{
  "id": "50b9556c-7164-5571-a321-426b46c920bb",
  "slug": "r3-1-proton-transfer-reactions-hl",
  "title": "R3.1 Proton transfer reactions (HL)",
  "course": "IB Chemistry",
  "level": "HL",
  "syllabusCode": "R3.1",
  "questionCount": 15,
  "page": "https://splycr.com/ib-chemistry/r3-1-proton-transfer-reactions-hl",
  "data": "https://splycr.com/library/r3-1-proton-transfer-reactions-hl.json",
  "play": "https://splycr.com/?set=50b9556c-7164-5571-a321-426b46c920bb",
  "section": {
    "name": "Reactivity 3: What are the mechanisms of chemical change?",
    "page": "https://splycr.com/ib-chemistry/mechanisms-of-chemical-change"
  },
  "source": {
    "name": "Biology by Bradford",
    "href": "https://www.biologybybradford.com",
    "note": "Written for the splycr library by Biology by Bradford."
  },
  "questions": [
    {
      "number": 1,
      "question": "pOH of a solution with pH 3 at 298 K?",
      "answer": "11",
      "wrongOptions": [
        "3",
        "7",
        "17"
      ]
    },
    {
      "number": 2,
      "question": "Expression for Ka of a weak acid HA?",
      "answer": "[H⁺][A⁻]/[HA]",
      "wrongOptions": [
        "[HA]/[H⁺][A⁻]",
        "[H⁺][A⁻]",
        "[H⁺]²/[A⁻]"
      ]
    },
    {
      "number": 3,
      "question": "Expression for Kb of ammonia?",
      "answer": "[NH₄⁺][OH⁻]/[NH₃]",
      "wrongOptions": [
        "[NH₃]/[NH₄⁺][OH⁻]",
        "[NH₄⁺][OH⁻]",
        "[NH₃][H⁺]/[NH₄⁺]"
      ]
    },
    {
      "number": 4,
      "question": "pKa is defined as…?",
      "answer": "−log Ka",
      "wrongOptions": [
        "log Ka",
        "1/Ka",
        "−ln Ka"
      ]
    },
    {
      "number": 5,
      "question": "Of two weak acids, the stronger one has the…pKa?",
      "answer": "Smaller",
      "wrongOptions": [
        "Larger",
        "Equal",
        "Zero"
      ]
    },
    {
      "number": 6,
      "question": "Ka × Kb for a conjugate acid–base pair equals…?",
      "answer": "Kw",
      "wrongOptions": [
        "1.0",
        "Ka²",
        "pKw"
      ]
    },
    {
      "number": 7,
      "question": "pKa + pKb for a conjugate acid–base pair at 298 K?",
      "answer": "14",
      "wrongOptions": [
        "7",
        "0",
        "28"
      ]
    },
    {
      "number": 8,
      "question": "pH of 0.10 mol dm⁻³ weak acid with Ka = 1.0 × 10⁻⁵?",
      "answer": "3",
      "wrongOptions": [
        "1",
        "5",
        "6"
      ]
    },
    {
      "number": 9,
      "question": "At the half-equivalence point of a weak acid–strong base titration, pH equals…?",
      "answer": "pKa",
      "wrongOptions": [
        "pKb",
        "pKw",
        "pOH"
      ]
    },
    {
      "number": 10,
      "question": "pH at the equivalence point of a weak acid–strong base titration?",
      "answer": "Above 7",
      "wrongOptions": [
        "Below 7",
        "Exactly 7",
        "Exactly 14"
      ]
    },
    {
      "number": 11,
      "question": "pH of aqueous ammonium chloride at 298 K is…?",
      "answer": "Below 7",
      "wrongOptions": [
        "Above 7",
        "Exactly 7",
        "Exactly 0"
      ]
    },
    {
      "number": 12,
      "question": "Suitable indicator for a weak acid–strong base titration?",
      "answer": "Phenolphthalein",
      "wrongOptions": [
        "Methyl orange",
        "Bromophenol blue",
        "Methyl red"
      ]
    },
    {
      "number": 13,
      "question": "Solution that resists pH change when small amounts of acid or base are added?",
      "answer": "Buffer",
      "wrongOptions": [
        "Indicator",
        "Titrant",
        "Standard solution"
      ]
    },
    {
      "number": 14,
      "question": "Pair of substances that forms an acidic buffer?",
      "answer": "CH₃COOH and CH₃COONa",
      "wrongOptions": [
        "HCl and NaCl",
        "NaOH and NaCl",
        "HCl and CH₃COOH"
      ]
    },
    {
      "number": 15,
      "question": "pH of a buffer with [A⁻]/[HA] = 10 and pKa = 4.0?",
      "answer": "5.0",
      "wrongOptions": [
        "3.0",
        "4.0",
        "14.0"
      ]
    }
  ]
}