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

Use

Specification

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.
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
        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).
        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.
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;

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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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