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What is the buffer capacity if 3 moles are added in 5 litres of the solution to change the pH by 2 units?
- a)0.2
- b)0.5
- c)0.15
- d)0.3
Correct answer is option 'D'. Can you explain this answer?
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What is the buffer capacity if 3 moles are added in 5 litres of the so...
Buffer capacity is a measure of the ability of a buffer solution to resist changes in pH when an acid or base is added. It is defined as the amount of acid or base that can be added to a buffer solution without causing a significant change in pH.
To calculate the buffer capacity, we need to use the Henderson-Hasselbalch equation, which relates the pH of a buffer solution to the concentration of the acid and its conjugate base:
pH = pKa + log([A-]/[HA])
Where:
- pH is the desired change in pH (in this case, 2 units)
- pKa is the negative logarithm of the acid dissociation constant, which is a measure of the strength of the acid
- [A-] is the concentration of the conjugate base
- [HA] is the concentration of the acid
In this case, 3 moles of acid are added to a 5 liter solution. We can assume that the acid and its conjugate base are present in equimolar amounts, so the concentration of the acid and the conjugate base is 3 moles/5 liters = 0.6 M.
Let's assume the pKa of the acid is 4. We can now substitute these values into the Henderson-Hasselbalch equation:
pH = 4 + log(0.6/0.6) = 4 + log(1) = 4
Since the pH does not change when 3 moles of acid are added to the solution, the buffer capacity is equal to the amount of acid added, which is 3 moles.
Therefore, the correct answer is option D: 0.3.
To calculate the buffer capacity, we need to use the Henderson-Hasselbalch equation, which relates the pH of a buffer solution to the concentration of the acid and its conjugate base:
pH = pKa + log([A-]/[HA])
Where:
- pH is the desired change in pH (in this case, 2 units)
- pKa is the negative logarithm of the acid dissociation constant, which is a measure of the strength of the acid
- [A-] is the concentration of the conjugate base
- [HA] is the concentration of the acid
In this case, 3 moles of acid are added to a 5 liter solution. We can assume that the acid and its conjugate base are present in equimolar amounts, so the concentration of the acid and the conjugate base is 3 moles/5 liters = 0.6 M.
Let's assume the pKa of the acid is 4. We can now substitute these values into the Henderson-Hasselbalch equation:
pH = 4 + log(0.6/0.6) = 4 + log(1) = 4
Since the pH does not change when 3 moles of acid are added to the solution, the buffer capacity is equal to the amount of acid added, which is 3 moles.
Therefore, the correct answer is option D: 0.3.
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What is the buffer capacity if 3 moles are added in 5 litres of the so...
Buffer capacity is defined as the number of moles of acid or base added in one litre of the solution to change the pH by Unity. Therefore here buffer capacity = 3/5 divided by 2 = 0.6/2 = 0.3. The buffer capacity is given as 0.3.
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What is the buffer capacity if 3 moles are added in 5 litres of the solution to change the pH by 2 units?a)0.2b)0.5c)0.15d)0.3Correct answer is option 'D'. Can you explain this answer?
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