Acids and Bases Overview
19 Questions
4 Views

Choose a study mode

Play Quiz
Study Flashcards
Spaced Repetition
Chat to Lesson

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

Which of the following is NOT a physical or chemical property of acids?

  • Causes a stinging sensation on skin
  • Neutralizes bases (correct)
  • Sour taste
  • Turns blue litmus paper red

What is the formula for the hydronium ion?

H3O+

Which of the following scientists is NOT associated with a model of acid-base theory?

  • Lewis
  • Arrhenius
  • Thomson (correct)
  • Brønsted-Lowry

What is the difference between the strength and concentration of an acid?

<p>Strength refers to the degree of ionization, while concentration refers to the amount of acid in a solution. (B)</p> Signup and view all the answers

Which of the following acids is diprotic?

<p>H2SO4 (B)</p> Signup and view all the answers

What does pH stand for?

<p>Power of Hydrogen (A)</p> Signup and view all the answers

The pOH scale is the inverse logarithmic scale of the hydrogen ion concentration.

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

What is the formula used to calculate the pH of a solution?

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

Neutralization reactions are double-replacement reactions.

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

What is the point in a titration reaction where moles of H+ from the acid equals moles of OH- from the base?

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

Titration curves show a sharp rise in pH at the equivalence point for both strong acid and strong base reactions, and weak acid and strong base reactions.

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

What type of acid is sulfuric acid (H2SO4)?

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

What is the conjugate base of H3PO4?

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

Which of the following is a strong base?

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

A weak base ionizes completely in a dilute aqueous solution.

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

How do acids and bases behave according to the Brønsted-Lowry model?

<p>In the Brønsted-Lowry model, an acid donates protons (H+), and a base accepts protons (H+).</p> Signup and view all the answers

Which of the following is NOT a Lewis acid?

<p>NH3 (B)</p> Signup and view all the answers

In the Lewis model, a Lewis base ______ a pair of electrons, while a Lewis acid ______ a pair of electrons.

<p>donates, accepts</p> Signup and view all the answers

Match the following terms with their definitions:

<p>Monoprotic acid = An acid that can donate two protons per molecule Diprotic acid = An acid that can donate one proton per molecule Polyprotic acid = An acid that can donate more than one proton per molecule Neutralization = A reaction between an acid and a base that produces salt and water</p> Signup and view all the answers

Flashcards

What are the common characteristics of acids?

Acids have a sour taste, turn blue litmus paper red, and neutralize bases.

What are the common characteristics of bases?

Bases have a bitter taste, turn red litmus paper blue, and neutralize acids.

How is the hydronium ion (H3O+) formed?

The hydronium ion (H3O+) is formed when a water molecule accepts a proton (H+) from another water molecule in a process called self-ionization of water.

What is the Arrhenius definition of acids and bases?

Arrhenius defined acids as substances that produce hydrogen ions (H+) when dissolved in water, while bases produce hydroxide ions (OH-).

Signup and view all the flashcards

What is the Brønsted-Lowry definition of acids and bases?

Brønsted-Lowry defined acids as proton (H+) donors, and bases as proton (H+) acceptors.

Signup and view all the flashcards

What is a conjugate acid?

A conjugate acid is formed when a base accepts a proton (H+).

Signup and view all the flashcards

What is a conjugate base?

A conjugate base is formed when an acid donates a proton (H+).

Signup and view all the flashcards

What is a conjugate acid-base pair?

A conjugate acid-base pair consists of two substances related to each other by donating and accepting a single proton (H+).

Signup and view all the flashcards

What is the Lewis definition of acids and bases?

A Lewis acid is a substance that accepts a pair of electrons, while a Lewis base donates a pair of electrons.

Signup and view all the flashcards

What are strong acids?

Strong acids ionize completely in water, releasing all their hydrogen ions (H+).

Signup and view all the flashcards

What are weak acids?

Weak acids only partially ionize in water, releasing only some of their hydrogen ions (H+).

Signup and view all the flashcards

What is concentration?

Concentration refers to the amount of solute dissolved in a given volume of solution.

Signup and view all the flashcards

What is a concentrated solution?

A concentrated solution has a high amount of solute dissolved in a given volume of solvent.

Signup and view all the flashcards

What is a dilute solution?

A dilute solution has a low amount of solute dissolved in a given volume of solvent.

Signup and view all the flashcards

What is molarity?

Molarity (M) is a unit of concentration that expresses the number of moles of solute per liter of solution.

Signup and view all the flashcards

What is a monoprotic acid?

Monoprotic acids release one proton (H+) per molecule when they ionize.

Signup and view all the flashcards

What is a diprotic acid?

Diprotic acids release two protons (H+) per molecule when they ionize.

Signup and view all the flashcards

What is a polyprotic acid?

Polyprotic acids can release more than two protons (H+) per molecule when they ionize.

Signup and view all the flashcards

What does pH measure?

pH measures the acidity or alkalinity of a solution.

Signup and view all the flashcards

What does pOH measure?

pOH measures the concentration of hydroxide ions (OH-) in a solution.

Signup and view all the flashcards

What is a neutralization reaction?

A neutralization reaction occurs when an acid and a base react to form salt and water.

Signup and view all the flashcards

What is titration?

Titration is a technique used to determine the concentration of an unknown solution by reacting it with a solution of known concentration.

Signup and view all the flashcards

What is the equivalence point in a titration?

The equivalence point in a titration is when the moles of acid and base are equal.

Signup and view all the flashcards

What is the endpoint in a titration?

The endpoint in a titration is when the indicator changes color, signaling that the neutralization reaction is complete.

Signup and view all the flashcards

How do you calculate pH?

The pH of a solution can be calculated using the formula pH = -log[H+], where [H+] is the concentration of hydrogen ions.

Signup and view all the flashcards

What is the difference between pH and pOH?

pH is a measure of the hydrogen ion concentration in a solution, while pOH is a measure of the hydroxide ion concentration in a solution.

Signup and view all the flashcards

What is the pH scale?

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

Signup and view all the flashcards

What is the pOH scale?

The pOH scale is also from 0 to 14, with 0 being the most basic and 14 being the most acidic.

Signup and view all the flashcards

How are pH and pOH related?

The pH and pOH are related by the equation: pH + pOH = 14.

Signup and view all the flashcards

How do you determine pH?

The pH of a solution can be determined using a pH meter or pH paper.

Signup and view all the flashcards

Study Notes

Acids and Bases

  • Acids and bases have distinct physical and chemical properties
  • Acids taste sour, turn blue litmus paper red, and neutralize bases. Bases taste bitter, turn red litmus paper blue, and neutralize acids.
  • Acids and bases are good conductors of electricity, and acids are corrosive, while bases are caustic. Acids feel astringent and bases feel slippery.
  • Acids and bases react with each other to produce a salt and water
  • Water produces equal numbers of hydrogen and hydroxide ions in a process called self-ionization
  • Hydronium ion is H3O+

Strength and Concentration

  • Acids and bases differ in strength (strong/weak) and concentration (concentrated/diluted).
  • Strong acids ionize completely, while weak acids ionize partially.
  • Strong bases completely ionize to produce hydroxide ions, while weak bases only partly ionize.
  • Concentration refers to the amount of solute in a given volume of solution.
  • Molarity (M) is calculated as moles of solute divided by liters of solution.

pH

  • pH is a measure of the concentration of hydrogen ions in a solution.
  • pH scale ranges from 0 to 14.
  • pOH is a measure of the concentration of hydroxide ions in a solution.
  • The sum of pH and pOH equals 14.
  • Calculations use the formulas: pH = -log[H+], pOH = -log[OH-], 10-pH = [H+], 10-pOH = [OH-], [H+][OH-] = 1 x 10-14

Neutralization

  • Neutralization is a reaction between an acid and a base that produces a salt and water.
  • A salt is an ionic compound formed from a cation from the base and an anion from the acid.
  • Neutralization is a double-replacement reaction.

Titration

  • Titration is a method for determining the concentration of an unknown solution by reacting it with a solution of known concentration.
  • A measured volume of the unknown solution is placed in a flask, and a known concentration solution (titrant) is added from a burette until the equivalence point is reached.
  • Equivalence point occurs when the moles of H+ ions from the acid equal the moles of OH- ions from the base.
  • An abrupt change in pH marks the equivalence point.

Models of Acids and Bases

  • Arrhenius model: Acids produce H+ ions in solution, and bases produce OH- ions.
  • Brønsted-Lowry model: Acids donate protons (H+), and bases accept protons. A conjugate acid-base pair is formed.
  • Lewis model: Acids accept electron pairs, and bases donate electron pairs.

Indicators

  • Chemical dyes that change color depending on the pH of a solution are called acid-base indicators.
  • Indicators are used to track the progress of a titration.
  • An end point is the point in a titration where the indicator changes color.

Examples of Acids and Bases

  • Strong acids: HCl (hydrochloric acid), HNO3 (nitric acid), H2SO4 (sulfuric acid), HBr (hydrobromic acid), HI (hydroiodic acid), HClO4 (perchloric acid).
  • Weak acids: CH3COOH (acetic acid), HCOOH (formic acid).
  • Strong bases: NaOH (sodium hydroxide), KOH (potassium hydroxide), Ca(OH)2 (calcium hydroxide), Ba(OH)2 (Barium hydroxide).

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

Quiz Team

Related Documents

U5 Acids and Bases Honors Chemistry PDF

Description

This quiz focuses on the distinct properties of acids and bases, including their physical and chemical characteristics. It also covers the concepts of strength and concentration, including the differences between strong and weak acids and bases. Test your knowledge on these fundamental chemical concepts!

More Like This

Use Quizgecko on...
Browser
Open
Browser
Browser