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Gen Chem (10)
| Question | Answer |
|---|---|
| What is the Arrhenius definition of an acid and base? | Acid = produces H⁺ ions in aqueous solution. Base = produces OH⁻ ions in aqueous solution. |
| What is the Brønsted-Lowry definition of an acid and base? | Acid = proton (H⁺) donor. Base = proton (H⁺) acceptor. Does NOT require aqueous solution. |
| What is the Lewis definition of an acid and base? | Acid = electron pair acceptor. Base = electron pair donor. It is the broadest definition. |
| How do the three acid-base definitions compare in scope? | Arrhenius (narrowest, aqueous only) ⊂ Brønsted-Lowry (most common, proton transfer) ⊂ Lewis (broadest, electron transfer). |
| What is a conjugate acid-base pair? | Two species that differ by exactly one proton (H⁺). The acid loses H⁺ to form its conjugate base; the base gains H⁺ to form its conjugate acid. |
| What is the inverse relationship between acid/base strength and conjugate strength? | The stronger the acid/base, the weaker its conjugate. The weaker the acid/base, the stronger its conjugate. |
| What Ka/Kb values indicate strong vs. weak acids/bases? | Strong: Ka or Kb > 1 (complete dissociation). Weak: Ka or Kb <<< 1 (partial dissociation). |
| What are the properties of a strong base? | High pH, low pOH, high [OH⁻], high Kb, low pKb, low Ka, high pKa. |
| What are binary acids, and what is the trend in their strength? | Binary acids = hydrogen halides (HF, HCl, HBr, HI). Strength increases with atomic radius of the halide: HI > HBr > HCl >> HF. HF is a weak acid; the others are strong. |
| Why is HF a weak acid despite being a binary acid? | 1) F⁻ is small and cannot stabilize negative charge well, making HF less likely to donate its proton. (2) The H−F intramolecular bond is stronger than in larger halides. |
| What are oxoacids, and what determines their strength? | Oxoacids contain oxygen. Strength increases with more oxygen atoms (more resonance stabilization of conjugate base) and with greater electronegativity of the central atom (for same number of oxygens). Example: H₂SO₄ > H₂SO₃; HClO₄ > HBrO₄ > HIO₄. |
| What are the strong acids to memorize? | HCl, HBr, HI, HNO₃, HClO₄, HClO₃, H₂SO₄. |
| What are the strong bases to memorize? | LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)₂, Sr(OH)₂, Ba(OH)₂. |
| What is a neutralization reaction and what is its formula? | Strong acid + strong base → salt + water. Formula: M₁V₁ = M₂V₂ (adjust for polyprotic acids/bases). |
| What type of salt is produced by strong acid + strong base, strong acid + weak base, and weak acid + strong base? | Strong + strong → neutral salt. Strong acid + weak base → acidic salt. Weak acid + strong base → basic salt. |
| How do you identify whether a salt is acidic, basic, or neutral? | Split the salt into its ions, then add H⁺ or OH⁻ to reconstruct the parent acid and base. Compare their strengths to determine the salt's nature. |
| What is a buffer solution and what is it made of? | A solution that resists pH changes when acid or base is added. Made of a weak acid/base and its conjugate base/acid, ideally in a 1:1 ratio. |
| How does a buffer resist pH changes? | When strong acid is added, the conjugate base neutralizes it. When strong base is added, the weak acid neutralizes it. |
| What are the six ways to make a buffer solution? | Acidic buffers: (1) weak acid + conj base salt 1:1, (2) weak acid + strong base 2:1, (3) conj base salt + strong acid 2:1. Alkaline buffers: (4) weak base + conj acid salt 1:1, (5) weak base + strong acid 2:1, (6) conjugate acid salt + strong base 2:1. |
| What is the buffering range of a buffer? | A buffer is effective within ±1 pH unit of its pKa. |
| What is a titration and what are its key components? | An experiment to find the unknown concentration of an acid/base. Titrant (known concentration, in burette) is added to analyte (unknown, in Erlenmeyer flask). An indicator signals the endpoint. |
| What is the equivalence point? | The point where moles of H⁺ = moles of OH⁻. It is the steepest part of the titration curve. Formula: NtVt = NaVa (where N = normality = M × n). |
| What is the pH at the equivalence point for each type of titration? | Strong acid + strong base → pH = 7. Strong acid + weak base → pH < 7. Weak acid + strong base → pH > 7. |
| What is a pH indicator and how do you choose one? | A weak acid/base that changes color between its protonated and deprotonated forms. Choose an indicator whose pKa is close to the pH of the equivalence point. |
| What is the half equivalence point? | Occurs at half the volume of the equivalence point, within the buffering region. At this point, pH = pKa, and [A⁻] = [HA]. |
| What are polyvalent titrations? | Titrations of polyprotic acids/bases (donate/accept >1 H⁺). The titration curve shows multiple buffering regions and multiple equivalence points — one per ionizable proton. |
| What are the useful logarithms to memorize for the OAT? | log(1) = 0, log(10) = 1, log(100) = 2. |
Created by:
smurtab