acidic solution?

    <p>$[H_3O^+] &gt; 1 imes 10^{-7}$</p> Signup and view all the answers

    What is the relationship of pH and pOH in a neutral solution?

    <p>$pH + pOH = 14$</p> Signup and view all the answers

    What can be inferred about a solution with a pH greater than 7?

    <p>The solution is basic.</p> Signup and view all the answers

    To calculate the pH from the concentration of hydronium ions, which formula is used?

    <p>$pH = -log[H_3O^+]$</p> Signup and view all the answers

    In basic solutions, how does the concentration of hydroxide ions $[OH^-]$ compare to hydronium ions $[H_3O^+]$?

    <p>$[OH^-] &gt; [H_3O^+]$</p> Signup and view all the answers

    What is the definition of a neutral solution in terms of hydronium and hydroxide ion concentrations?

    <p>$[H_3O^+] = [OH^-]$</p> Signup and view all the answers

    Which of the following describes the mathematical relationship between the hydronium and hydroxide ion concentrations?

    <p>They are inversely proportional.</p> Signup and view all the answers

    What happens to the concentration of $[H_3O^+]$ as the pH decreases?

    <p>It increases.</p> Signup and view all the answers

    What characteristic defines a Brønsted-Lowry acid?

    <p>It donates protons to another substance.</p> Signup and view all the answers

    Which of the following pairs constitutes a conjugate acid-base pair in the reaction $H_2O + NH_3 ightarrow OH^- + NH_4^+$?

    <p>$NH_4^+$ and $OH^-$</p> Signup and view all the answers

    What defines the $H_3O^+$ concentration of a neutral solution at 25 °C?

    <p>$1 imes 10^{-7} M$</p> Signup and view all the answers

    Which substance is considered a strong base?

    <p>Lithium hydroxide ($LiOH$)</p> Signup and view all the answers

    In the context of acid-base reactions, what role does the hydroxide ion ($OH^-$) play?

    <p>It lowers the concentration of $H_3O^+$.</p> Signup and view all the answers

    How do the listed strong acids compare in strength?

    <p>Certain strong acids are stronger than others based on their ionization.</p> Signup and view all the answers

    Which statement regarding the ion product of water at 25 °C is correct?

    <p>It equals $1 imes 10^{-14}$ at 25 °C.</p> Signup and view all the answers

    What occurs between acids and bases in a neutralization reaction?

    <p>Hydrogen ions combine with hydroxide ions to form water.</p> Signup and view all the answers

    Which of the following statements about acidic solutions is true?

    <p>They have a pH less than 7.</p> Signup and view all the answers

    What does a pH greater than 7 indicate about a solution?

    <p>The solution is basic.</p> Signup and view all the answers

    What occurs in a solution when the concentration of hydronium ions $[H_3O^+]$ exceeds that of hydroxide ions $[OH^-]$?

    <p>The solution is acidic.</p> Signup and view all the answers

    Which equation correctly represents the relationship between concentrations of hydronium and hydroxide ions in water at equilibrium?

    <p>$[H_3O^+] imes [OH^-] = 1.0 imes 10^{-14}$</p> Signup and view all the answers

    What is the pH of a solution where the concentration of hydroxide ions $[OH^-]$ is $1.0 imes 10^{-9}$ M?

    <p>9</p> Signup and view all the answers

    How is the pOH of a solution calculated from hydroxide ion concentration?

    <p>pOH = -log $[OH^-]$</p> Signup and view all the answers

    In a basic solution, how does the concentration of hydronium ions $[H_3O^+]$ compare to that of hydroxide ions $[OH^-]$?

    <p>$[H_3O^+] &lt; [OH^-]$</p> Signup and view all the answers

    What is the mathematical relationship between pH and pOH in an aqueous solution?

    <p>pH + pOH = 14.00</p> Signup and view all the answers

    Which concentration indicates a neutral solution?

    <p>$[H_3O^+] = [OH^-] = 1.0 imes 10^{-7}$ M</p> Signup and view all the answers

    Which of the following statements regarding acidic solutions is accurate?

    <p>They have a greater concentration of hydronium ions than hydroxide ions.</p> Signup and view all the answers

    What is the proper formula to calculate the hydronium ion concentration from the hydroxide ion concentration?

    <p>$[H_3O^+] = 1 imes 10^{-14} / [OH^-]$</p> Signup and view all the answers

    Study Notes

    Chapter 13: Acids and Bases

    • Exam Scope: Covers textbook, lectures, and assignments. Utilize class attendance, readings, practice problems, and online resources (OWLv2, ASP, multimedia activities) for effective preparation. Seek help if needed.

    Acid-Base Definitions

    • Arrhenius Definition:

      • Acids produce hydrogen ions (H+) in solution.
      • Bases produce hydroxide ions (OH-) in solution.
      • Limited applicability; not all cases fit this model.

    • Brønsted-Lowry Definition:

      • Broader than Arrhenius.
      • Applicable to solutions that do not contain water.
      • Focuses on proton (H+) transfer.
      • Acids are proton donors.
      • Bases are proton acceptors.

    Conjugate Pairs

    • Acid/Conjugate Base Pairs: In a reaction, the substances before and after the proton transfer form an acid/conjugate base pair. This is especially important in aqueous solutions with proton transfer.
    • Base/Conjugate Acid Pairs: Also in a reaction, the substances before and after the proton transfer form a base/conjugate acid pair. This is true in reactions and solutions with water.

    Strong and Weak Acids/Bases

    • Identifying Strong Acids/Bases: The provided text lists six strong acids and six strong bases. These undergo essentially complete ionization in aqueous solutions; this is crucial in calculations.

    pH and pH Calculations

    • H3O+ Concentration: Acidity is usually specified by the concentration of hydronium ions (H3O+) in moles per liter of solution (M).

    • Ion Product of Water (Kw): The product of H3O+ and OH concentrations in an aqueous solution. A constant at a given temperature.

    • Acidic/Basic Solutions: Characteristics and calculations for pH and pOH are included based on H3O+ and OH- concentration and pH values. The pH scale ranges from 0 to 14. A pH of 7 is neutral. Greater than 7 is basic and less than 7 is acidic.

    Acid Rain

    • Description: Formation and chemical reactions involved in acid rain. A combination of various factors.
    • Effects Include environmental damage to materials, water, human health, forests, and overall.

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    Description

    This quiz focuses on the fundamental concepts of acids and bases as defined by both the Arrhenius and Brønsted-Lowry theories. It covers conjugate acid-base pairs and their significance in chemical reactions. Prepare using lecture notes, textbook readings, and practice problems for success.

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