A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of...
A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77.
What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer? (Assume the addition cause negligible volume change.)
Homework Answers
The concept used here is based on the dissociation constant 
of an acid is used for the determination of the strength of an acid. Higher the value of dissociation constant, higher will be acid strength and vice versa.
The Henderson-Hasselbalch equation is used for the determination of the 
corresponding to the buffer solution. A buffer solution is basically composed of an acid and its corresponding conjugate base or vice versa.
The molarity of a solution is given as shown below.
…… (1)
Here,
is a number of moles of solute, is 
the volume of solution in liters.
The Henderson-Hasselbalch equation is given as shown below.
![salt]
pH= pK,+10 acid]](http://img.homeworklib.com/questions/b9e50080-498b-11ea-b3c7-bb326f2516ea.png?x-oss-process=image/resize,w_560)
…… (2)
Here, 
is the negative logarithm of the dissociation constant, ![[salt]](http://img.homeworklib.com/questions/ba9c1e10-498b-11ea-ba70-f906b0f1d13c.png?x-oss-process=image/resize,w_560)
is the concentration of salt and ![acid]](http://img.homeworklib.com/questions/baf26140-498b-11ea-897b-8d02ba45d985.png?x-oss-process=image/resize,w_560)
is the concentration of acid.
To calculate the moles of 
, substitute the value of 
as 
, 
as 
in the equation (1)
To calculate the moles of 
, substitute the value of as , as 
in the equation (1)
The Henderson-Hasselbalch equation for the solution can be written as shown below using equation (2).
![pH - pк, + log HСOONa]
PH - рк, + 1og (HСООН]
[НСООН]](http://img.homeworklib.com/questions/beb2fd50-498b-11ea-9fee-2bb1f5916b19.png?x-oss-process=image/resize,w_560)
Now, substitute the value of 
as 
, ![[НCООН]](http://img.homeworklib.com/questions/bfa0f940-498b-11ea-b858-f533070ac9be.png?x-oss-process=image/resize,w_560)
as 
and 
as in the above equation
The chemical equation after the addition of sodium hydroxide can be written as shown below.
To calculate the concentration of 
substitute 
as 
and 
as 
in the equation (1).
To calculate the concentration of 
substitute as 
and as 
in the equation (1).
The Henderson-Hasselbalch equation for the solution can be written as shown below using equation (2).
Now, substitute the value of 
as , as 
and as 
in the above equation.
The 
of the solution after the addition of 
sodium hydroxide is 
.
The 
of the solution after the addition of 
sodium hydroxide is 
.
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