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 (D)</p> Signup and view all the answers

What impact does acid rain have on the environment?

<p>It can damage aquatic ecosystems (A)</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. (A)</p> Signup and view all the answers

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

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

Which of these acids is commonly not found in wines?

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

Which property is characteristic of acids?

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

Which of the following substances would exhibit the highest acidity?

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

Which substance is classified as a base?

<p>NaOH (A)</p> Signup and view all the answers

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

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

Which of the following substances is considered the most basic?

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

Which substance functions as a weak acid?

<p>HCN (B)</p> Signup and view all the answers

What is the hydroxide ion formula?

<p>OH– (A)</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. (B)</p> Signup and view all the answers

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

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

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

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

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

<p>7 (A)</p> Signup and view all the answers

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

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

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

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

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

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

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

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

What characterizes strong acids compared to weak acids?

<p>Strong acids completely ionize in solution. (D)</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. (C)</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 $[OH^-]$. (A)</p> Signup and view all the answers

Which substance is classified as a strong base?

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

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

<p>They can accept protons. (C)</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 (D)</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 $NH_4^+$ (D)</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 $1.0 \times 10^{-14}$ (A)</p> Signup and view all the answers

Which of the following statements regarding strong acids is accurate?

<p>They completely ionize in solution. (D)</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. (D)</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. (B)</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 $1 \times 10^{-7} M$. (B)</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 $1 \times 10^{-7} M$. (A)</p> Signup and view all the answers

Which of the following best defines a strong base?

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

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

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

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

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

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

<p>$pH + pOH = 14$ (D)</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. (B)</p> Signup and view all the answers

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

<p>$pH = -log[H_3O^+]$ (C)</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>$[OH^-] &gt; [H_3O^+]$ (A)</p> Signup and view all the answers

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

<p>$[H_3O^+] = [OH^-]$ (A)</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. (C)</p> Signup and view all the answers

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

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

What characteristic defines a Brønsted-Lowry acid?

<p>It donates protons to another substance. (A)</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 $OH^-$ (B)</p> Signup and view all the answers

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

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

Which substance is considered a strong base?

<p>Lithium hydroxide ($LiOH$) (A)</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 $H_3O^+$. (D)</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. (B)</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. (A)</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. (A)</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. (D)</p> Signup and view all the answers

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

<p>The solution is basic. (A)</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. (D)</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>$[H_3O^+] imes [OH^-] = 1.0 imes 10^{-14}$ (A)</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 (A)</p> Signup and view all the answers

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

<p>pOH = -log $[OH^-]$ (B)</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>$[H_3O^+] &lt; [OH^-]$ (D)</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 (C)</p> Signup and view all the answers

Which concentration indicates a neutral solution?

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

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

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

Flashcards

Acid definition

Substances that donate protons (H+ ions) in a solution.

Base definition

Substances that accept protons (H+ ions) in a solution.

Strong Acid

An acid that completely ionizes in solution.

pH calculation

A measure of the concentration of hydrogen ions (H+) in a solution, used to indicate the acidity or basicity of the solution.

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Antacid reaction (with NaHCO3)

Sodium bicarbonate (NaHCO3) neutralizes acids, producing water and carbon dioxide gas. This reaction helps to neutralize excess stomach acid.

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Acid Properties

Acids have several properties, including a sour taste, the ability to turn litmus paper red, and the ability to dissolve some metals.

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Base Identification

A base is a substance that typically has a bitter taste, feels slippery to the touch, and can neutralize acids. A common example is sodium bicarbonate (NaHCO3).

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Arrhenius Base Definition

An Arrhenius base is a substance that produces hydroxide ions (OH-) when dissolved in water.

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Bronsted-Lowry Base Definition

A Bronsted-Lowry base is a substance that accepts protons (H+ ions) when in solution.

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Water as a Proton Donor/Acceptor

Water can act as both a proton donor (acid) and a proton acceptor (base) because it can both lose and gain protons.

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Weak Base

A weak base only partially ionizes in solution, meaning it doesn't dissociate entirely into ions.

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Weak Acid

A weak acid only partially ionizes in solution, meaning it doesn't dissociate entirely into ions.

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pH of Strong Base Solution

A 1.0 M solution of a strong base has a pH of 14.

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pH Scale

A scale used to measure the acidity or basicity of a solution. Values range from 0 to 14, with 7 being neutral, below 7 being acidic and above 7 being basic.

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Acidic Solution

A solution with a pH less than 7, which means it has a higher concentration of hydrogen ions (H+).

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Basic Solution

A solution with a pH greater than 7, which means it has a lower concentration of hydrogen ions (H+).

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pH Change: 1 Unit Difference

A one-unit change in pH represents a tenfold change in hydrogen ion concentration.

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Tartness of Vinegar

Vinegar's tartness comes from acetic acid.

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Active Ingredient in Aspirin

Aspirin's main ingredient is acetylsalicylic acid.

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Stomach Acid

The stomach acid is hydrochloric acid (HCl).

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Arrhenius Acid

A substance that produces hydrogen ions ($H^+$) in solution.

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Arrhenius Base

A substance that produces hydroxide ions ($OH^-$) in solution.

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Brønsted–Lowry Acid

A substance that donates protons ($H^+$ ions) in a solution.

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Brønsted–Lowry Base

A substance that accepts protons ($H^+$ ions) in a solution.

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Conjugate Acid-Base Pair

Two substances that differ by only one proton ($H^+$ ion).

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Strong Base

A base that completely ionizes in solution.

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pH

A measure of the hydrogen ion concentration ($H^+$) in a solution, ranging from 0 to 14. Lower pH means higher acidity, and higher pH means higher alkalinity.

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Ion Product of Water ($K_w$)

The product of the concentrations of hydronium ions ($[H_3O^+]$) and hydroxide ions ($[OH^-]$) in water at a given temperature. It is a constant value, $1 imes 10^{-14}$ at 25°C.

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How to Calculate $pH$

The $pH$ of a solution can be calculated by taking the negative logarithm of the hydronium ion concentration: $pH = -log[H_3O^+]$

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Inversely Proportional Relationship

The concentrations of hydronium ions and hydroxide ions in water are inversely proportional. If one increases, the other decreases, keeping their product constant.

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Basic (Alkaline) Solution

A solution with a higher concentration of hydroxide ions ($[OH^-]$) than hydronium ions ($[H_3O^+]$), resulting in a pH greater than 7.

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Neutral Solution

A solution where the concentrations of hydronium and hydroxide ions are equal, resulting in a pH of 7.

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$pH$ Scale Range

The $pH$ scale ranges from 0 to 14, with 0 being the most acidic, 14 being the most basic, and 7 being neutral.

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Antacid Action of Sodium Bicarbonate ($NaHCO_3$)

Sodium bicarbonate reacts with stomach acid (HCl) to produce sodium chloride (NaCl), water ($H_2O$), and carbon dioxide ($CO_2$)

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Antacid Action of Sodium Carbonate ($Na_2CO_3$)

Sodium carbonate reacts with stomach acid (HCl) to produce sodium chloride (NaCl), water ($H_2O$), and carbon dioxide ($CO_2$)

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Brnsted-Lowry acid

A substance that donates protons ($H^+$ ions) in a solution.

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Brnsted-Lowry base

A substance that accepts protons ($H^+$ ions) in a solution.

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What is an acid?

An acid is a substance that donates protons (H+ ions) in a solution.

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What is a base?

A base is a substance that accepts protons (H+ ions) in a solution.

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pH + pOH = 14

The sum of the pH and pOH values for a solution is always 14.

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Antacid action of Sodium carbonate (Na2CO3)

Sodium carbonate reacts with stomach acid (HCl) to produce sodium chloride (NaCl), water (H2O), and carbon dioxide (CO2), neutralizing excess stomach acid.

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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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Related Documents

CHEM 1010 General Study Guide Chapters 13 PDF
Practice Exam Chapter 13 PDF
CHEM 1010 General Study Guide - Chapters 13 PDF

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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