Calculating the pH of buffer solutions

Last updated: 11/02/2020
AQA A-Level Chemistry Acids and bases Calculating the pH of buffer solutions
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  1. What is the definition of a buffer solution?

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  2. What is the aim of a buffer?

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  3. What part of a buffer solution controls the pH?

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  4. Which of the following is a method used to create an acidic buffer solution?

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  5. Which of the following is a method used to create an acidic buffer solution?

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  6. What happens to the pH of a buffer solution when a small amount of acid is added?

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  7. What happens to the pH of a buffer solution when a small amount of alkali is added?

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  8. When calculating the pH of an acidic buffer, which of the following assumptions must be made?

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  9. When calculating the pH of an acidic buffer, which of the following assumptions must be made?

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  10. What happens to the concentration of H+^+ ions when small amounts of acid is added to a buffer solution?

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  11. When a small amount of acid is added to a buffer solution there is an excess of H+^+ ions, what happens to the excess H+^+ ions?

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  12. How does the equilibrium change when a small amount of acid is added to a buffer solution?

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  13. When a small amount of acid is added to a buffer solution there is an excess of hydrogen ions, how does the buffer solution respond to this?

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  14. What happens to the concentration of OH−^- ions when small amounts of alkali is added to a buffer solution?

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  15. When a small amount of alkali is added to a buffer solution the concentration of hydroxide ions increases, what happens to the hydroxide ions?

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  16. When a small amount of alkali is added to a buffer solution what compound is formed?

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  17. How does the equilibrium change when a small amount of alkali is added to a buffer solution?

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  18. What process, carried out by the human body, allows the buffer system to control the pH levels in the blood?

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  19. Give one example where a buffer solution is used.

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  20. In order to control the pH of blood, what buffer system should be used?

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