Acid-Base Chemistry Quiz

<p>Water can act as both an acid and a base. (B)</p> Signup and view all the answers

<p>[OH-] &gt; [H3O+] (C), [H3O+] &lt; [OH-] (D)</p> Signup and view all the answers

<p>1.0 x 10^-9 M (A)</p> Signup and view all the answers

<p>2NH3  NH4+ + NH2- (D)</p> Signup and view all the answers

<p>12 (D)</p> Signup and view all the answers

<p>NH4+ (D)</p> Signup and view all the answers

<p>Kc = [NH4+][NH2-]/[NH3]^2 (C)</p> Signup and view all the answers

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

<p>2.0 x 10^-11 M (C)</p> Signup and view all the answers

<p>10 (D)</p> Signup and view all the answers

<p>2.5 (A)</p> Signup and view all the answers

<p>6.3 x 10^-11 M (B)</p> Signup and view all the answers

<p>1.0 x 10^-9 M (D)</p> Signup and view all the answers

<p>13.0 (A)</p> Signup and view all the answers

<p>2.0 (A)</p> Signup and view all the answers

<p>3.2 x 10^-10 M (C)</p> Signup and view all the answers

<p>6.0 (A)</p> Signup and view all the answers

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

<p>Stronger acids have lower pH values. (C)</p> Signup and view all the answers

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

<p>Weak acids only partially dissociate in water. (A)</p> Signup and view all the answers

<p>The reaction seeks to achieve equilibrium by favoring the formation of the most stable products. (A)</p> Signup and view all the answers

<p>Stronger bases have lower pOH values. (B)</p> Signup and view all the answers

<p>Carbonic acid (H2CO3) (A)</p> Signup and view all the answers

<p>Stronger acids ionize to a greater extent. (D)</p> Signup and view all the answers

<p>Kb = [HB+][OH-] / [B] (B)</p> Signup and view all the answers

<p>The relationship between the concentrations depends on the specific base and its Kb value. (C)</p> Signup and view all the answers

<p>Ethylamine (C2H5NH2) - Kb = 4.7 × 10^-4 (D)</p> Signup and view all the answers

<p>The pH increases. (B)</p> Signup and view all the answers

<p>A smaller Kb value corresponds to a stronger conjugate acid. (C)</p> Signup and view all the answers

<p>We calculate the concentration of OH- ions first, instead of H+ ions. (C)</p> Signup and view all the answers

<p>The solution can be acidic, basic, or neutral depending on the relative concentrations of the base and its conjugate acid. (A)</p> Signup and view all the answers

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

<p>Water is a very strong electrolyte. (C)</p> Signup and view all the answers

<p>The process where water molecules react with each other to form hydronium and hydroxide ions. (C)</p> Signup and view all the answers

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

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

<p>Water acts as a base, accepting a proton from CH3COOH. (C)</p> Signup and view all the answers

<p>It enables water to dissolve a wide range of substances, both polar and nonpolar. (A)</p> Signup and view all the answers

<p>Water acts as a reactant, donating and accepting protons. (D)</p> Signup and view all the answers

<p>The reaction of water with HCl to form H3O+ and Cl-. (B), The reaction of water with itself to form H3O+ and OH-. (C)</p> Signup and view all the answers

The process where water molecules self-ionize to form H3O+ and OH- ions.

The ion product of water, equal to [H3O+][OH-] at 25°C.

A substance that only partially ionizes in solution, like water.

A measure of the strength of an acid in solution, showing the extent of dissociation.

A measure of the strength of a base in solution, showing the extent of dissociation.

Water is known as a unique solvent due to its ability to dissolve many substances.

The process where water molecules ionize to produce H3O+ and OH- ions.

Species capable of acting as both an acid and a base depending on the reaction.

A substance that donates protons (H+), acting as an acid in reactions.

A species that accepts protons (H+), acting as a base in reactions.

Water acts as an acid when it donates a proton to a base.

Water behaves as a base when it accepts a proton from an acid.

Reactions showcasing water's duality: with NH3 (as acid) and CH3COOH (as base).

A solution where [H3O+] = [OH-].

A solution where [H3O+] > [OH-].

A solution where [OH-] > [H3O+].

The product of H3O+ and OH- concentrations in water at 25°C.

Compare [H3O+] and [OH-] to find acidity or basicity.

Use Kw to find hydroxide concentration from H3O+ concentration.

The strongest acids that can exist in liquid ammonia solution.

An acid that completely dissociates in water, releasing protons.

An acid that partially dissociates in solution, not releasing all protons.

A base that readily accepts protons in solution, producing more hydroxide ions.

A base that does not readily accept protons, resulting in fewer hydroxide ions.

A scale measuring the acidity or basicity of a solution, ranging from 0 to 14.

A scale measuring the concentration of hydroxide ions; lower pOH means stronger bases.

Strength of acids/bases depends on their hydrogen or hydroxide ion concentration.

The tendency of an acid or base to ionize in solution affects reaction direction.

NH3 ionizes to form NH4+ and OH- in water.

Kb = [NH4+][OH-] / [NH3] under constant water concentration.

Ammonia has a Kb value of 1.8 × 10–5, indicating weak ionization.

For weak bases, calculate [OH-] first, not [H+].

Kb for hydroxylamine is 1.1 × 10–6, classifying it as weak.

Strong bases have large Kb values; weak bases have small Kb values.

Aniline has a Kb of 4.0 × 10–10, indicating low basicity.

A measure of hydroxide ion concentration, defined as pOH = -log[OH-].

To find [OH-], use [OH-] = 10^(-pOH).

Kw = [H3O+] * [OH-] = 1.0 x 10^-14 at 25°C.

The sum of pH and pOH equals 14 at 25°C.

pH = -log[H3O+]. This derives from [H3O+] concentration.

pOH can be calculated using pOH = 14 - pH.

At pH 7.40, [H3O+] = 10^-7.40 ≈ 4.0 x 10^-8 M.

Using pOH, [OH-] = 10^-6.6 ≈ 2.51 x 10^-7 M.