Acid (Arrhenius Definition): A substance that increases the concentration of H⁺ ions (protons) in aqueous solution.
Example: HCl dissociates to produce H⁺ and Cl⁻.
Base (Arrhenius Definition): A substance that increases the concentration of OH⁻ ions in aqueous solution.
Example: NaOH dissociates to produce Na⁺ and OH⁻.
Proton (H⁺) Donor (Brønsted-Lowry Definition): An acid is a substance that donates a proton to another species.
Example: H₂SO₄ donates H⁺ ions in solution.
Proton (H⁺) Acceptor (Brønsted-Lowry Definition): A base is a substance that accepts a proton from another species.
Example: NH₃ accepts H⁺ to form NH₄⁺.
Electron Pair Acceptor (Lewis Definition): An acid is a substance that can accept a pair of electrons to form a covalent bond.
Example: BF₃ accepts an electron pair from NH₃.
pH: A logarithmic scale measuring the acidity or alkalinity of a solution, calculated as (\text{pH} = -\log[H^+]).
Range: 0 (most acidic) to 14 (most basic), with 7 being neutral.
1. What does the term 'acid-base definition' refer to in chemistry?
2. What is the hydrogen ion concentration in a neutral solution with a pH of 7?
3. What is the primary role of strong acids and bases compared to weak acids and bases in chemical reactions?
Acid — definition?
Substance increasing H⁺ in solution.
pH scale — range?
0 to 14, measures acidity or alkalinity.
Strong vs weak acids — difference?
Strong dissociate fully; weak dissociate partially.
pH — definition?
Logarithmic measure of 0H^+ concentration.
[H^+] — effect on pH?
Higher 0H^+ lowers pH.
pH 7 — solution type?
Neutral solution.
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