Aqueous solutions of methanoic acid, HCOOH , and propanoic acid, $$\(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH}\)$$, are mixed together. An equilibrium is set up between two conjugate acid-base pairs. (i) Define conjugate acid-base pair. (ii) The $$\(\mathrm{p} K_{\mathrm{a}}\)$$ of HCOOH is 3.75 and of $$\(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH}\)$$ is 4.87 . Complete the equation for the Brønsted-Lowry equilibrium between the stronger of these two acids and water.
Exam No：9701_s24_qp_42 Year：2024 Question No：6
Answer:
Knowledge points:
25.1.1 understand and use the terms conjugate acid and conjugate base
25.1.10.1 understand and use the common ion effect to explain the different solubility of a compound in a solution containing a common ion
25.1.10.2 perform calculations using values and concentration of a common ion
25.1.2 define conjugate acid–base pairs, identifying such pairs in reactions
25.1.3 define mathematically the terms pH, use them in calculations and the equation will not be tested)
25.1.4.1 strong acids
25.1.4.2 strong alkalis
25.1.4.3 weak acids
25.1.5.1 define a buffer solution
25.1.5.2 explain how a buffer solution can be made
25.1.5.3 explain how buffer solutions control pH; use chemical equations in these explanations
25.1.5.4 describe and explain the uses of buffer solutions, including the role of in controlling pH in blood
25.1.6 calculate the pH of buffer solutions, given appropriate data
25.1.7 understand and use the term solubility product
25.1.8 write an expression for
25.1.9 calculate from concentrations and vice versa
Solution:
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