Chemistry Acid-Base Concepts Quiz

False (B)

$K_w$ represents the equilibrium constant of the dissociation of water, calculated as [H+][OH−].

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

<p>HCl(g) → H+(aq) + Cl−(aq) = Strong Acid CH3COOH(aq) ↔ CH3COO−(aq) + H+(aq) = Weak Acid NaOH(s) → Na+(aq) + OH−(aq) = Strong Base NH3(aq) + H2O(l) ↔ NH4+(aq) + OH−(aq) = Weak Base</p> Signup and view all the answers

<p>13.00 (A)</p> Signup and view all the answers

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

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

<p>sulfuric acid</p> Signup and view all the answers

<p>HCl = Strong monoprotic acid H₂SO₄ = Strong diprotic acid NaOH = Strong base that fully ionizes KOH = Strong base that fully ionizes</p> Signup and view all the answers

<p>1.70 (B)</p> Signup and view all the answers

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

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

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

<p>Brønsted-Lowry acid = Proton donor Brønsted-Lowry base = Proton acceptor Acid (HA) + Water = Produces H₃O⁺ Base (B) + Water = Produces OH⁻</p> Signup and view all the answers

<p>1.30 (A)</p> Signup and view all the answers

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

<p>0.200 mol dm⁻³</p> Signup and view all the answers

<p>3.5 x 10⁻³</p> Signup and view all the answers

<p>HCl = Strong monoprotic acid H2SO4 = Strong diprotic acid HNO3 = Strong monoprotic acid pH = 0.699 = pH of 0.100 mol dm⁻³ H2SO4</p> Signup and view all the answers

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

<p>0.001 mol/dm3</p> Signup and view all the answers

<p>3.00</p> Signup and view all the answers

<p>pH 1.00 = 0.10 mol/dm3 pH 2.00 = 0.010 mol/dm3 pH 3.00 = 0.001 mol/dm3 pH 4.00 = 0.0001 mol/dm3</p> Signup and view all the answers

<p>1.40 (A)</p> Signup and view all the answers

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

<p>0.013 mol/dm3</p> Signup and view all the answers

A substance that donates a proton (H+ ion) in a chemical reaction.

A substance that accepts a proton (H+ ion) in a chemical reaction.

An acid that almost completely dissociates (breaks apart) into ions in water.

An acid that only slightly dissociates in water.

The equilibrium constant for the dissociation of water.

The pH of a strong monoprotic acid is calculated by taking the negative logarithm of the acid's concentration.

An acid that releases one proton per molecule.

pH = -log[H+]

An acid that releases two protons per molecule.

The concentration of H+ ions from a diprotic acid is twice the concentration of the acid.

Kw = [H⁺][OH⁻], constant for aqueous solutions at a specific temperature.

2.00

1.00 x 10⁻¹⁴ mol²/dm⁶

Equal to the hydroxide ion concentration

pH is a measure of hydrogen ion concentration in a solution. It's a logarithmic scale because hydrogen ion concentrations can vary widely.

pH = -log[H+]

Calculate pH when given hydrogen ion concentration (e.g., [H+] = 0.010 mol/dm3).

Find [H+] when pH is known. Use inverse logarithm: [H+] = 10-pH

Hydrogen ion concentration units are mol/dm3

Example: Calculate pH of solution with [H+] = 0.050 mol/dm3.

Logarithms are used because of the wide range of hydrogen ion concentrations found in solutions.

A scale used to measure acidity or basicity of a solution.

To calculate the pH of a strong acid solution, directly use the acid's concentration as the hydrogen ion concentration ([H+]). Then, plug this value into the pH equation: pH = -log[H+].

To determine the pH of a strong base solution, calculate the hydroxide ion concentration ([OH-]) first. Then, use the Kw expression (Kw = [H+][OH-]) to find the hydrogen ion concentration ([H+]). Finally, calculate pH using the equation pH = -log[H+].

A diprotic acid can donate two moles of hydrogen ions (H+) per mole of acid. This means it has two acidic protons.

A strong base, like sodium hydroxide, turns universal indicator paper dark blue, indicating a high pH value.

The ion product constant of water (Kw) is an equilibrium constant that defines the relationship between hydrogen ion ([H+]) and hydroxide ion ([OH-]) concentrations in water at a given temperature: Kw = [H+][OH-]