For a solution that e 0.275M
(a)
Interpretation:
A solution consists propionic acid,
Concept introduction:
The concentration of any solution is calculated by the molarity of the solution. It is defined as the number of moles of solute in 1 L of the solution.
Here, n is number of moles of solute and V is volume of solution in L.
The dissociation constant of the weak acid is calculated by the following formula-
The expression can be written as follows:
Answer to Problem 1E
The concentration of
Explanation of Solution
The complete dissociation of strong acid occurs in the solution, whereas weak acid is not able to dissociate completely.
From the given information,
Propionic acid,
The molarity of propionic acid
Hydroiodic acid, HI = strong acid
The molarity of [HI] or [H3O+] ion = 0.0892 M
The chemical equation of this reaction is given below:
Now, the concentration will be calculated by using the following ICE table:
Initial (I) | 0.275 | - | 0 | 0.0892 |
Change (C) | - x | - | + x | + x |
Equilibrium (E) | 0.275- x | - | x | 0.0892+ x |
Given that-
Ka = 1.3×10-5
The equation for the Ka is as follows:
Put the given values in equation (1).
On calculation −
Now, the concentration of
(b)
Interpretation:
A solution consists propionic acid,
Concept introduction:
The concentration of any solution is calculated by the molarity of the solution. It is defined as the number of moles of solute in 1 L of the solution.
Here, n is number of moles of solute and V is volume of solution in L.
The dissociation constant of the weak acid is calculated by the following formula:
The expression can be written as follows:
The relation between the dissociation constant of acid and the base is given by the following equation-
Here,
Answer to Problem 1E
The concentration of
Explanation of Solution
The chemical equation of this reaction is given below:
The concentration of
Given that-
And,
Put the above values in equation (1)
(c)
Interpretation:
A solution consists propionic acid,
Concept introduction:
The concentration of any solution is calculated by the molarity of the solution. It is defined as the number of moles of solute in 1 L of the solution.
Here, n is number of moles of solute and V is volume of solution in L.
The dissociation constant of the weak acid is calculated by the following formula:
The expression can be written as follows:
Answer to Problem 1E
The concentration of
Explanation of Solution
The chemical equation of this reaction is given below:
Now, the concentration will be calculated by using the following ICE table:
Initial (I) | 0.275 | - | 0 | 0.0892 |
Change (C) | -x | - | +x | +x |
Equilibrium (E) | 0.275-x | - | x | 0.0892+x |
From the ICE table:
Ka = 1.3×10-5
The equation for the Ka is given as
Put the given values in equation (1).
On calculation −
Therefore,
(d)
Interpretation:
A solution consists propionic acid,
Concept introduction:
The dissociation constant of the weak acid is calculated by the following formula:
The expression can be written as follows:
The strong acid dissociates completely in comparison to the weak acid.
Answer to Problem 1E
The concentration of [HI] = 0.0892 M.
Explanation of Solution
The complete dissociation of strong acid occurs in the solution, whereas weak acid is not able to dissociate completely.
From the given question −
Hydroiodic acid, HI = strong acid
The molarity of [HI] or [H3O+] ion = 0.0892 M
As hydroiodic acid is strong acid it will dissociate completely in the solution. Hence, the initial concentration of [HI] = 0.0892 M.
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