Chemistry Chapter 14 - Acid-Base Equilibria

Fundamental Equilibrium Concepts, including Chemical Equilibrium, Equilibrium Constants, Shifting Equilibria: Le Châtelier's Principle, and Equilibrium Calculations.

A compound that donates a proton to another compound.

<p>A pair of molecules or ions that differ by a single proton. The acid is the molecule or ion that donates a proton, and the base is the molecule or ion that accepts the proton.</p> Signup and view all the answers

<p>It emphasizes that the acid and base in a pair are related by the transfer of a single proton. The conjugate base is formed when the acid loses a proton, and the conjugate acid is formed when the base gains a proton.</p> Signup and view all the answers

<p>Species that can either accept or donate a proton.</p> Signup and view all the answers

<p>Water (H₂O)</p> Signup and view all the answers

<p>The process in which water molecules react with each other to form hydronium (H₃O⁺) and hydroxide (OH⁻) ions.</p> Signup and view all the answers

<p>The equilibrium constant for the autoionization of water, which is the product of the hydronium ion concentration and the hydroxide ion concentration.</p> Signup and view all the answers

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

<p>Because the concentration of water remains essentially constant in dilute aqueous solutions, it does not significantly change during autoionization, and therefore it is not included in the equilibrium constant expression.</p> Signup and view all the answers

<p>They are inversely proportional to each other. As the concentration of one increases, the concentration of the other decreases.</p> Signup and view all the answers

<p>A logarithmic scale used to express the acidity or basicity of a solution.</p> Signup and view all the answers

<p>They are related by the equation pH + pOH = 14.</p> Signup and view all the answers

<p>A neutral pH of 7 indicates a solution where the concentrations of hydronium and hydroxide ions are equal, leading to neither acidic nor basic properties.</p> Signup and view all the answers

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

<p>Use the antilog function: [H₃O⁺] = 10⁻pH.</p> Signup and view all the answers

<p>A logarithmic measure of the hydroxide ion concentration in a solution, similar to pH but focused on OH⁻ instead of H₃O⁺ .</p> Signup and view all the answers

<p>pOH = - log[OH⁻]</p> Signup and view all the answers

<p>Common substances and their associated pH ranges include: 1 M HCl (pH 0), gastric juice (pH 1-2), lime juice (pH 2-3), 1 M CH₃CO₂H (pH 3), stomach acid (pH 3-4), wine (pH 3-4), orange juice (pH 3-4), coffee (pH 4-5), rainwater (pH 5-6), pure water (pH 7), blood (pH 7.3-7.4), ocean water (pH 8), baking soda (pH 9), Milk of Magnesia (pH 10-11), household ammonia (pH 11-12), bleach (pH 12-13), 1 M NaOH (pH 14).</p> Signup and view all the answers

<p>A laboratory technique used to determine the concentration of an unknown solution by reacting it with a solution of known concentration.</p> Signup and view all the answers

<p>A solution that resists changes in pH when small amounts of acid or base are added.</p> Signup and view all the answers

<p>Acids that can donate more than one proton in a reaction.</p> Signup and view all the answers

<p>The reaction of a salt with water to produce an acidic or basic solution.</p> Signup and view all the answers

<p>HA(aq) + B(aq) ⇌ A⁻(aq) + HB⁺(aq)</p> Signup and view all the answers