If pK_(a) of value of acid is 6.4, then what should be the ratio between salt to acid concentration to prepared a buffer solution of pH = 5.4?
Correct answer: B. 1 : 10
- A. 1 : 1
- B. 1 : 10
- C. 10 : 1
- D. 1 : 2
Explanation
To determine the ratio of salt to acid concentration for the buffer solution, apply the Henderson-Hasselbalch equation: pH = pKa + log([Salt]/[Acid]). Given pH = 5.4 and pKa = 6.4, subtracting gives: 5.4 = 6.4 + log([Salt]/[Acid]) -1 = log([Salt]/[Acid]). Solving for the ratio: [Salt]/[Acid] = 10-1 = 1/10, or 1:10. Therefore, the correct ratio is 1:10, which supports the buffer solution at a pH of 5.4. The other options either suggest equal concentrations or incorrect ratios that would not achieve the desired pH.
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About Acids, Bases and Salts
Acid and base behaviour is explained through the Bronsted-Lowry transfer of protons and the Lewis donation or acceptance of electron pairs. The topic includes pH, pOH, ionisation and water equilibrium, plus salt formation and hydrolysis, where a salt solution may become acidic, basic or neutral.
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