Creative Problem Solving in Chemistry: H⁺ ions in water

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Estimate the number of H⁺(aq) ions in a single drop of: water; 1.0 mol dm^-3 HCl; 1.0 mol dm^-3 NaOH.

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H⁺ ions in water
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Level

16-18 years

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Specification

Northern Ireland
- A/AS level
  - CCEA Chemistry
    - Unit A2 1: Further Physical and Organic Chemistry
      - 4.5 Acid-base equilibria
        4.5.3 carry out calculations involving pH for strong acids, strong bases and weak acids;
Wales
- A/AS level
  - WJEC Chemistry
    - Unit 3: PHYSICAL AND INORGANIC CHEMISTRY
      - 3.9 Acid-base equilibria
        (d) how to use pH, Kw, Ka and pKa in calculations involving strong and weak acids and pH and Kw in calculations involving strong bases
Republic of Ireland
- Leaving Certificate
  - Chemistry
    - 9. Environmental chemistry: water
      - 9.1 pH Scale
        Depth of treatment
        Self-ionisation of water, Kw;
        pH scale. Use of universal indicator paper or solution. Limitations of the pH scale - usefulness confined to dilute aqueous solutions.
        pH of weak acids and bases.
        Activities
        Calculation of pH of dilute aqueous solutions of strong acids and bases (calculation of pH of mixtures of strong acids and bases not required).
England
- A/AS level
Scotland
- National 5
  - SQA Chemistry
    - Chemical changes and structure
      - Acids and bases
        pH
        The pH scale is an indication of the hydrogen ion concentration and runs from below 0 to above 14.
        Water is neutral as it dissociates according to the equation 2H₂O (l) ⇌ H⁺ (aq) + OH⁻ (aq) producing equal concentrations of hydrogen and hydroxide ions. At any time, only a few water molecules are dissociated into free ions
        Acidic solutions have a higher concentration of H⁺(aq) ions than OH⁻(aq) and have a pH below 7.
        Alkaline solutions have a higher concentration of OH⁻(aq) ions than H⁺(aq) ions and have a pH above 7.

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Creative Problem Solving in Chemistry: H⁺ ions in water

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H⁺ ions in water

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