A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO.
What is the pH of this buffer? Ka
= 1.7
The concept used to solve this problem is based on buffer solutions.
The pH of an acidic buffer solution is determined with the help of Henderson-Hasselbalch equation.
Buffer solutions are those which resists change in its pH when a small amount of an acid or a base are added to it. The Henderson-Hasselbalch equation is shown as follows:
Here, is concentration of salt and concentration of weak acid.
The dissociation of the acid is shown as follows:
Now, convert volume into liters as follows:
Now, total volume is calculated as follows:
Substitute for and 1.00 L for .
Now calculate the concentration in terms of molarity as follows:
And,
Now, Henderson-Hasselbalch equation is as follows:
Substitute 3.77 for , 0.125 for and 1 for .
Ans:The pH of the given buffer is 2.87.
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