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?

Amphoteric Signup and view all the answers

What is a strong acid in aqueous solution?

Completely ionized Signup and view all the answers

What is the Ka for a weak acid called?

Acid dissociation constant Signup and view all the answers

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

Water and a soluble salt Signup and view all the answers

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

A proton donor Signup and view all the answers

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

Diprotic Signup and view all the answers

When does a neutral solution occur?

[H3O+] = [OH-] Signup and view all the answers

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

1.0 E-7 M Signup and view all the answers

What is the pH of an acidic solution?

Less than seven Signup and view all the answers

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

Kw, the ion product constant for water Signup and view all the answers

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

10 Signup and view all the answers

What is phenolphthalein used as?

An indicator Signup and view all the answers

What is a buffer composed of?

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

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

The equivalence point Signup and view all the answers

What is the Kb for a weak base called?

Base ionization constant Signup and view all the answers

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

Acidic Signup and view all the answers

What is the device used to perform a titration called?

Buret 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.