Concept explainers
(a)
Interpretation:
The
Concept Introduction:
Buffer:
An aqueous solution of mixture of weak acid and its salt, or weak base and its conjugate acid solution is called “buffer”. It is resistant to change in
Acid Buffer:
A mixture of weak acid and its corresponding salt solution is called “Acidic Buffer”.
Base Buffer:
A mixture weak base and its corresponding salt solution forms a buffer is called “Basic Buffer”.
(a)
Explanation of Solution
The Henderson-Hassel batch equation for buffer is given by,
In the case of acidic buffer,
Therefore, the above equation becomes,
The dissociation reaction for the given Phosphorous acid is given by,
Concentration of starting phosphorous acid solution,
The equilibrium constant and its values as follows:
Finally,
Calculation for pH:
Therefore, the pH of the initial solution is 1.89
(b)
Interpretation:
The
(b)
Explanation of Solution
The reaction between phosphorous acid and NaOH is as follows:
The total number of moles of
The
From the above calculations, the remaining number of moles of
Total volume of the solution is 0.055L
Calculation for remaining concentration of
Calculation for remaining concentration of
Number of moles of Arsenic acid in the starting solution can be calculated as follows,
Number of moles =
The expression for equilibrium constant and its value as follows,
Thus, ‘x’ is the equilibrium concentration of
Calculation for pH:
Therefore, pH of the solution is 1.96
(c)
Interpretation:
The
(c)
Explanation of Solution
Total number of moles of
After addition of NaOH, the total number of moles of
Calculation for remaining moles of
Total volume of the solution is 0.060L. The concentration will be
Thus the
The dissociation concentration of phosphorous acid is small, so the second dissociation is ignored. Calculate the
Calculation for pH:
Therefore, pH of the solution is 11.6
Conclusion:
The
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Chapter 6 Solutions
EBK CHEMICAL PRINCIPLES
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