Acids and Bases Flashcards
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Questions and Answers

What is an acid?

An electrolyte

By the Arrhenius definition, what does a base produce in aqueous solution?

OH-

What is an H+ ion in aqueous solution more accurately described as?

A hydronium ion

What do you call a substance that can act as an acid or a base?

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

What is a strong acid in aqueous solution?

<p>Completely ionized</p> Signup and view all the answers

What is the Ka for a weak acid called?

<p>Acid dissociation constant</p> Signup and view all the answers

What does the reaction of an acid and a base in equal molar amounts produce?

<p>Water and a soluble salt</p> Signup and view all the answers

According to Bronsted-Lowry theory, what is an acid?

<p>A proton donor</p> Signup and view all the answers

What type of acid is sulfuric acid, H2SO4(aq)?

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

When does a neutral solution occur?

<p>[H3O+] = [OH-]</p> Signup and view all the answers

In pure water at 25°C, what does [OH-] equal?

<p>1.0 E-7 M</p> Signup and view all the answers

What is the pH of an acidic solution?

<p>Less than seven</p> Signup and view all the answers

What is the product of [H3O+] and [OH-] in water?

<p>Kw, the ion product constant for water</p> Signup and view all the answers

If the pH drops from 3 to 2, what factor does [H3O+] change by?

<p>10</p> Signup and view all the answers

What is phenolphthalein used as?

<p>An indicator</p> Signup and view all the answers

What is a buffer composed of?

<p>Both a weak acid and its conjugate base, as well as a weak base and its conjugate acid</p> Signup and view all the answers

What should the end point in a titration be close to?

<p>The equivalence point</p> Signup and view all the answers

What is the Kb for a weak base called?

<p>Base ionization constant</p> Signup and view all the answers

If the pOH of a solution is 8, how would you describe the solution?

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

What is the device used to perform a titration called?

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

Study Notes

Acids and Bases Study Notes

  • An acid is classified as an electrolyte, capable of conducting electricity when dissolved in water.
  • According to the Arrhenius definition, a base generates hydroxide ions (OH-) when in aqueous solution.
  • In aqueous solutions, an H+ ion more accurately exists as a hydronium ion (H3O+).
  • Substances that can function as either an acid or a base are termed amphoteric.
  • A strong acid in solution is characterized by complete ionization, meaning it dissociates fully into its ions.
  • The acid dissociation constant (Ka) quantifies the strength of a weak acid based on its equilibrium concentration of ions.
  • When an acid reacts with a base in equal molar amounts, the products are water and a soluble salt.
  • According to Bronsted-Lowry theory, an acid acts as a proton donor, transferring H+ ions to other substances.
  • Sulfuric acid (H2SO4) is classified as a diprotic acid, capable of donating two protons.
  • A neutral solution is characterized by equal concentrations of hydronium and hydroxide ions, expressed as [H3O+] = [OH-].
  • In pure water at 25°C, the concentration of hydroxide ions ([OH-]) is 1.0 x 10^-7 M.
  • An acidic solution has a pH value that is lower than seven, indicating a higher concentration of hydronium ions.
  • The product of the concentrations of H3O+ and OH- in water is known as Kw, the ion product constant for water.
  • A drop in pH from 3 to 2 indicates that the concentration of H3O+ has increased by a factor of 10.
  • Phenolphthalein serves as a common pH indicator, changing color based on pH levels.
  • A buffer solution consists of either a weak acid and its conjugate base or a weak base and its conjugate acid, providing resistance to changes in pH.
  • In titration, the end point, where the indicator changes color, should ideally coincide with the equivalence point, where the reactants are in stoichiometric proportions.
  • The base ionization constant (Kb) determines the degree of ionization of a weak base in aqueous solution.
  • A solution with a pOH of 8 is classified as acidic, with a corresponding relatively low pH.
  • A buret is the apparatus used to precisely measure and dispense liquid in titrations.

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Description

This quiz features key concepts and definitions related to acids and bases. Test your knowledge on electrolytes, Arrhenius definitions, and amphoteric substances. Perfect for students studying chemistry fundamentals.

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