Find out and list as much information as possible about a weak acid from experimental results shown.
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On the acid trail
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Creative Problem Solving in Chemistry - On the acid trail
Specification
- Northern Ireland
- Republic of Ireland
- Scotland
- Wales
- A/AS level
- WJEC Chemistry
- Unit 3: PHYSICAL AND INORGANIC CHEMISTRY
- 3.9 Acid-base equilibria
- (b) differences in behaviour between strong and weak acids and bases in terms of the acid dissociation constant, Ka
- (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
- (e) shapes of the titration curves for strong acid/strong base, strong acid/weak base, weak acid/strong base and weak acid/weak base systems
- 3.9 Acid-base equilibria
- Unit 3: PHYSICAL AND INORGANIC CHEMISTRY
- WJEC Chemistry
- A/AS level
- England
- A/AS level
- AQA Chemistry
- Edexcel Chemistry
- Topic 12: Acid-base equilibria
- 2. know that acid-base reactions involve the transfer of protons
- 4. be able to define the term ‘pH’
- 5. be able to calculate pH from hydrogen ion concentration
- 6. be able to calculate the concentration of hydrogen ions, in mol dm⁻³, in a solution from its pH, using the expression [H⁺] = 10⁻ᵖᴴ
- 7. understand the difference between a strong acid and a weak acid in terms of degree of dissociation
- 9. be able to deduce the expression for the acid dissociation constant, Ka, for a weak acid and carry out relevant calculations
- 10. be able to calculate the pH of a weak acid making relevant assumptions
- 13. be able to define the terms ‘pKa’ and ‘pKw’
- 15. be able to calculate Ka for a weak acid from experimental data given the pH of a solution containing a known mass of acid
- 16. be able to draw and interpret titration curves using all combinations of strong and weak monobasic acids and bases
- 19. understand the action of a buffer solution
- 20. be able to calculate the pH of a buffer solution given appropriate data
- 22. understand how to use a weak acid–strong base titration curve to demonstrate buffer action, and determine Ka from the pH at the point where half the acid is neutralised
- Topic 12: Acid-base equilibria
- OCR Chemistry A
- Module 5: Physical chemistry and transition elements
- 5.1 Rates, equilibrium and pH
- 5.1.3 Acids, bases and buffers
- ci) the acid dissociation constant, Ka, for the extent of acid dissociation
- cii) the relationship between Ka and pKa
- d) use of the expression for pH as: pH = –log[H⁺]; [H⁺] = 10⁻ᵖᴴ
- g) calculations of pH, Ka or related quantities, for a weak monobasic acid using approximations
- h) limitations of using approximations to Ka related calculations for ‘stronger’ weak acids
- l) calculation of the pH of a buffer solution, from the Ka value of a weak acid and the equilibrium concentrations of the conjugate acid–base pair; calculations of related quantities
- 5.1.3 Acids, bases and buffers
- 5.1 Rates, equilibrium and pH
- Module 5: Physical chemistry and transition elements
- A/AS level
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